List and describe the steps of the scientific method.
What is the change in energy if the electron from part a now drops to the ground state?what is the wavelength λ of the photon that has been released in part b?
The change in energy when the electron drops to the ground state can be calculated. The wavelength of the released photon can be determined using the equation: wavelength = hc / energy.
Explanation:When an electron drops from a higher energy level to the ground state, it releases energy in the form of a photon. The change in energy can be calculated by taking the difference between the initial energy and the energy of the ground state. The wavelength of the photon can be determined using the equation:
wavelength = hc / energy
where h is Planck's constant (6.626 x 10^-34 J s), c is the speed of light (3.00 x 10^8 m/s), and energy is the change in energy calculated earlier.
Typically, water runs through the baseboard copper tubing and, therefore, fresh hot water is constantly running through the piping. However, consider a pipe where water was allowed to sit in the pipe. The hot water cools as it sits in the pipe. What is the temprature change, (ΔT), of the water if 190.0 g of water sat in the copper pipe from part A, releasing 2284 J of energy to the pipe? The specific heat of water is 4.184 (J/g)⋅∘C
The temperature change (ΔT) of the water after sitting in the copper pipe can be found using the formula for heat transfer (q = mcΔT), considering that the water releases 2284 J of energy. Thus, ΔT = 2284 / (190.0 * 4.184).
Explanation:The temperature change of water in the copper pipe can be determined by using the formula for heat transfer (q = mcΔT), where q is heat in joules, m is the mass in grams, c is the specific heat capacity, and ΔT is the temperature change in degrees Celsius. Here, the initial temperature of the water is not given, but we know that the water releases 2284 J of energy. Plugging in the mass (190.0 g), the specific heat of water (4.184 J/g °C), and the heat (2284 J) into the formula, we get the equation
2284 = 190 * 4.184 * ΔT.
Solving for ΔT, we get ΔT = 2284 / (190.0 * 4.184), which should provide the temperature change of the water after sitting in the copper pipe.
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What are groups 1, 2, and 3 examples of on a periodic table of elements?
A) Metals
B) Nonmetals
C) Metalloids
D) Noble gass
Answer:
A) Metals
Explanation: They mainly explain metals in "periodic table" well it's in it too.
The boiling point of a liquid is 64 °c and the enthalpy change for the conversion of this liquid to the gas is 32.21 kj/mole. what is the entropy change for vaporization, δsvap?
Entropy change of vaporization is simply the ratio of enthalpy change and the temperature in Kelvin.
Temperature = 64 + 273.15 = 337.15 K
Hence,
δsvap = (32.21 kJ / mole) / 337.15 K
δsvap = 0.0955 kJ / mole K = 95.5 J / mole K
Answer:
[tex]\Delta S_{vap}=0.096\frac{kJ}{mol*K} =96\frac{J}{mol*K}[/tex]
Explanation:
Hello,
In this case, the entropy of vaporization (conversion from liquid to gas) is mathematically defined in terms of enthalpy and the boiling temperature in K as shown below:
[tex]\Delta S_{vap}=\frac{\Delta H_{vap}}{T_b}[/tex]
Thus, for the given data we obtain:
[tex]\Delta S_{vap}=\frac{32.21kJ/mol}{(64+273.15)K} \\\\\Delta S_{vap}=0.096\frac{kJ}{mol*K} =96\frac{J}{mol*K}[/tex]
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what is the molar mass of potassium
94.0, is the answer for sure
What would you predict is worse based on your knowledge of quantum theory - a weak beam of ultraviolet light, or an intense beam of infrared light?
Answer : Amongst the given choices a weak beam of ultraviolet light is considered to be the worst as compared to others.
The wavelength of UV light is from 10 nm to 400 nm, and its energy varies from 3 eV to 124 eV.
