Answer:
The temperature will be 137 K for the gas pressure to remain constant
Explanation:
If the gas pressure keeps on constant, volume of the gas will be modified according to temperature.
V1 / T1 = V2 / T2
4L / 274K = 2L / T2
(4L / 274K) . T2 = 2L
T2 = 2L . (274K / 4L)
T2 = 137K
The mechanism for producing a concentrated urine involves all of the following except
The mechanisms for producing concentrated urine are countercurrent multiplication, ADH secretion, and osmoregulation. Excretion of excess water is not involved.
In the production of concentrated urine, all of the following mechanisms are involved:
Countercurrent multiplication: This process occurs in the loop of Henle and helps to establish a concentration gradient in the medulla of the kidney. ADH secretion: Antidiuretic hormone (ADH) is released by the pituitary gland, which increases the permeability of the collecting ducts to water. Osmoregulation: The kidneys regulate the concentration of solutes in the urine through the reabsorption and secretion of various substances.
The mechanism that is not involved in producing concentrated urine is the excretion of excess water.
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In producing a concentrated urine, the kidney uses several mechanisms including high NaCl concentration, ADH secretion, aquaporin insertion and facultative water reabsorption, but not obligatory water reabsorption in the proximal convoluted tubule. therefore, option D is correct
Explanation:The key mechanism for producing concentrated urine in the kidney involves several steps, but the option D, obligatory water reabsorption in the proximal convoluted tubule, does not directly contribute to the urine's concentration. This obligatory water reabsorption happens regardless of your body's state of hydration, and it reabsorbs about 70% of the water from the urine before it reaches the section of the kidney where the urine's concentration is adjusted. The other options - a high concentration of NaCl in the interstitial fluid, secretion of ADH, insertion of aquaporins, and increase in facultative water reabsorption - are all steps which allow the regulation of the urine's concentration depending on the body's need to retain or expel water.
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the complete Question is given below
The mechanism which the kidney uses to produce a concentrated urine involves all of the following EXCEPT
A. a high concentration of NaCl in the interstitial fluid that surrounds the collecting ducts.
B. secretion of ADH by the posterior pituitary gland.
C, aquaporins being inserted into the membranes of the collecting duct cells.
D. obligatory water reabsorption in the proximal convoluted tubule.
E. an increase in facultative water reabsorption.
how is temperature a factor in cloud seeding
Explanation:
In order for water to condense from vapor to liquid, the temperature of the air must be at or below the dew point, and there must be condensation nuclei present. The seeding provides the nuclei, but the air temperature must also be below the temperature at which the air is saturated with water vapor.
A container holds oxygen, hydrogen and nitrogen gas. The nitrogen gas has a partial pressure of 0.88 atm, while occupying 15% of the container’s volume. If the oxygen gas occupies 57% of the container’s volume, what is the partial pressure of the hydrogen gas in the container? a. 0.88 atm b. 1.64 atm c. 3.34 atm
Answer:
The partial pressure of hydrogen gas = 1.64 atm
Explanation:
Step 1: Data given
partial pressure of nitrogen = 0.88 atm
Nitrogen occupies 15% of the volume (Let's assume the volume is 1L)
Oxygen gas occupies 57 % of the volume
Step 2: Calculate % volume of hydrogen
100 % - 15% - 57 % = 28 %
Step 2:
P1/V1 = P2/V2
⇒ with p1 = the partial pressure of nitrogen = 0.88 atm
⇒ with V1 = the volme occupied by nitrogen = 15% ( assume 0.15 L)
⇒ with P2 = the partial pressure of hydrogen = TO BE DETERMINED
⇒ with V2 = the volume occupied by hydrogen = 28 % = 0.28 L
0.88/ 0.15 = X/0.28
X = 1.64 atm
The partial pressure of hydrogen gas = 1.64 atm
The enthalpy of combustion of lactose, C12H22O11, is -5652 kJ/mol. A 2.50 g sample of lactose was burned in a calorimeter that contained 1350 g of water. The heat capacity of the calorimeter is 1630 J/oC, and the initial temperature was 24.58oC. What was the final temperature(oC)?
Answer:
30.25°C
Explanation:
The calorimeter is an equipment used to measure the combustion enthalpy of a substance. The heat loss in the reaction is used to heat the water and the equipment. By the conservation of energy:
Qcombustion + Qcalorimeter + Qwater = 0
Because there is no phase change:
Qcalorimeter = C*ΔT, where C is the heat capacity, and ΔT the variation in temperature (final - initial)
Qwater = m*c*ΔT, where m is the mass, and c is the specific heat (4.184 J/g°C).
The molar mass of lactose is 342.3 g/mol, so the number of moles in 2.50 g is:
n = mass/molar mass
n = 2.50/342.3
n = 0.0073 mol
Qcombustion = -5652 kJ/mol * 0.0073 mol
Qcombustion = -41.28 kJ
Qcombustion = - 41280 J
Thus,
-41280 + 1630*(T - 24.58) + 1350*4.184*(T - 24.58) = 0
(T - 24.58) * (1630 + 5648.4) = 41280
7278.4(T - 24.58) = 41280
T - 24.58 = 5.67
T = 30.25°C
The student needs to calculate the final temperature of water in a calorimeter after lactose combustion by using the initial temperature, lactose's enthalpy of combustion, and heat released by the combustion is absorbed by the water and calorimeter, raising their temperature.
