One method for the decomposition of carbon dioxide proceeds as follows:
2CO₂(g)
2CO(g) + O₂(g) ; ΔH = 559 kJ
Which of the following changes will cause an increase in the equilibrium concentration of CO?

Question

One method for the decomposition of carbon dioxide proceeds as follows:
2CO₂(g)

One method for the decomposition of carbon dioxide proceeds as follows: 2CO<sub>2</sub>(g) 2CO(g) + O<sub>2</sub>(g) ; ΔH = 559 kJ Which of the following changes will cause an increase in the equilibrium concentration of CO? A) adding more O<sub>2</sub> to the system B) adding a catalyst C) removing CO<sub>2</sub> from the system D) increasing the pressure of the system at constant temperature E) increasing the temperature of the system

2CO(g) + O₂(g) ; ΔH = 559 kJ
Which of the following changes will cause an increase in the equilibrium concentration of CO?

Quizplus · Accepted Answer

According to Le Chatelier's principle, increasing the temperature of the system will shift the equilibrium towards the products side (i.e. towards CO). This is because the decomposition of CO2 is an endothermic reaction (ΔH=559 kJ) and increasing the temperature will favor the forward reaction to consume more heat. Therefore, increasing the temperature will increase the concentration of CO at equilibrium.

One Method for the Decomposition of Carbon Dioxide Proceeds as Follows