As a single beam of UV light will have much energy in each photon which is emitted. The damage done by UV rays is observed to be very harmful in human cells and may cause many diseases. UV rays can also damage the eyes as more than 99% of UV radiation is absorbed by the front of the eyes. It can also lead to ultimate blindness. Therefore, it is considered to be much worse than an intense beam of infrared light.
How many atoms are in 80.16g of calcium?
Using the mass of a proton 1.0073 amu and assuming it's diameter is1.0x10^-15, calculate the density of a proton in g/cm^3. I'm not sure about how to convert amu to grams. Thanksfor the help!!
What happens if you cool the crystallization solution in a container of ice that is too big?
Based on the answers to parts (a)-(c), explain why cinnamaldehyde is not miscible with water. incorporate relevant intermolecular forces in your answer.
The combination of a single polar group and dominant non-polar regions prevents effective hydrogen bonding with water, leading to the immiscibility of cinnamaldehyde in water.
**Structure:**
O
|
C=CH-CH=CH-CH2-CH2-CH3
|
H
**Analysis:**
a) **Non-polar regions:**
* **Double bonds:** The double bonds (C=C) have evenly distributed electron density, making them non-polar. Circle both double bonds.
* **Alkyl chains:** The aliphatic chains (CH2-CH2-CH3) also have similar electron densities across their C-H bonds, making them non-polar. Circle both alkyl chains.
b) **Polar region:**
* **Carbonyl group (C=O):** The carbonyl group has a significant dipole moment due to the electronegativity difference between oxygen and carbon. This creates a partial positive charge on the carbon and a partial negative charge on the oxygen. Circle the carbonyl group (C=O).
c) **Water's preferred intermolecular force:**
* **Hydrogen bonding:** Water molecules are highly polar due to their lone pairs and O-H bonds, enabling strong hydrogen bonding with other polar molecules.
d) **Cinnamaldehyde's immiscibility with water:**
* Although the carbonyl group is polar, its interaction with water is significantly weakened by the extensive non-polar regions (double bonds and alkyl chains) dominating the molecule.
* These non-polar regions prefer London dispersion forces (weak attractive forces between all molecules due to temporary fluctuations in electron density) over the stronger hydrogen bonding with water.
* The weak London dispersion forces cannot overcome the stronger intermolecular hydrogen bonding network of water, resulting in immiscibility.
Therefore, the combination of a single polar group and dominant non-polar regions prevents effective hydrogen bonding with water, leading to the immiscibility of cinnamaldehyde in water.
The probable question may be:
1. Re-draw the chemical structure of cinnamaldehyde and use it to answer the following solubility-based questions:
a) Circle and label all regions of the molecule that exhibit non-polar behavior.
b) Circle and label the region of the molecule that exhibits polar behavior.
c) Water prefers to interact with solute molecules with what type of intermolecular force (choose one answer): hydrogen bonding, dipole- induced dipole, or induced dipole-induced dipole (London dispersion)?
d) Based on the answers to parts (a)-(c), explain why cinnamaldehyde is NOT miscible with water. Incorporate relevant intermolecular forces in your answer.
How do electrons differ from protons and neutrons?
A.
They do not move.
B.
They are larger.
C.
They are not in a fixed position.
D.
They are located in the nucleus
Answer:
Option c, They are not in a fixed position.
Explanation:
As per Bohr's model of atomic atoms,
Electrons revolve around around the nucleus in a fixed path or energy level. Electrons revolving in these energy levels do not radiate energy.
Therefore, electrons are not present in a fixed position. They present outside the nucleus.
Mass of protons and neutrons are same whereas electrons are smaller.
Among the given options, options c best describe the difference between electrons from protons and neutrons.
A teacher listed the following two processes. • Process 1: water changing to ice in a freezer • Process 2: steam coming out of a kettle filled with hot of water Which table correctly identifies the change of state taking place in each example?
Which element would release the most energy while adding an electron to a neutral atom in the gas phase?