The student wants to calculate the final temperature of water in a calorimeter after burning a 2.50 g sample of lactose with an enthalpy of combustion of -5652 kJ/mol. To solve this, we need to find the amount of heat absorbed by the water and calorimeter, which can be calculated using the specific heat capacities of water and the calorimeter and the mass of the water.
First, the number of moles of lactose combusted is found by dividing the mass in grams (2.50 g) by the molar mass of lactose ($C_{12}H_{22}O_{11}$). Then, the total heat released by the combustion of lactose is calculated by multiplying the number of moles by the enthalpy of combustion. Since the heat of combustion is expressed in kJ/mol, and the heat capacity of the calorimeter is in J/°C, we must ensure our units are consistent when calculating the energy absorbed by the water and calorimeter. The final temperature is obtained by adding the temperature change to the initial temperature of 24.58°C.
Calculate moles of lactose: 2.50 g / (342.30 g/mol) - molar mass of lactose.Calculate total heat released: Moles of lactose x -5652 kJ/mol.Convert kJ to J for consistency.Calculate the temperature change: Heat released / (heat capacity of water + calorimeter).Find final temperature: Initial temperature + temperature change.Given the initial temperature and the enthalpy of combustion of lactose, the final temperature can be found after determining the heat transferred to the water and calorimeter.
Which of the following techniques is most appropriate for the recovery of solid KNO3 from an aqueous solution of KNO3?A. Paper chromatographyB. FiltrationC. TitrationD. ElectrolysisE. Evaporation to dryness
Answer:
E. Evaporation to dryness
Explanation:
E. - Evaporation to dryness is the best method for the recovery of solid KNO3 from an aqueous solution of KNO3.
(KNO3 is very soluble, and will violently decompose if overheated.)
Paper chromatography is for separation of different weight molecules in solution.
B. Filtration won't work on a solution
C.Titration would contaminate the salt with something else and is used
to determine concentrations
D. Electrolysis would destroy the salt
Answer:
E
Explanation:
Which statements are correct relative to carbohydrates?
a.only source of fuel quick source of energy consists of carbon,
b.hydrogen and nitrogen polymers formed by hydrolysis most are monosaccharides
Answer:
Hi, the statements given in the question (a and b) are combination of right and wrong answers. But i will split the statement a and b into necessary fragments.
Carbohydrates are quick source of energy relatively. That is the only correct statement in the question.
Explanation:
Carbohydrates are naturally occurring organic compounds containing carbon, hydrogen and oxygen with the general formula (Cx H2y Oy) or Cx (H2O)y. They can be classified into simple sugar or complex sugar.
Simple sugars can be further divided into Monosaccharides (e.g glucose, fructose and galactose) and Disaccharides (e.g sucrose and maltose).
Complex sugar can be referred to as Polysaccharides (e.g cellulose and starch)
The statement above that says carbohydrate contains carbon, hydrogen and nitrogen polymers is not correct.
Carbohydrates are not mostly monosaccharides. They also contain Disaccharides and Polysaccharides.
They are not the only source of fuel.
Answer:
quick source of energy
most are monosaccharides
Explanation:
YW!
What is true for all exergonic reactions?
Answer:
The reaction proceeds with a net release of free energy.
Explanation:
Exergonic reactions: It is known as the chemical reaction where the change in the free energy is occur negative or there is a net release of free energy, and indicating a spontaneous reaction. For the processes this takes place under constant temperature, and pressure conditions.
The Gibbs free energy is used whereas the processes which takes place under constant volume, and temperature conditions, and their Helmholtz energy is used. Cellular respiration is the example of an exergonic reaction.
A gas-filled weather balloon with a volume of 65.0 L is released at sea level where conditions are745 torr and 25 ºC. The balloon can expand to a maximum volume of 835 L. When the balloon rises to an altitude at which the temperature is –5 ºC and the pressure is 0.066 atm, will it have exceeded its maximum volume?
Answer:
It will reach to its maximum volume.
Explanation:
Using Ideal gas equation for same mole of gas as :-
[tex] \frac {{P_1}\times {V_1}}{T_1}=\frac {{P_2}\times {V_2}}{T_2}[/tex]
Given ,
V₁ = 65.0 mL
V₂ = ?
P₁ = 745 torr
The conversion of P(torr) to P(atm) is shown below:
[tex]P(torr)=\frac {1}{760}\times P(atm)[/tex]
So,
Pressure = 745 / 760 atm = 0.9803 atm
P₁ = 0.9803 atm
P₂ = 0.066 atm
T₁ = 25 ºC
T₂ = -5 ºC
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (25 + 273.15) K = 298.15 K
T₂ = (-5 + 273.15) K = 268.15 K
Using above equation as:
[tex] \frac {{P_1}\times {V_1}}{T_1}=\frac {{P_2}\times {V_2}}{T_2}[/tex]
[tex] \frac{{0.9803}\times {65.0}}{298.15}=\frac{{0.066}\times {V_2}}{268.15}[/tex]
Solving for V₂ as:-
[tex]V_2=\frac{0.9803\times \:65.0\times 268.15}{298.15\times 0.066}[/tex]
[tex]V_2=\frac{17086.38392}{19.6779}[/tex]
V₂ = 868 L
Given that:- V max = 835 L
Thus, it will reach to its maximum volume.
