Question

6. Now consider the following equilibrium also occurring when you burn gas: 2 CO2(g) → 2 CO (g) + O2 (g) Predict what will occur to the CO concentration under the following conditions: and EXPLAIN WHY i. some oxygen is selectively removed from the mixture ii. the temperature is increased iii. the total pressure is increased by making the container smaller iv. Some CO2 (g) is added to the mix

Answer 1

(i) When some oxygen is selectively removed from the mixture, the reaction will shift forward to counteract the decreased concentration of oxygen and establish a new equilibrium. As the reaction shifts forward, the concentration of CO will increase.

(ii) The reaction is an exothermic reaction where heat is released. So, when the temperature is increased, system will shift backward to dscreased the temperature and establish a new equilibrium. As the reaction shifts backward, the concentration of CO will decrease.

(iii) The number of moles of gas is 3 at the product side and 2 at the reactant side. So, when the total pressure is increased the reaction will shift backward where the number of moles of gas is less in order to counteract the increased pressure and establish a new equilibrium. As the reaction shifts backward, the concentration of CO will decrease.

(iv) When some CO₂(g) is added, the system will counteract the increased concentration of CO₂ by shifting the reaction forward and establish a new equilibrium. As the reaction shifts forward, the concentration of CO will increase.