For most compounds in which a nitrogen atom bears no formal charge, the valence of this nitrogen atom is
Answer:
3
Explanation:
Hello,
In this case, as nitrogen is not bearing any formal charge, we apply its mathematical definition to find such oxidation state:
Formal charge= # of valence electrons - # of lone-pair electrons - 1/2 # of bond pair electrons
Since no formal charge is born, no lone-pair electrons are formed and 6 bond pair electrons are always present for the nitrogen to complete the octate, the valence turns out into:
# of valence electrons = 0 + 0 + 1/2 * 6
# of valence electrons = 3
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Water is formed when two hydrogen atoms bond to an oxygen atom.
The hydrogen and the oxygen in this example are different
A) complexes.
B) compounds.
C) elements.
D) mixtures.
When solid potassium chlorate is heated, it decomposes to form solid potassium chloride and oxygen gas. express your answer as a balanced chemical equation. identify all of the phases in your answer?
Why are covalent bonds between hydrogen and nitrogen or oxygen polar? see section 2.1 ( page 57) ?
Remember to use the proper number of significant figures and leading zeros in all calculations. A sample has a mass of 35.4 g and a volume of 36.82 mL. What is the density of the sample?
1.04011 g/mL
1.04 g/mL
0.96143 g/mL
0.961g/mL
Answer : The correct option is, 0.961 g/ml
Solution : Given,
Mass of sample = 35.4 g
Volume of sample = 36.82 ml
Formula used :
[tex]\text{Density of sample}=\frac{\text{Mass of sample}}{\text{Volume of sample}}[/tex]
Now put all the given values in this formula, we get the density of the sample.
[tex]\text{Density of sample}=\frac{35.4g}{36.82ml}=0.961g/ml[/tex]
Therefore, the density of the sample is, 0.961 g/ml
Answer:
The correct option is, 0.961 g/ml
Explanation:
What is the atomic number of an element that has 43 protons and 50 neutrons?
A 10.0 gram piece of metal is placed in an insulated calorimeter containing 250.0 grams of water initially at 20.0°c. if the final temperature of the mixture is 25.0°c, what is the heat change of piece of metal? 5230 j â5230 j 209 j â209 j 5440 j
Write the symbol for the ion formed when each element gains electrons and attains a noble-gas electron configuration. Br, H, Se.
Explanation:
When an atom gain electrons then it acquires a negative charge whereas when an atom loses electrons then it acquires a positive charge.
For example, atomic number of bromine is 35 and its electronic distribution is 2, 8, 18, 7. So, in order to gain stability bromine accepts one electrons and thus it acquires a negative charge as [tex]Br^{-}[/tex].
Therefore, the symbol for the ion formed when each given element gains electrons and attains a noble-gas electron configuration are as follows.
Br changes into [tex]Br^{-}[/tex].H changes into [tex]H^{-}[/tex].Se changes into [tex]Se^{2-}[/tex].
What is the henry's law constant for co2 at 20∘c? express your answer to three significant figures and include the appropriate units?
The value of Henry’s law constant for [tex]{\text{C}}{{\text{O}}_{\text{2}}}[/tex] at [tex]20{\text{ }}^\circ {\text{C}}[/tex] is [tex]\boxed{3.70 \times {{10}^{ - 2}}{\text{ L}} \cdot {\text{atm}} \cdot {\text{mo}}{{\text{l}}^{ - 1}}}[/tex].
Further explanation:
Solubility
It is that property of substance by virtue of which it becomes able to dissolve in other substances. It is measured in terms of the maximum amount of solute that can be dissolved in the given amount of solvent.
Henry’s Law
According to this law, solubility of gas dissolved in the liquid is directly related to the partial pressure of gas. High partial pressure means high solubility and vice-versa.