The following questions pertain to a system contains 122 g CO(g) in a 0.400 L container at -71.2 degrees C.
a.Calculate the pressure exerted by the CO(g) in this system using the ideal gas equation.
b.The actual pressure exerted by the carbon monoxide was found to be 145 atm. Explain why the actual pressure is less than what would be expected?
Answer:
a. P = 182 atm
b. due to daviation from ideal gas behavior
Explanation:
Data Given:
amount of CO = 122g
Volume of CO = .400 L
Temperature of CO = -71.2°C
Convert the temperature to Kelvin
T = °C + 273
T = -71.2 + 273
T = 201.8 K
a. Calculate the pressure exerted by the CO(g) in this system using the ideal gas equation (P) = ?
Solution:
To calculate Pressure by using ideal gas formula
PV = nRT
Rearrange the equation for Pressure
P = nRT / V . . . . . . . . . (1)
where
P = pressure
V = Volume
T= Temperature
n = Number of moles
R = ideal gas constant = 0.08206 L.atm / mol. K
For this we have to know the mole of the gas and the following formula will be used
no. of moles = mass in grams / molar mass . . . . . . (2)
Molar mass of CO = 12 + 16 = 28 g/mol
Put values in equation 2
no. of moles = 122 g / 28 g/mol
no. of moles = 4.4 mol
Now put the value in formula (1) to calculate Pressure for CO
P = 4.4 x 201.8 K x 0.08206 (L.atm/mol. K) / 0.400 L
P = 182 atm
So the pressure will be 182 atm
__________
b. Data Given:
Actual pressure exerted by CO = 145 atm
expected pressure exerted by CO = 182 atm
why the actual pressure is less than what would be expected = ?
Explanation:
This is because of the deviation from ideal behavior of real gases.
The real gases approaches to ideal behavior under very high temperature and very low pressure.
But CO deviate from ideal behavior to give expected value for pressure, because it behave at high pressure and low temperature.
This non-ideal behavior is due to two postulate of ideal behavior
• gas molecules have negligible volume
• Gas molecules have negligible inter-molecular interaction
but these postulates not obeyed under real condition. so we calculated the pressure using ideal condition values for gas and obtained the expected value for pressure but the actual pressure value was detected under normal condition.
Hydrogen bonds between water molecules are responsible for the unique chemical and physical properties of water. True False
Answer:
True
Explanation:
The physical and chemical properties of a substance depend on the nature of intermolecular forces between its molecules. For instance, water has a high boiling point because of hydrogen bonding between water molecules. Liquid water is denser than ice because of the difference in the nature of hydrogen bonding in liquid water and ice.
Final answer:
Hydrogen bonds between water molecules are responsible for the unique chemical and physical properties of water. - True
Explanation:
Hydrogen bonds are a type of intermolecular force that naturally occurs between water molecules when the positive hydrogen end of one molecule is attracted to the negative oxygen end of another molecule. These bonds significantly impact water's physical properties.
For instance, they are why water remains liquid over a wide range of temperatures, why water has a high boiling point relative to its molecular weight, and why it is known as the universal solvent. In short, hydrogen bonding is essential for the many unique properties of water that are crucial for life on Earth.
The pK of acetic acid is pK = 4.76. For a 0.1 M solution of acetic acid at a pH = 4.76 what is the concentration of [H+]?
Answer:
[H+] = 1.74 x 10⁻⁵
Explanation:
By definition pH = -log [H+]
Therefore, given the pH, all we have to do is solve algebraically for [H+] :
[H+] = antilog ( -pH ) = 10^-4.76 = 1.74 x 10⁻⁵
Final answer:
The concentration of [H+] in a 0.1 M solution of acetic acid at a pH of 4.76 is 1.32 × 10^-3 M.
Explanation:
The concentration of [H+] in a 0.1 M solution of acetic acid at a pH of 4.76 can be calculated using the equation Ka = [H+][CH3COO-]/[CH3COOH]. Since the pK of acetic acid is 4.76, it means that at this pH, [H+] will be equal to [CH3COO-]. Substituting the values, we get [H+] = [CH3COO-] = 1.32 × 10^-3 M. Therefore, the concentration of [H+] in the solution is 1.32 × 10^-3 M.
4.0 L of He(g), 6.0 L of N2(g), and 10. L of Ar(g), all at 0°C and 1.0 atm, are pumped into an evacuated 8.0 L rigid container, the final pressure in the container at 0°C is
Answer:
The final pressure in the container at 0°C is 2.49 atm
Explanation:
We apply the Ideal Gases law to know the global pressure.
