What is the ph of a solution containing 0.12 mol/l of nh4cl and 0.03 mol/l of naoh (pka of is 9.25)?

Answer:ANSWER

Explanation:

To find the minimum volume of chlorine gas required to react with 7.85 g of aluminum, we convert the mass of aluminum to moles, find the necessary moles of chlorine gas using the balanced equation, and then apply the ideal gas law to find the volume.

The question is asking about the volume of chlorine gas required to completely react with a given amount of aluminum. We know from the balanced equation that 2 moles of aluminum (Al) react with 3 moles of chlorine gas (Cl) to form 2 moles of aluminum chloride (AlCl₃). First, we've to convert the mass of aluminum to moles by dividing the mass 7.85g by the molar mass of aluminum (26.98 g/mol), giving approximately 0.291 mol.

From the equation, we know the mole ratio of Al to Cl2 is 2 to 3. Therefore, 0.291 moles of Al will require 0.437 mol of Cl₂. Next, we apply the ideal gas law (PV=nRT) to find the volume. Here, P=225 mmHg (which is 0.296 atmospheres), R=0.0821(atm L)/(mol K), T=298 K and n=0.437 mol.

Finally, solving for V in PV=nRT gives us V = nRT/P, approximating 11.08 L as the minimum volume of chlorine gas required to react.

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Answer: The drying process worked to preserve them

Explanation: apex

Answer:

Explanation:

The compounds in exercise 48 are:

a) P4O6,

b) Ca3 (PO4)2, and

c) Na2 H PO4

So, proceed with the calculus for each compound.

a) Molecular formula: P4O6

Molar mass: 4 * 31 g/mol + 6* 16g/mol = 220 g/mol

Number of moles in 1.00 grams of compound = mass in grams / molar mass =

= 1.00 g / 220 g/mol = 0.004545 mol

0.004545 mol of P4O6 contains 4 * 0.004545 =  0.01818moles of atoms of P.

=> 0.01818 moles * 6.022 * 10^23 atoms / mol = 1.095 * 10^ 22 atoms of P.

Answer: 1.095 * 10^22 atoms of P.

b) Ca3 (PO4)2

molar mass = 3 * 40.1 g/mol + 2 * 31.0 g/mol + 8 * 16 g/mol = 310.3 g/mol

number of moles in 1.00 g of Ca3 (PO4)2 = 1.00 g / 310.3 g/mol = 0.00322 mol

0.00322 mol of compound * 2 mol P / mol of compound = 0.00644 mol P

0.00644 mol P * 6.022 * 10^23 atom / mol = 3.878 * 10 ^ 21 atoms P

Answer: 3.878 * 10^21 atoms P

c) Na2 H PO4

molar mass = 2 * 23.0 g/mol + 1 g/mol + 31.0 g/mol + 4 * 16g/mol = 142.0 g/mol

number of moles = 1.00 g / 142.0 g/mol = 0.0070 moles Na2HPO4

=> 0.0070 moles P

=> 0.0070 * 6.022 * 10^23 = 4.215 * 10^21 atoms of P

Answer: 4.215 * 10^21 atoms P

Final answer:

To determine the number of atoms of phosphorus in a compound, you need to use the molar mass and Avogadro's number. Convert the mass of the compound to moles and then multiply by Avogadro's number to get the number of atoms.

Explanation:

The number of atoms of phosphorus present in a compound can be determined using the molar mass and Avogadro's number. We need to convert the mass of the compound to moles using its molar mass, and then multiply by Avogadro's number to get the number of atoms.

For example, if we have 1.00g of phosphorus pentoxide (P2O5), we can calculate the number of atoms of phosphorus by:

The result will be the number of atoms of phosphorus in 1.00g of P2O5.

Answer:

112 °C = 385 K

Explanation:

The relation between Kelvin and Celsius degrees is

0°C = 273.15 K

To convert the temperature from Celsius to Kelvin we must add 273.15:

112 °C + 273.15 = 385.15 K

With the correct significant figures the answer would be 385 K

Answer:

Exothermic chemical reaction

Endothermic chemical reaction

An Exothermic chemical reaction releases energy, whereas an Endothermic chemical reaction requires an input of energy.