Mathematically,
[tex]{{\text{S}}_{{\text{gas}}}} \propto {{\text{P}}_{{\text{gas}}}}[/tex] …… (1)
To remove the proportionality constant in equation (1), constant known as Henry’s constant is incorporated and equation (1) modifies to,
[tex]{{\text{S}}_{{\text{gas}}}} = {{\text{k}}_{\text{H}}}{\mathbf{ \times }}\;{{\text{P}}_{{\text{gas}}}}[/tex] …… (2)
Here,
[tex]{{\text{S}}_{{\text{gas}}}}[/tex] is the solubility of gas.
[tex]{{\text{k}}_{\text{H}}}[/tex] is Henry’s constant.
[tex]{{\text{P}}_{{\text{gas}}}}[/tex] is the pressure of gas.
Equation (2) can be rearranged in order to calculate Henry’s constant [tex]\left( {{{\text{k}}_{\text{H}}}} \right)[/tex] and equation (2) becomes,
[tex]{{\text{k}}_{\text{H}}} = \dfrac{{{{\text{S}}_{{\text{gas}}}}}}{{{{\text{P}}_{{\text{gas}}}}}}\;[/tex] …… (3)
At [tex]20{\text{ }}^\circ {\text{C}}[/tex] , the value of Henry’s law constant for [tex]{\text{C}}{{\text{O}}_{\text{2}}}[/tex] up to three significant figures is [tex]3.70 \times {10^{ - 2}}{\text{ L}} \cdot {\text{atm}} \cdot {\text{mo}}{{\text{l}}^{ - 1}}[/tex].
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What is the concentration of alcohol in terms of molarity? https://brainly.com/question/9013318 Determine whether solubility will increase, decrease or remains the same: https://brainly.com/question/2802008
Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: Solutions
Keywords: solubility, gas, Henry’s law, partial pressure, solubility, dissolve, CO2, three significant figures, [tex]3.70*10^-2 L atm/mol,[/tex] high partial pressure, high solubility.
The Henry's law constant for CO₂ at 20°C is 3.91 × 10⁻² M/atm. The pressure required to achieve a CO₂ concentration of 6.90 × 10⁻² M at 20°C is approximately 23.4 atm.
Part A - To answer the question, we need to understand that Henry's Law states that the concentration of a gas in a liquid is directly proportional to the partial pressure of that gas above the liquid. The law is represented by the equation:
C = kH * P
where C is the concentration of the gas, kH is the Henry's law constant, and P is the partial pressure of the gas.
Given that the Henry's law constant for CO₂ in water at 25°C is 3.4 × 10⁻² M/atm, we can use interpolated values to find the constant at 20°C. Experimentally, at 20°C, the Henry's law constant for CO₂ is found to be 3.91 × 10⁻² M/atm.
Therefore, the Henry's law constant for CO₂ at 20°C is 3.91 × 10⁻² M/atm.
Part B: Pressure Required for CO₂ Concentration
To find the pressure required to achieve a CO₂ concentration of 6.90 × 10⁻² M at 20°C, we can use Henry's Law:
pCO₂ = KH × [CO₂]
where pCO₂ is the partial pressure of CO₂, KH is the Henry's Law constant, and [CO₂] is the concentration of CO₂ in moles per liter.
Rearranging the equation to solve for pCO2:
pCO₂ = KH × [CO₂] = 3.39 × 10² L·atm/mol × 6.90 × 10⁻² mol/L ≈ 23.4 atm
So, the pressure required to achieve a CO₂ concentration of 6.90 × 10⁻² M at 20°C is approximately 23.4 atm.
Complete Question - Part A What is the Henry's law constant for CO₂ at 20°C? Express your answer to three significant figures and include the appropriate units. Part B What pressure is required to achieve CO₂ concentration of 6.90x10⁻² M at 20°C? Express your answer to three significant figures and include the appropriate units.
what type of equation is Cu + 2AgNO3=Cu(NO3)2 + 2Ag?
The given equation is a double-replacement reaction where solid copper reacts with an aqueous solution of silver nitrate to produce a solution of copper(II) nitrate and solid silver.