We need to know, the moles of each:
P He . V He = moles of He . R . 273K
(1atm . 4L) / R . 273K = moles of He → 0.178 moles
P N₂ . V N₂ = moles of N₂ . R . 273K
(1atm . 6L) / R . 273K = moles of N₂ → 0.268 moles
P Ar . V Ar = moles of Ar . R . 273K
(1atm . 10L) / R . 273K = moles of Ar → 0.446 moles
Total moles: 0.892 moles
P . 8L = 0.892 mol . R . 273K
P = ( 0.892 . R . 273K) / 8L = 2.49 atm
R = 0.082 L.atm/mol.K
The final pressure in the evacuation container at 0 °C is 2.499 atm
To solve this question, we'll begin by calculating the number of mole of each gas. This can be obtained as follow:
For He:Volume (V) = 4 L
Pressure (P) = 1 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Temperature (T) = 0 °C = 273 K
Number of mole (n) =? PV = nRT1 × 4 = n × 0.0821 × 273
4 = n × 22.4133
Divide both side by 22.4133
n = 4 / 22.4133
n = 0.178 mole For N₂:Volume (V) = 6 L
Pressure (P) = 1 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Temperature (T) = 0 °C = 273 K
Number of mole (n) =? PV = nRT1 × 6 = n × 0.0821 × 273
6 = n × 22.4133
Divide both side by 22.4133
n = 6 / 22.4133
n = 0.268 mole For Ar:Volume (V) = 10 L
Pressure (P) = 1 atm
Gas constant (R) = 0.0821 atm.L/Kmol
Temperature (T) = 0 °C = 273 K
Number of mole (n) =?PV = nRT
1 × 10 = n × 0.0821 × 273
10 = n × 22.4133
Divide both side by 22.4133
n = 10 / 22.4133
n = 0.446 moleNext, we shall determine the total moles of the gas in the container.
Mole of He = 0.178 mole
Mole of N₂ = 0.268 mole
Mole of Ar = 0.446 mole
Total mole =?Total mole = 0.178 + 0.268 + 0.446
Total mole = 0.892 moleFinally, we shall determine the pressure in evacuation container. This can be obtained as follow:
Volume (V) = 8 L
Gas constant (R) = 0.0821 atm.L/Kmol
Temperature (T) = 0 °C = 273 K
Number of mole (n) = 0.892 mole
Pressure (P) =? PV = nRTP × 8 = 0.892 × 0.0821 × 273
P × 8 = 19.993
Divide both side by 8
P = 19.993 / 8
P = 2.499 atmTherefore, the final pressure in the evacuation container at 0 °C is 2.499 atm
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Because metallic bonds permit one plane of ions to slide past another without breaking bonds, metals are:_______
A. brittle.
B. nonreflective.
C. malleable.
D. poor conductors of electricity.
Answer:
D. poor conductors of electricity.
Explanation:
Because metallic bonds permit one plane of ions to slide past another without breaking bonds, metals are poor conductors of electricity. Therefore, option D is correct.
What are metals ?A metal is a substance that exhibits a shiny appearance when freshly processed, polished, or shattered, and conducts electricity and heat rather well. Generally speaking, metals are malleable and ductile. These characteristics are the outcome of the metallic link that exists between the metal's atoms or molecules.
Ferrous metals, which include iron, and non-ferrous metals, which do not, are the two basic categories into which metals can be separated. Iron-based metals. Pure iron is too soft and ductile to be much use as an engineering material.
Metals have high melting and boiling temperatures because they have massive lattice structures and must break a huge number of electrostatic forces.
Thus, option D is correct.
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If 4.00 moles of oxygen gas, 3.00 moles of hydrogen gas, and 1.00 mole of nitrogen gas are combined in a closed container at standard pressure, what is the partial pressure exerted by the hydrogen gas?
Answer:
Partial pressure of H₂ is 0.375 atm
Explanation:
We apply the mole fraction to solve this.
Standard pressure is 1 atm
Mole fraction of a gas = Moles of gas / Total moles
Mole fraction of pressure = Partial pressure of gas / Total pressure
Both values are the same
Total moles = 4 moles of O₂ + 3 moles of H₂ and 1 mol of N₂ = 8 moles
3 moles H₂ / 8 moles = Partial pressure H₂ / 1 atm
(3 / 8 ) .1 = 0.375 atm → Partial pressure of H₂
The partial pressure exerted by the hydrogen gas, H₂ in the container is 0.375 atm
We'll begin by calculating the mole fraction of H₂ in the gas mixture. this can be obtained as follow:
Mole of O₂ = 4 moles
Mole of H₂ = 3 moles
Mole of N₂ = 1 mole
Total mole = 4 + 3 + 1 = 8 moles
Mole fraction of H₂ = ?[tex]mole \: fraction \: = \frac{mole \: of \: gas}{total \: mole} \\ \\ = \frac{3}{8} \\ \\ [/tex]
Mole fraction of H₂ = 0.375 Finally, we shall determine the partial pressure of H₂ .This can be obtained as illustrated below:Mole fraction of H₂ = 0.375
Total pressure = STP = 1 atm
Partial pressure of H₂ = ?Partial pressure = mole fraction × Total Pressure
Partial pressure of H₂ = 0.375 × 1
Partial pressure of H₂ = 0.375 atmTherefore, the partial pressure of H₂ in the container is 0.375 atm
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In the reaction of silver nitrate with sodium chloride, how many grams of silver chloride will be produced from 100. g of silver nitrate when it is mixed with an excess of sodium chloride? The equation for the reaction is below. AgNO3(aq)+ NaCl(aq) → AgCl(s) + NaNO3(aq)
Answer:
85g
Explanation:
Firstly, from the balanced equation, we can see that one mole of silver nitrate yielded one mole of silver chloride. This is the theoretical relation. We need to get the actual relation. To do this, we will first need to get the number of moles of silver nitrate.
