Question

part a

The reaction of nitrogen and hydrogen to produce ammonia:

N2(g) + 3H2(g) ⇌ 2NH3(g) has an equilibrium constant Kc= 1.2 at 375 °C. If the starting concentrations are [H2] = 0.76 M, [N2] = 0.60 M, and [NH3] = 0.48 M, at equilibrium which gases will have increased in concentration and which will have decreased in concentration?

a. H2

b. N2

c. NH3

part b

When solid sodium bicarbonate is heated the following decomposition reaction occurs: 2NaHCO3(s) ⇌ Na2CO3(s) + H2O(g) + CO2(g) In a closed container the reaction will reach equilibrium. If this reaction were at equilibrium, what effect would each of the following changes have on the reaction?

a. Some of the CO2 is selectively removed from the system.

b. Some solid Na2CO3 were added to the system.

c. Some solid NaHCO3 were removed from the system.

d. Some steam were added to the system.

part c

For the following reaction in a closed container at 351°C: CaCO3(s) ⇌ CaO(s) + CO2(g). The partial pressure of CO2 is 0.12 atm. Assume this reaction is the only source of CO2. What is Kc for this reaction? Assume units of mol/L

Answer 1

part a

in this reaction the equilibrium will shift on the right so the concentration of NH3 will increase and the concentrations of H2 and N2 will decrease

part b

Remember that solids don't enter into the equilibrium constant as long as there is SOME of the solid present. Adding more Na2CO3 won't change the equilibrium. when the steam added to the system the carbon dioxide is replaced then the equillibrium shifted towards left side .and if we remove sodium bicarbonate the equillibrium is shifting towards the right side. and removing the carbondioxide leads the equillibrium is shifting towards the left side

part c Kc = (CaCO3) / (CaO) (CO2)