For the reaction CO₂(g) + 2H₂O(g) $\rightarrow$ CH₄(g) + 2O₂(g) , $\Delta$ H° = 803 kJ
Which of the following will increase K?

Question

For the reaction CO₂(g) + 2H₂O(g) $\rightarrow$ CH₄(g) + 2O₂(g), $\Delta$H° = 803 kJ Which of the following will increase K?

Quizplus · Accepted Answer

According to Le Chatelier's Principle, increasing the temperature of an endothermic reaction will shift the equilibrium towards the side of the reaction that absorbs heat. In this case, the forward reaction is endothermic, so increasing the temperature will shift the equilibrium towards the products, increasing the value of K. Decreasing the number of moles of methane or increasing the volume of the system will shift the equilibrium towards the reactants, decreasing the value of K. Therefore, option D is incorrect and option E is incorrect.

For the Reaction CO2(g) + 2H2O(g) →\rightarrow→ CH4(g) + 2O2(g) Δ\DeltaΔ H° = 803 KJ Which of the Following Will Increase

For the Reaction CO₂(g) + 2H₂O(g) $\rightarrow$ CH₄(g) + 2O₂(g) $\Delta$ H° = 803 KJ
Which of the Following Will Increase