An Exothermic chemical reaction involves the release of heat(thermal energy) in a system to the surroundings. The enthalpy(heat) change which is ΔH decreases in this type of reaction

An Endothermic chemical reaction involves the absorption or input of heat in the form of thermal energy by the system from the surroundings. The enthalpy(heat) change which is ΔH increases in this type of reaction.  

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The evaporation of 190g of isopropyl alcohol would remove approximately 463.6 kJ of heat.

The student asked: 'How much heat is removed from the skin by the evaporation of 190 g (about 1/2 cup) of isopropyl alcohol?' The process of evaporation removes heat from the surface it's occurring on because energy is needed to change a substance from a liquid state to a gaseous one. This is known as the enthalpy of vaporization. Unfortunately, the value provided for the vaporization of water can't be directly used for isopropyl alcohol. However, using related scientific data, the approximate heat of vaporization for isopropyl alcohol is about 2.44 kJ/g. Therefore, to calculate the heat removed by evaporation of 190g of isopropyl alcohol, we would multiply the mass (190g) by the heat of vaporization (2.44 kJ/g) which totals approximately 463.6 kJ.

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To calculate the heat removed by the evaporation of isopropyl alcohol, one would typically multiply the number of moles of the alcohol by its heat of vaporization, which is approximately 45.3 kJ/mol at boiling point; however, the specific heat of vaporization at skin temperature is necessary to determine the exact amount of heat removed.

To determine how much heat is removed from the skin by the evaporation of isopropyl alcohol, we need the heat of vaporization for isopropyl alcohol (also known as isopropanol). The heat of vaporization is the amount of heat required to turn a liquid into a vapor without a temperature change. Unfortunately, we do not have the exact heat of vaporization value for isopropyl alcohol at human skin temperature provided in the reference, which would directly allow the calculation. However, we can consider that the heat of vaporization for isopropyl alcohol is typically around 45.3 kJ/mol at its boiling point.

For the sake of explanation, let's assume that this value is close enough to use for a skin temperature of 37 °C. The molar mass of isopropyl alcohol (C3H8O) is approximately 60.1 g/mol. First, we would convert 190 g of isopropyl alcohol to moles:

Moles of isopropyl alcohol = mass (g) / molar mass (g/mol) = 190 g / 60.1 g/mol

Then, we would multiply the moles by the heat of vaporization to get the total amount of heat removed:

Heat removed (kJ) = moles * heat of vaporization (kJ/mol)

Without the exact value for the heat of vaporization of isopropyl alcohol at skin temperature, we cannot provide the exact amount of heat removed. However, this process illustrates how the calculation would be performed given the correct data.

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Answer:

Initial pressure = 600 torr

Explanation:

Given:

Initial pressure, P1 = 900 torr

Initial Temperature, T1 = 300 K

Final temperature, T2 = 450 K

To determine:

Final pressure of  gas, P2

Explanation:

Based on the ideal gas equation

[tex]PV = nRT\\[/tex]

where n = moles of gas

R = gas constant, T = temperature

At constant volume (V), the above equation becomes:

P/T = constant

This is Gay-Lussac's law

[tex]\frac{P1}{T1} =\frac{P2}{T2} \\\\P1=\frac{P2}{T2} *T1=\frac{900\ torr}{450\ K} *300\ K=600\ torr[/tex]

In the reaction, each mole of O2 produces 1.2 moles of H2O. By converting the mass of O2 in the problem to moles (using O2's molar mass), multiply by 1.2 to find moles of H2O, and then converting moles of H2O to grams (using H2O's molar mass), the problem can be solved.

