Question

***Please type answer if possible***

GAS VOLUME STOICHIOMETRY PROBLEMS

1. The combustion of ethanol (C₂H₅OH) takes place by the following reaction equation.

            C₂H₅OH (l)    +     3 O₂ (g)     →    2 CO₂ (g)    +    3 H₂O (g)

What is the volume of CO₂ gas produced by the combustion of excess ethanol by 23.3 grams of O₂gas at 25^oC and 1.25 atm?

GAS VOLUME STOICHIOMETRY PROBLEMS

2. Acetic acid (CH₃COOH) is formed from its elements by the following reaction equation:

            C (graphite)    +     2 H₂ (g)     +     O₂ (g)     →     CH₃COOH (g)

What is the volume of acetic acid CH₃COOH gas produced by the reaction of 18.6 grams of H₂ gas at 35^oC and 1.05 atm?

GAS VOLUME STOICHIOMETRY PROBLEMS

3. The formation of hydrazine (N₂H₄) from its elements takes place by the following reaction equation.

                        N₂ (g)              +                      2 H₂ (g)           →                    N₂H₄ (g)

What are the volumes of N₂ gas and H₂ gas required to form 28.5 grams of N₂H₄ at 30^oC and 1.50 atm?

GAS VOLUME STOICHIOMETRY PROBLEMS

4. The combustion of benzene (C₆H₆) takes place by the following reaction equation.

            2 C₆H₆ (g)     +     15 O₂ (g)     →     12 CO₂ (g)     +     6 H₂O (g)

What is the    volume of CO₂ gas formed by the combustion of 18.5 grams of C₆H₆ at 30^oC and 1.50 atm?

PARTIAL PRESSURE - MOLE FRACTION PROBLEMS

5. A mixture of gases consists of 4.00 moles of He, 2.00 moles of H₂, 3.00 moles of CO₂ and 5.00 moles of Ar. The total pressure of the mixture is 2900 mm. Determine the mole fraction of each gas in the mixture. Determine the mole percent of each gas in the mixture. Determine the partial pressure of each gas in the mixture.

PARTIAL PRESSURE - MOLE FRACTION PROBLEMS

6. Determine the total pressure of a mixture of 0.400 mole of He and 0.600 mole of Ne in a 2.00 liter container at 25^oC.

PARTIAL PRESSURE - MOLE FRACTION PROBLEMS

7. Determine the mass of Ar in 1.00 liter of a gas mixture at 25^oC which contains 0.300 atm of Ne and has a total pressure of 4.00 atm.

PARTIAL PRESSURE - MOLE FRACTION PROBLEMS

8. A 1.00 liter container holds a mixture of 0.52 mg of He and 2.05 mg of Ne at 25^oC. Determine the partial pressures of He and Ne in the flask. What is the total pressure?

Answer 1

since no particular question has been mentioned, so i am answering the first one

1. C₂H₅OH (l) + 3O₂   2CO₂ (g) + 3H₂O (g)

we are given that mass of oxygen gas = 23.3 g

we know that, number of moles = mass / molar mass ; also molar mass for  O₂ = 32.00 g/mol

n(O₂ ) = 23.3g / (32 g/mol)

n(O₂) = 0.728 mol

from balanced rxn, it can be seen that 3 moles of O₂ give 2 moles of CO₂

So, moles of CO₂  produced by 0.728 moles of O₂ = (2/3) X 0.728 mol = 0.485 mol

Volume of CO₂  can be calculated from ideal gas equation,

PV = nRT   V = nRT / P

where, n= number of moles, P= pressure = 1.25 atm; V=volume of the gas;

T=Absolute temperature( in K) = (25+273.15) K = 298.15 K

R=Ideal Gas constant also known as Boltzmann Constant = 0.082057 L atm K^-1 mol^-1.

V = [(0.485 mol) X (0.082057 L atm K^-1 mol^-1) X (298.15 K)] / 1.25 atm

V = 9.492 L

Question 2, 3 and 4 can be solved in a similar manner.

hope this helps!