The number of moles is the mass of silver nitrate divided by the molar mass of silver nitrate. The molar mass of silver nitrate is 108 + 14 + 3(16) = 108 + 14 + 48 = 170g/mol
The number of moles is thus 100/170 = 0.59 moles
Since the mole ratio is 1 to 1, the number of moles of silver chloride produced too is 0.59 moles.
To get the mass of silver chloride produced, we simply multiply the number of moles of silver chloride by the molar mass of silver chloride. The molar mass of silver chloride is 108 + 35.5 = 143.5g/mol
The mass is thus = 143.5 * 0.59 = 84.67g
Iridium is a component of cosmic dust that rains down upon the earth at a constant rate. Why did Luis Alvarez suggest measuring iridium levels in the K-T boundary?
Answer:
In order to determine the rate at which the sediment layers were deposited
Explanation:
Iridium is an important element that belongs to the Platinum group and they are dominantly present in the asteroids and comets. They are the key evidence that suggests the occurrence of an asteroidal impact or a mass extinction event that has taken place in the geological past.
The presence of Iridium mixed with the clay sediments in the boundary between the Cretaceous and Tertiary (K-T boundary) suggested the mass extinction event that wiped out numerous life forms from the earth.
The famous scientist Dr. Luis Walter Alvarez suggested measuring the concentration of Iridium in this K-T boundary in order to determine the rate at which these sediment layers were deposited. They were able to determine that these Iridium elements were present due to the asteroid impact on earth, that wiped out the dinosaurs from the earth. They also considered that this element can be produced from the eruptions of volcanoes.
Answer:
The presence of Iridium mixed with the clay sediments in the boundary between the Cretaceous and Tertiary (K-T boundary) suggested the mass extinction event that wiped out numerous life forms from the earth.
The famous scientist Dr. Luis Walter Alvarez suggested measuring the concentration of Iridium in this K-T boundary in order to determine the rate at which these sediment layers were deposited. They were able to determine that these Iridium elements were present due to the asteroid impact on earth, that wiped out the dinosaurs from the earth. They also considered that this element can be produced from the eruptions of volcanoes.
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Explanation:Iridium is a component of cosmic dust that rains down upon the earth at a constant rate. Why did Luis Alvarez suggest measuring iridium levels in the K-T boundary?
Which two properties are characteristic of ionic compounds?
brittleness
ductility
high melting point
low boiling point
malleability
Answer:
Options A and C
Explanation:
In chemistry, an ionic compound is a chemical compound composed of ions held together by electrostatic forces termed ionic bonding. The compound is neutral overall, but consists of positively charged ions called cations and negatively charged ions called anions.
Option A - This is correct because In ionic compounds, electrons are tightly held by the ions, and the ions cannot move translationally relative to each other. This explains many properties of ionic solids. They are hard and brittle.
Option B and E - This is incorrect. Due to the electrons being tightly held and the ions not being able to move translationally, they are not malleable or ductile (i.e. cannot be shaped without cracking/breaking).
Option C - Ionic compounds have high melting points because there is a strong electrostatic force of attraction between the oppositely charged ions and hence a large amount of energy is required to break the strong bonding force between ions. This option is correct.
Option D - Ionic cmpounds have High Boiling point so this option is wrong.
Thermal decomposition of sodium azide (NaN₃) into nitrogen gas and sodium metal is used to inflate car airbags. The reaction proceeds by the following chemical reaction.
2NaN₃(s)⟶3N₂(g)+2Na(s)
How many grams of NaN₃ are need to inflate a 10.00L airbag with nitrogen gas at 1.000 atm and 273.15 K assuming ideal gas behavior?
Answer:
19.5g
Explanation:
Firstly, we can use the ideal gas equation to calculate the number of moles of nitrogen gas needed.
We use the following formula:
PV = nRT
n = PV/RT
In the question, we were given:
P = 1 atm
V = 10L
T = 273.15k
R = molar gas constant= 0.082L.atm/mol.k
Let us insert these values into the ideal gas equation.
n = (1 * 10)/(273.15 * 0.082) = 0.45moles
The number of moles of nitrogen required is 0.45 moles
From the balanced reaction equation, we can see that 2 moles of sodium azide yielded 3 moles of Nitrogen.