This question concerns the reaction of ammonia (NH3) with oxygen gas (O2) to produce nitric oxide (NO) and water (H2O). This is an oxidation-reduction reaction. The balanced equation for the reaction is actually 4NH3 (g) + 5O2 (g) -> 4NO (g) + 6H2O (g). Oxygen's molar mass is 32.00 g/mol, the molar mass of water is 18.02 g/mol. Therefore, for every 5 mol of O2, 6 mol of H2O are produced, or every 1 mol of O2 produces 1.2 mol of H2O (6/5). So, you can calculate the number of moles of gas in 8.45 g then multiply by 1.2 to get the number of moles of H2O, and finally multiply this by the molar mass of H2O to find the mass in grams. The final answer can be rounded to 3 significant digits.

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Answer:

1- Carbon dioxide in our breath comes from the carbon in our food.

2- All plants need carbon dioxide to survive.

3- About .04 percent of the atmosphere's air is carbon dioxide and  4.4       percent of our breath is carbon dioxide we breathe out more carbon          dioxide than we breathe in.

4- Some effects might include combustion with other gasses and it could also potentially kill all life.

Explanation:

The solution would be like this for this specific problem:

Given:

66.0 g of carbon monoxide

In the given reaction moles of carbon are needed to produce 66.0 g of carbon monoxide is 2.35 moles.

Moles of any substance will be calculated as:

n = W/M, where

W = given mass

M = molar mass

Given chemical reaction is:

2C + O₂ → 2CO

Moles of 66g of CO = 66g / 28g/mol = 2.35 mol

2 moles of CO = produced by 2 moles of carbon

2.35 moles of CO = produced by 2.35 moles of carbon

Hence, required moles of carbon are 2.35 moles.

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We need an equation that would relate the concentration of the original solution to that of the desired solution. To solve this we use the equation expressed as follows, 

M1V1 = M2V2

where M1 is the concentration of the stock solution, V1 is the volume of the stock solution, M2 is the concentration of the new solution and V2 is its volume.

M1V1 = M2V2

0.266 M x V1 = 0.075 M x 150 mL

V1 = 42.29 mL

Therefore, we need about 42.29 mL of the 0.266 M of lithium nitrate solution to make 150.0 mL of the 0.075 M lithium nitrate solution.

[tex]\boxed{{\text{42}}{\text{.3 mL}}}[/tex] of a 0.266 M [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution is required to make 150 mL of a 0.075 M [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution.

Further Explanation:

The concentration is the proportion of substance in the mixture. The most commonly used concentration terms are as follows:

1. Molarity (M)

2. Molality (m)

3. Mole fraction (X)

4. Parts per million (ppm)

5. Mass percent ((w/w) %)

6. Volume percent ((v/v) %)

Molarity is a concentration term that is defined as the number of moles of solute dissolved in one litre of the solution. It is denoted by M and its unit is mol/L.

The molarity equation is given by the following expression:

[tex]{{\text{M}}_{\text{1}}}{{\text{V}}_{\text{1}}} = {{\text{M}}_{\text{2}}}{{\text{V}}_{\text{2}}}[/tex]                      …… (1)

Here,

[tex]{{\text{M}}_{\text{1}}}[/tex] is the molarity of the initial [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution.

[tex]{{\text{V}}_{_{\text{1}}}}[/tex] is the volume of the initial [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution.

[tex]{{\text{M}}_{\text{2}}}[/tex] is the molarity of the new [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution.

[tex]{{\text{V}}_{_{\text{2}}}}[/tex] is the volume of the new [tex]{\text{LiN}}{{\text{O}}_{\text{3}}}[/tex] solution.

Rearrange equation (1) to calculate [tex]{{\text{V}}_{\text{1}}}[/tex].

[tex]{{\text{V}}_{\text{1}}}=\frac{{{{\text{M}}_{\text{2}}}{{\text{V}}_{\text{2}}}}}{{{{\text{M}}_{\text{1}}}}}[/tex]                    …… (2)

The value of [tex]{{\text{M}}_{\text{1}}}[/tex] is 0.266 M.

The value of [tex]{{\text{M}}_{\text{2}}}[/tex] is 0.075 M.

