1) Consider the following gas-phase equilibria at 800.0 K: c) Consider a mixture

Question

1) Consider the following gas-phase equilibria at 800.0 K:

c) Consider a mixture of air, which is essentially 80.0 mole percent N2(g) and 20.0 mole percent O2(g), and a trace amount of NO2(g) placed into a closed container and allowed to achieve equilibrium at 800.0 K with a total pressure of 1.05 atm. What are the equilibrium partial pressures (in atm) of N2(g), O2(g), NO(g), and NO2(g) in this container. (HINT: based on the values of the Kp for the equilibria above, what approximations can you make?)

a) If the total pressure in the container, which has a volume of 100.0 mL, is 0.85 atm, what are the partial pressures (in atm) of NO2(g) and N2O4(g) in this container at 300.0 K?

b) Using your answer to (b), what are the equilibrium concentrations (in M) of NO2(g) and N2O4(g) in this container at 300.0 K?

c) Use your answer to (c) to evaluate Kc for this equilibrium. Verify equation Kp= Kc(RT)?n which relates Kp and Kc for gas-phase equilibria.

d) At low temperatures, close examination of the closed reaction vessel containing essentially all dinitrogen tetroxide shows small amounts of a blue-green liquid that comes from the reaction of dinitrogen tetroxide with trace amounts of water leading to dinitrogen trioxide (blue) and nitric acid (colorless). Write the balanced chemical equation for this reaction.

e) With greater amounts of water, dinitrogen tetroxide hydrolyzes into nitrous acid and nitric acid. Write the balanced chemical equation for this process.

3) Suggest four ways in which the equilibrium concentration of NO2(g) can be increased in a closed container if the only chemical equilibrium is

Explanation / Answer

(2)

(3)

i. Increase in concentration of reactants

ii. Decrease in temperature, because it is exothermic in nature

iii. Increase in pressure, because forward reaction involves in decrease in number of gaseous moles.

iv. Removing product formed.

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