Hence the number of moles of sodium azide produced from 0.45 moles of nitrogen would be : (0.45 * 2)/3 = 0.3mole
To get the mass of sodium azide needed, we simply multiply the number of moles of sodium azide by the molar mass of sodium azide. We know the number of moles but we do not know the molar mass. The molar mass of sodium azide is 23 + 3(14) = 23 + 42 = 65g/mol
The mass = 65 * 0.3 = 19.5g
The mass of azide required is 19.3 g.
The equation of the reaction is given as; 2NaN₃(s)⟶3N₂(g)+2Na(s)
We have to obtain the number of moles of the nitrogen gas from;
P = 1.000 atm
V = 10.00L
T= 273.15 K
R = 0.082 atm L K-1mol-1
n = PV/RT
n = 1.000 atm × 10.00L/0.082 atm L K-1mol-1 × 273.15 K
n = 0.446 moles
Now;
2 moles of azide yields 3 moles of nitrogen
x moles of azide yieilds 0.446 moles of nitrogen
x = 2 moles × 0.446 moles/3 moles
x = 0.297 moles
Mass of azide required= 0.297 moles × 65 g/mol = 19.3 g
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Magnesium reacts with oxygen gas to form magnesium oxide. Which of the following represents the balanced chemical equation?
Mg + O2 --> MgO
Mg + O2 --> 2MgO
2Mg + 2O2 --> 2MgO
2Mg + O2 --> 2MgO
Answer:
2Mg + O2 → 2MgO
Explanation:
Step 1: Data given
Magnesium = Mg
Oxygen = O2
magnesiumoxide = MgO
Step 2: The unbalanced equation
Mg + O2 → MgO
Step 3: Balancing the equation
On the left we have 2x O so on there right, we should mulitply MgO by 2 so we have on each side 2x O
Mg + O2 → 2MgO
On hte right side we have 2x Mg, so we have to multiply on the left side Mg by 2 to have the same amount of Mg on both sides
2Mg + O2 → 2MgO
Now the equation is balanced
The balanced chemical equation for magnesium reacting with oxygen to form magnesium oxide is 2Mg + O2 → 2MgO.
Explanation:Magnesium reacts with oxygen gas to form magnesium oxide, and the balanced chemical equation that represents this reaction is 2Mg + O2 → 2MgO. In this reaction, magnesium (Mg) is oxidized, and oxygen (O2) is reduced. Magnesium, being a highly reactive metal, combines with oxygen to produce magnesium oxide, where two atoms of magnesium react with one molecule of oxygen to yield two formula units of magnesium oxide.
A sound wave traveling through a certain freshwater lake has a frequency of 349.2 Hz and a wavelength of 4.25 m. What is the speed of a sound wave in this water?
To calculate the speed of sound in a freshwater lake, use the formula Speed of sound = Frequency x Wavelength. Given a frequency of 349.2 Hz and a wavelength of 4.25 m, the speed of sound in the water is 1483.7 m/s.
Speed of sound = Frequency x Wavelength
Given Frequency = 349.2 Hz, Wavelength = 4.25 m
Speed of sound = 349.2 Hz x 4.25 m = 1483.7 m/s
What is the total number of grams of H20 produced when 116 grams of the product, Naci, is formed?
A) 36 9g
B) 54 9
C) 18 g
D) 9.0 g
Answer:
A) 36 g
Explanation:
From the source, some values have been correct.
Given that;-
Mass of NaCl formed = 116 grams
Molar mass of NaCl = 58 g/mol
Moles of NaCl = [tex]\frac{Mass}{Molar\ mass}=\frac{116}{58}\ mol=2\ mol[/tex]
According to the reaction shown below:-
[tex]HCl+NaOH\rightarrow NaCl+H_2O[/tex]
1 mole of NaCl and 1 mole of [tex]H_2O[/tex] are produced upon reaction.
So,
2 moles of NaCl and 2 moles of [tex]H_2O[/tex] are produced upon reaction.
Moles of water = 2 moles
Molar mass of water = 18 g/mol
Mass = [tex]Moles\times Molar\ mass=2\times 18\ g=36\ g[/tex]
36 g of [tex]H_2O[/tex] is produced.
how many grams of turpentine are consumed to produce 569g of carbon with C10H16+_8Cl=10C+16HCl
Answer:
644.2918 g of turpentine are consumed.
Explanation:
Calculation of the moles of [tex]C[/tex] as:-
Mass = 569 g
Molar mass of carbon = 12.0107 g/mol
The formula for the calculation of moles is shown below:
[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]
Thus,
[tex]Moles= \frac{569\ g}{12.0107\ g/mol}[/tex]
[tex]Moles_{C}= 47.3744\ mol[/tex]
According to the given reaction:-
[tex]C_{10}H_{16}+8Cl_2\rightarrow 10C+16HCl[/tex]
10 moles of C are produced when 1 mole of turpentine undergoes reaction
1 mole of C are produced when [tex]\frac{1}{10}[/tex] mole of turpentine undergoes reaction
47.3744 moles of C are produced when [tex]\frac{1}{10}\times 47.3744[/tex] moles of turpentine undergoes reaction
Moles of turpentine = 4.73744 moles
Molar mass of turpentine = 136 g/mol
[tex]Mass=Moles\times Molar\ mass=4.73744\ moles\times 136\ g/mol=644.2918\ g[/tex]
644.2918 g of turpentine are consumed.