The value of [tex]{{\text{V}}_{_{\text{2}}}}[/tex] is 150 mL.

Substitute these values in equation (2).

[tex]\begin{aligned}{{\text{V}}_{\text{1}}}&=\frac{{\left({{\text{0}}{\text{.075 M}}} \right)\left( {{\text{150 mL}}} \right)}}{{{\text{0}}{\text{.266 M}}}}\\&=42.29{\text{ mL}}\\&\approx 42.{\text{3 mL}}\\\end{aligned}[/tex]

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Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Concentration terms

Keywords: molarity, LiNO3, 42.3 mL, molarity equation, volume, M1, M2, V1, V2, 150 mL, 0.075 M, 0.266 M, concentration, concentration terms.

The total Hhydr is:

Hhydr = – 336 kJ/mol + – 532.7 kJ/mol

Hhydr = - 868.7 kJ/mol

Therefore using the formula Hsol = –Hlat + Hhydr we can get Hlat.

– 58 kJ/mol = – Hlat + - 868.7 kJ/mol

- Hlat = 810.7 kJ/mol

Hlat = - 810.7 kJ/mol

ANSWER: 

Answer:D

Explanation:

We can calculate for temperature by assuming the equation for ideal gas law:

P V = n R T

Where,

P = pressure = 1.80 atm

V = volume = 18.2 L

n = number of moles = 1.20 moles

R = gas constant = 0.08205746 L atm / mol K

Substituting to the given equation:

T = P V / n R

T = (1.8 atm * 18.2 L) / (1.2 moles * 0.08205746 L atm / mol K)

T = 332.70 K

We can convert K unit to ˚C unit by subtracting 273.15 to Kelvin, therefore

T = 59.55 ˚C

Matt's conclusion that only metals conduct both heat and electricity is partially correct. While most metals do conduct both, there are also non-metal substances, like graphite and ionic solutions, that exhibit these properties.

While Matt's observation that many materials that conduct heat also conduct electricity is correct, his conclusion that only metals conduct both heat and electricity is not completely accurate. In fact, there are also some non-metal materials which can conduct heat and electricity. For example, graphite, a form of carbon and a non-metal, has layers of carbon atoms that are free to move and conduct electricity. Similarly, many ionic solutions can also conduct electricity when they are in the liquid state as their ions are free to move.

Conduction of heat and electricity often happens in materials that have free electrons. Metals are a great example of this, but they're not the only example. So, while it's true that most metals do conduct both heat and electricity, it's important to note that they are not the only materials that can do so.

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Copper is a metallic atomic solid , the atoms are arranged in a regular pattern, with the valence electrons being free to move throughout the structure.Thus, the correct option is metallic atomic solid.

Copper is an example of a metal, and metals typically exhibit metallic bonding, where the valence electrons form a "sea" of delocalized electrons, creating strong bonds between the metal atoms. This allows for the high electrical and thermal conductivity that metals are known for.

Metallic solids are compounds that are entirely comprised of metal atoms that are held together by metallic bonds.Metallic bonding is a type of intramolecular force of attraction that occurs between a lattice of positive ions and a "sea" of delocalized electrons.

Thus, the correct option is metallic atomic solid.

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Final answer:

To determine the number of moles of NaOH from 20 grams, calculate the substance's molar mass (39.997 g/mol) and divide the given mass by the molar mass, resulting in 0.5001 moles of NaOH.

Explanation:

The question asks about calculating the moles of sodium hydroxide (NaOH) from its mass in grams. To find moles, one has to use the molar mass of the substance.

First, calculate the molar mass of NaOH:
Na (1 x 22.990 g/mol) + O (1 x 15.999 g/mol) + H (1 x 1.008 g/mol) = 39.997 g/mol.

Next, use this molar mass to find the number of moles:
Given: 20.0 g NaOH,
Desired: moles NaOH
Since 1 mole of NaOH weighs 39.997 g, then:
moles of NaOH = mass (20 g) ÷ molar mass (39.997 g/mol) = 0.5001 moles.