Explanation:The given equation is a chemical equation, specifically a double-replacement reaction. In this type of reaction, the cations are swapped between two compounds. In this case, solid copper (Cu) reacts with an aqueous solution of silver nitrate (AgNO3) to produce a solution of copper(II) nitrate (Cu(NO3)2) and solid silver (Ag). The balanced equation for this reaction is:
Cu + 2AgNO3 = Cu(NO3)2 + 2Ag
What kind of reaction adds water to break large molecules into subunits?
Complete and balance the molecular equation, including phases, for the reaction of aqueous iron(III) nitrate, Fe(NO3)3 and aqueous lithium hydroxide, LiOH.
The Complete balanced equation for the reaction of Aqueous iron (iii) nitrate, Fe(NO3)3 and aqueous lithium hydroxide, LiOH, is given by;
Fe(NO₃)₃(aq) + 3LiOH(aq) → 3LiNO₃(aq) + Fe(OH)₃(s)
Further Explanation:Chemical equations Chemical equations are equations showing reactions between reactants to form products. Chemical equations show the reactants or starting substances and products or substances formed during the reaction.Law of conservation of mass The law of conservation requires that when writing chemical equations, the mass of the reactants should be equal; to the mass of the products.This is done by making sure the number of atoms of each element involved in the chemical equation is equal on both sides of the equation.To ensure the law of conservation in chemical equations is observed we balance chemical equations.Balancing chemical equation:Balancing chemical equations is a try and error method that ensures the number of atoms in the side of the reactants is equal to the number of atoms in the side of products.Balancing chemical equations may also require inclusion of state symbols which shows the state of each compound or element involved in the chemical reactions.For example; the equation; Fe(NO₃)₃(aq) + 3LiOH(aq) → 3LiNO₃(aq) + Fe(OH)₃(s), is balanced as there are equal number of atoms of any given element on both sides; A single atom of Fe, six oxygen atom, 3 nitrogen atoms and 3 lithium atoms on both side of the equation.
Keywords: Chemical equations, balancing of chemical equations
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Subject: Chemistry
Topic: Chemical equations
Sub-topic: Balancing chemical equations
The balanced chemical equation between aqueous iron(III)nitrate and aqueous lithium hydroxide is Fe(NO₃)₃[tex]_(aq)[/tex] + 3 LiOH [tex]_(aq)[/tex][tex]\rightarrow[/tex] 3 LiNO₂ [tex]_(aq)[/tex] +Fe(OH)₃[tex]_(s)[/tex].
What is a chemical equation?Chemical equation is a symbolic representation of a chemical reaction which is written in the form of symbols and chemical formulas.The reactants are present on the left hand side while the products are present on the right hand side.
A plus sign is present between reactants and products if they are more than one in any case and an arrow is present pointing towards the product side which indicates the direction of the reaction .There are coefficients present next to the chemical symbols and formulas .
The first chemical equation was put forth by Jean Beguin in 1615.By making use of chemical equations the direction of reaction ,state of reactants and products can be stated. In the chemical equations even the temperature to be maintained and catalyst can be mentioned.
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Helium has a density of 1.79 x 10-4 g/mL at standard temperature and pressure. A balloon has a volume of 6.3 liters. Calculate the mass of helium that it would take to fill the balloon.
35,000 g
1.1 x 10-3 g
2.8 x 10-5 g
1.1 g
The mass of helium that it would take to fill the balloon is 1.1 grams.
What is the relation between mass and density?Relation between the mass of any substance and their density will be represented as:
Density = Mass / Volume
Given that,
Density of helium gas = 1.79 × 10⁻⁴ g/mL
Volume of balloon in which gas is present = 6.3L = 6300 mL
On putting all these values, we get
Mass = (1.79 × 10⁻⁴ g/mL)(6300mL) = 1.12 grams
Hence required mass of helium is 1.1 g.