Diets high in trans and what other type of fatty acid contribute to chronic diseases, including heart disease and cancer?
Answer: Saturated Fatty Acids
Explanation: Saturated fats are one's in which fatty Acids chains
Largely or totally contains a single bond. Most animal fats contains high proportion of Saturated Fatty acid such as milk, cheese and butter. Foods like pizza, sausage also have high proportion of Saturated Fatty acid.
Three 1.0L flasks, maintained at 308K are connected to each other with stopcocks. Initially, the stopcocks are closed: One of the flasks contains 1.0atm N2, the second 2.0g of H2O and the third, 0.50g ethanol, C2H6O. The vapor pressure of H2O at 308K is 24mmHG and that of ethanol is 102mmHG. The stopcocks are then opened and the contents mix freely. What is the pressure of the system after mixing? Please give all work including a description of each step.
Answer:
Pt = 0.392 atm
Explanation:
First, we must separate the initial condition for each gas:
- N₂ :
V₁ = 1 Lt , T₁ = 308 K , P₁ = 1 atm
- H₂O :
V₂= 1 Lt , T₂= 308 K, P₂= 24 mm Hg = 0.032 atm
- C₂H₆O:
V₃= 1 Lt, T₂= 308 K, P₃= 102 mm Hg = 0.134 atm
For this case, we consider that 1 atm = 760 mm Hg
We then calculate the number of moles for each case (in gas phase), and we consider that al gasses behave like an ideal gas:
PV = nRT we consider R = 0.082 Lt*atm/K*mol
- N₂ :
n H₂ = PV/RT = 1x1/0.082x308 = 0.04
- H₂O:
n H₂O = PV/RT = 0.032x1/0.082x308 = 1.27x10⁻³
- C₂H₆O:
n C₂H₆O = PV/RT = 0.134x1/0.082x308 = 5.31x10⁻³
Finally, when the stopcocks are open and the 3 gases are mixed together, T will remain as 308 K, total volume will be the volume of the three flasks (3 Lt), so total pressure (Pt) after mixing the 3 gases will be:
Pt = (n N₂ + n H₂O + n C₂H₆O)xRT/V = (0.04658x0.082x308)/3
Pt = 0.392 atm
Which of the following correctly provides the name of the element, the symbol for the ion, and the name of the ion?a) fluorine, F, fluoride ionb) sulfur, S, sulfurous ionc) copper, Cu, cuprous iond) zinc, Zn, zincate ion
The element with the correct symbol for the ion, and the name of the ion has been fluorine, [tex]\rm F^-[/tex], Fluoride. ion. The correct option is a.
The elements tend to attain the stable electronic configuration and acquire the noble gas configuration. The elements gain electrons and acquire a -ve charge while losing electrons attain a +ve charge onto the element.
The IUPAC nomenclature gives the addition '-ide' as a suffix to the metal losing electrons.
The fluorine has been a halogen losing an electron, the symbol is [tex]\rm F^-[/tex], and symbolized as Fluoride.Sulfur has been a nonmetal. and loses 2 electrons. The symbol has been [tex]\rm S^2^-[/tex], and the name has been Sulfide.
Copper has been a transition metal that loses one electron to form [tex]\rm Cu^+[/tex], and the ion has been cupric ion.
Zinc ion loses electron and form [tex]\rm Zn^2^+[/tex], the ion has been zinc ion.
Thus, the element with the correct symbol for the ion, and the name of the ion has been fluorine, [tex]\rm F^-[/tex], Fluoride. ion. The correct option is a.
For more information about ions, refer to the link:
https://brainly.com/question/12843101
Two samples of Mg(s) of equal mass were placed in equal amounts of HCl(aq) contained in two separate reaction vessels. Particle representations of mixing of Mg(s) and HCl(aq) in the two reaction vessels are shown in Figure 1 and 2 above. Water molecules are not included in the particle representations. Which of the reactions will initially proceed faster and why?
Explanation:
The two figures are missing so I can't tell which reactions will proceed faster, but the answer will follow this logic:
If the two samples of Mg(s) are equal, the two amounts of HCl(aq) are equal, the operation conditions are the same (Temperature, pressure,etc.), the difference in the speed of reaction will only depend difference in the quality of mixing of the Mg(s).
Being that said:
If the particles of Mg are poorly distributed in the solution and very close to each other, the surface that interacts with HCl is small and in result the speed of reaction is lower. On the other hand, if the Mg is well mixed and its concentration is almost homogeneous in all the solution, the surface of reaction will be bigger and the speed of reaction higher than the other case.Which of the following represents the ground state electron configuration for the Mn3+ ion? (Atomic number Mn = 25) 1s2 2s22p6 3s23p63d4
Answer:
[tex]1s^22s^22p^63s^23p^63d^{4}[/tex]
Explanation:
Manganese is the element of group 7 and forth period. The atomic number of Manganese is 25 and the symbol of the element is Mn.
