Question

Consider the exothermic reaction 4HCl(g) + O2(g)  ⇋  2Cl2(g) + 2H2O(g). Which of the following should cause the equilibrium to shift right to form more Cl2 gas?

Answer 1

Increasing the pressure causes the equilibrium to shift towards the products side.

Step-by-step explanation:

According to Le Chatelier's principle, if pressure is increased, then the equilibrium shifts to the side with the fewer number of moles of gas. This particular reaction shows a total of 4 mol of gas as reactants and 2 mol of gas as products, so the reaction shifts toward the products side.

Answer 2

I believe the choices in this question are:

A. Lowering the temperature of the reaction.
B. Lowering the enthalpy of the reaction.
C. Decreasing the volume of the system.
D. Adding oxygen gas.
E. Decreasing the pressure of the system.

From the choices above, A, B, and D will result in creation of more Cl2 gas.