Assume that the following $\underline{\text{ endothermic }}$chemical reaction is at equilibrium. C(s)+ H₂O(g) H₂(g)+ CO(g) Which of the following statements is/are CORRECT? 1)Increasing the concentration of H₂(g)will cause the reaction to proceed in the backward direction,increasing the equilibrium concentration of H₂O(g). 2)Decreasing the temperature will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g). 3)Increasing the amount of C(s)will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).

Question

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1) According to Le Chatelier's principle, increasing the concentration of H₂(g) will cause the equilibrium to shift in the opposite direction to consume some of the excess reactant, which means the reaction will proceed in the backward direction, increasing the equilibrium concentration of H₂O(g). This is because the reaction is endothermic, and adding more of the reactant on the product side will help consume some of the product and shift the equilibrium towards more products. 2) Decreasing the temperature will cause the equilibrium to shift to the exothermic direction, which is the forward direction, since the reaction is endothermic. Thus, the equilibrium concentration of CO(g) will increase. 3) Adding more C(s) will not affect the equilibrium since it is a solid and does not participate in the equilibrium. Therefore, the equilibrium concentrations of the gases, H₂O(g) and CO(g) will not be affected by the addition of C(s).

Assume That the Following endothermic ‾\underline{\text{ endothermic }} endothermic ​ Chemical Reaction Is at Equilibrium

Assume That the Following $\underline{\text{ endothermic }}$ Chemical Reaction Is at Equilibrium