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At what temperature does water evaporate?
Air is 21% oxygen by volume. Oxygen has a density of 1.31 g/L. What is the volume in liters of a room that holds enough air to contain 55kg of oxygen?
Answer:
199,927.29 L is the volume air that holds enough air to contain 55 kg of oxygen.
Explanation:
Density of oxygen = 1.31 g/L
Mass of oxygen gas,m = 55 kg = 55,000 g
Volume of the oxygen gas = V
Volume of the air = [tex]V_a[/tex]
[tex]Density=\frac{Mass}{Volume}[/tex]
[tex]1.31 g/L=\frac{55,000 g}{V}[/tex]
V = 41.984.732 L
Air is 21% oxygen by volume.That is in 100 L of air 21 L of oxygen is present.
So, when oxygen gas is 41.984.732 L the volume of the air will be:
[tex]21\%=\frac{41.984.732 L}{V_a}\times 100[/tex]
[tex]V_a=199,927.29 L[/tex]
199,927.29 L is the volume air that holds enough air to contain 55 kg of oxygen.
The volume of the room that can hold enough air containing 55 Kg of oxygen is 199927.29 L
We'll begin by converting 55 kg of oxygen to grams (g). This can be obtained as follow:
1 Kg = 1000 g
Therefore,
55 kg = 55 × 1000
55 Kg = 55000 gNext, we shall determine the volume of oxygen. This can be obtained as follow:
Mass of oxygen = 55000 kg
Density of oxygen = 1.31 g/L
Volume of oxygen =?[tex]Density = \frac{mass}{volume} \\\\1.31 = \frac{55000 }{volume}[/tex]
Cross multiply
1.31 × Volume = 55000
Divide both side by 1.31
Volume = 55000 / 1.31
Volume of oxygen = 41984.73 LFinally, we shall determine the volume of the room by calculating the volume of air. This can be obtained as follow:
Volume of oxygen = 41984.73 L
Percentage of oxygen in air = 21%
Volume of air =?[tex]Percentage of oxygen =\frac{volume of oxygen}{Volume of air} * 100[/tex]
21% = [tex]\frac{41984.73}{Volume of air}[/tex]
[tex]0.21 = \frac{41984.73}{Volume of air }[/tex]
Cross multiply
0.21 × Volume of air = 41984.73
Divide both side by 0.21
[tex]Volume of air = \frac{41984.73}{0.21}\\\\[/tex]
Volume of air = 199927.29 LTherefore, we can conclude that the volume of the room that can hold enough air containing 55 Kg of oxygen is 199927.29 L
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You are about to perform some intricate electrical studies on single skeletal muscle fibers from a gastronemius muscle. but first, you must prepare 6l of a 170 mm nacl solution in which to bath the isolated muscle during your studies. how many grams of nacl must you weigh out on the lab balance to prepare this bath solution? (hint: the molecular weight of nacl is 58.44 grams/mole).
To prepare a 6L solution of 170 mM NaCl, you need to calculate the moles required and use the molecular weight of NaCl to convert to grams. Multiply the molarity by the volume to get moles, and then multiply by the molecular weight to get 59.6088 grams.
Explanation:To prepare a 170 mM NaCl solution, you will need to calculate the number of grams of NaCl required. First, you need to understand the concentration units. Here, 170 mM (millimolar) indicates 170 millimoles of NaCl are needed per liter of solution. To find out how many millimoles you need for 6 liters, you multiply 170 mmol/L by 6 L, yielding 1020 mmol, or 1.020 mol since 1000 mmol is equivalent to 1 mol.
Next, you use the molecular weight of NaCl, which is 58.44 g/mol, to convert moles to grams. The calculation is:
1.020 mol × 58.44 g/mol = 59.6088 gTherefore, you would need to weigh out 59.6088 grams of NaCl and dissolve it in enough water to make the total volume up to 6 liters.