Consider the following reaction occurring at 960 K:
CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g)
At equilibrium,the concentrations of reactants and products are: [CO₂] = 0.0400 M,[H₂] = 0.0220 M,[CO] = 0.0240 M,and [H₂O] = 0.0190 M.This equilibrium is perturbed by adding CO₂(g) to the system such that when a new equilibrium is reached,the concentration of CO₂ is 0.050 M.What is the concentration of H₂(g) at this equilibrium?

Question

Quizplus · Accepted Answer

The addition of COS (carbon oxysulfide) shifts the equilibrium to the right according to Le Chatelier's principle, increasing the consumption of H2S (hydrogen sulfide) and the production of CO (carbon monoxide) and H2SO (hydrogen thioperoxide). Since the initial and final concentrations of COS are given, and assuming the reaction proceeds without any side reactions, the change in concentration of COS (from 0.0400 M to 0.0500 M) directly affects the concentration of H2S. However, without the stoichiometry of the reaction or additional information, the exact change in H2S concentration cannot be calculated precisely from the given data. The correct answer, therefore, is based on understanding the qualitative effect of the reaction shift rather than a quantitative calculation that can be directly inferred from the provided information.

Consider the Following Reaction Occurring at 960 K