Answer to Question #313856 in General Chemistry for soidq

Question

Consider the reaction that has reached a state of equilibrium at 200^oC:

2HCl(g) + O2(g) ⇌ 2Cl2(g) + 2H2O(g)   exothermic

Determine whether each of the following will increase the equilibrium concentration of Cl2 product. Explain your reasoning.

a. Remove H2O gas

b. Remove HCl gas

c. Removing Cl2 gas.

d. Increasing the temperature of the system: 

e. Decreasing the pressure in the reaction vessel: 

Answer 1

a) removing H20 gas will favour the forward reaction, thus there will be an increase in the equilibrium concentration of Cl2 gas

b) removing HCl gas will favour the backward reaction, thus there will be a decrease in the equilibrium concentration of Cl2 gas

c) removing Cl2 gas will favour the forward reaction, thus there will be an increase in the equilibrium concentration of Cl2 gas

d) because the system is exothermic, an increase in temperature will favour the backward reaction, thus there will be a decrease in the equilibrium concentration of Cl2 gas

e) there are 3 moles on the LHS and 4 moles on the RHS. Decreasing the pressure of the system will favour the forward reaction.i.e the side with more moles, thus there will be an increase in the equilibrium concentration of Cl2 gas.