The electronic configuration of the element, manganese is -
[tex]1s^22s^22p^63s^23p^63d^{5}4s^2[/tex]
To form [tex]Mn^{3+}[/tex], it will lose 3 electrons from the valence electrons and thus the configuration of the ion is:-
[tex]1s^22s^22p^63s^23p^63d^{4}[/tex]
The ground state electron configuration for the Mn3+ ion is 1s2 2s2 2p6 3s2 3p6 3d4 after removing three electrons from the highest energy orbitals, which are the 4s and 3d in the case of manganese.
Explanation:The ground state electron configuration for the Mn3+ ion starts with the neutral manganese atom, which has an atomic number of 25. The neutral Mn atom would have an electron configuration of 1s2 2s2 2p6 3s2 3p6 3d5 4s2. However, for Mn3+, three electrons are removed to account for the +3 charge, typically from the outermost orbitals first which in this case are the 4s and 3d orbitals. Since the 4s electrons are generally removed before the 3d electrons, after losing two electrons from 4s and one electron from 3d, the configuration will be 1s2 2s2 2p6 3s2 3p6 3d4.
PLEASE HELP & SHOW WORK
i will really really appreciate it, i am stuck!!
1) 5 grams of N2 -----> mol N2
2) 4.0*10^23 molecules of N2 to atoms of N
3) 1.2 mol N2 to molecules of N2
4) How much does 4.5*10^24 atoms of carbon weigh? (you are looking for grams)
5) Number of atoms in 1.3g of NaCl
6) Number of molecules of water (H20) in 500mL
Answer:
1. 0.178 moles ; 2. 8x10²³ atoms ; 3. 7.22x10²³ molecules ; 4. 89.6 g ; 5. 1.34x10²² atoms ; 6. 1.67x10²⁵ molecules
Explanation:
1. Mass / Molar mass = Mol
5g / 28 g/m = 0.178 moles
2. 1 molecule of N₂ has 2 atoms, it is a dyatomic molecule.
4x10²³ x2 = 8x10²³ atoms
3. 1 mol of anything, has 6.02x10²³ particles
6.02x10²³ molecules . 1.2 mol = 7.22x10²³
4. 1 atom of C weighs 12 amu.
4.5x10²⁴ weigh ( 4.5x10²⁴ . 12) = 5.24x10²⁵ amu
1 amu = 1.66054x10⁻²⁴g
5.24x10²⁵ amu = (5.24x10²⁵ . 1.66054x10⁻²⁴) = 89.6 g
5. Molar mass NaCl = 58.45 g/m
1.3 g / 58.45 g/m = 0.0222 moles
1 mol has 6.02x10²³ atoms
0.0222 moles → ( 0.0222 . 6.02x10²³) = 1.34x10²²
6. Density of water is 1 g/mL, so 500 mL are contained in 500 g of water
Molar mass H₂O = 18 g/m
500 g / 18 g/m = 27.8 moles
6.02x10²³ molecules . 27.8 moles = 1.67x10²⁵
Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate how much remains after 36 L of H2 reacts with 12 L of CS2. 4H2(g) + CS2(g) → CH4(g) + 2H2S(g)
Answer:
There will be produced 9L of CH4 and 18 L of H2S. There will remain 3 L of CS2
Explanation:
Step 1: Data given
volume of H2 = 36.00 L
volume of CS2 = 12 L
Step 2 = the balanced equation
4H2(g) + CS2(g) → CH4(g) + 2H2S(g)
Step 3: Calculate number of moles of H2
1 mol = 22.4 L
36 L = 1.607 mol
Step 4: Calculate moles of CS2
1 mol = 22.4 L
12 L = 0.5357 moles
Step 5: Calculate the limiting reactant
For 4 moles of H2 we need 1 mol of CS2 to produce 1 mol of CH4 and 2 moles of H2S
H2 is the limiting reactant. It will completely be consumed. ( 1.607 moles)
CS2 is in excess. There will react 1.607/4 = 0.40175 moles
There will remain 0.5357 - 0.40175 = 0.13395 moles of CS2
0.13395 moles of CS2 = 3 L
Step 6: Calculate products
For 4 moles of H2 we need 1 mol of CS2 to produce 1 mol of CH4 and 2 moles of H2S
For 1.607 moles of H2 we'll have 0.40175 moles of CH4 (= 9L) and 0.8035 moles of H2S =(18L)
There will be produced 9L of CH4 and 18 L of H2S. There will remain 3 L of CS2
What element has 5 occupied principal energy levels
Answer:
Group 3-12 transition metals has 5 occupied principal energy levels
Explanation:
The group 3-12 transition metal includes rubidium, strontium, yttrium, zirconium, niobium, molybdenum, technetium, ruthenium, rhodium, palladium, silver, cadmium, indium, tin, antimony, tellurium, iodine, xenon. The elements can also go beyond the 5th principal energy level. The filling of the orbital always depends on the atomic number of the atom. The orbitals filled with the electrons in the ascending order of the energy of the orbitals. The starting element of the period of the the periodic table shows the new principal energy level.