To solve this problem, we should recall that the change in enthalpy is calculated by subtracting the total enthalpy of the reactants from the total enthalpy of the products:

ΔH = Total H of products – Total H of reactants

You did not insert the table in this problem, therefore I will find other sources to find for the enthalpies of each compound.

ΔHf CO2 (g) = -393.5 kJ/mol

ΔHf CO (g) = -110.5 kJ/mol

ΔHf Fe2O3 (s) = -822.1 kJ/mol

ΔHf Fe(s) = 0.0 kJ/mol

Since the given enthalpies are still in kJ/mol, we have to multiply that with the number of moles in the formula. Therefore solving for ΔH:

ΔH = [3 mol ( − 393.5 kJ/mol) + 1 mol (0.0 kJ/mol)] − [3 mol ( − 110.5 kJ/mol) + 2 mol ( − 822.1 kJ/mol)]

ΔH = 795.2 kJ

Answer:

-189.5

Explanation:

Correct with Acellus Chemistry

The balanced equation for the reaction of hydrogen peroxide with ferrous ions to produce ferric ions and water in an acidic solution is H2O2(aq) + 2H+(aq) + 2Fe2+(aq) → 2H2O(l) + 2Fe3+(aq).

The balanced equation for the oxidation-reduction reaction that occurs when hydrogen peroxide reacts with the ferrous ion (Fe2+) in an acidic solution to produce ferric ion (Fe3+) and water is:

H2O2(aq) + 2H+(aq) + 2Fe2+(aq) → 2H2O(l) + 2Fe3+(aq)

This reaction showcases the oxidizing property of hydrogen peroxide. The ferrous ion (Fe2+) is oxidized to the ferric ion (Fe3+), while the hydrogen peroxide (H2O2) is reduced to water (H2O).

Covalent bonds between atoms form when these atoms share one or more pairs of their valence electrons. This is a pathway to stability for the atoms involved. This type of bonding happens in many compounds, such as in a molecule of hydrogen.

A covalent bond between two atoms occurs when these atoms share one or more pairs of their valence electrons. In this type of bonding, both atoms contribute at least one electron to the shared pair. This is a way for both atoms to achieve a stable electron configuration, often completing an outer shell of electrons.

For example, consider the hydrogen molecule, H2. Hydrogen has one valence electron and needs two for stability, so two hydrogen atoms can share their electrons to form a covalent bond, resulting in a stable molecule.

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The one I would expect to have the largest dispersion forces would be the largest and heaviest molecule. This is evidenced by the fact that that molecule is a liquid at room temperature while all the others are gases.

C3H8 = This is propane and a gas at room temperature

F2 = Also a gas at room temperature

BeCl2 = This is a solid and forms an extended lattice in the form of Be-Cl-Be bridges therefore dispersion forces are not important

Therefore the answer to this is C12H26 which is a wax and a liquid at room temperature.

Answer:

C12H26

Among the substances listed (C12H26, Be, Cl2, C3H8, F2), the largest dispersion forces are expected in C12H26 due to its larger molecular size and weight. Dispersion forces are temporary shifts in electron density causing attraction between molecules and are much stronger in larger and heavier molecules.  Smaller molecules like Cl₂ and F₂ have weaker dispersion forces.

The substance expected to have the largest dispersion forces from the ones mentioned (C12H26, Be, Cl2, C3H8, F2) is C12H26 due to its large size and molecular weight. Dispersion forces, also known as London dispersion forces, are temporary shifts in electron density in non-polar molecules that result in attraction between molecules. This is typically stronger in larger and heavier molecules. As C12H26 is a larger, heavier, and more complex molecule than the others listed, it has more electrons, hence more shifting of electron density and stronger resultant dispersion forces.

For other compounds like Cl₂ and F₂, they are gases at room temperature, meaning that their dispersion forces are weaker. This is because dispersion forces influence the boiling and melting points of substances. Larger dispersion forces lead to higher melting and boiling points, which is also why C12H26, a component of diesel and other heavy oils, is a liquid at room temperature.

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