Solution Found!
Answer: Consider the following equilibrium process at
Chapter 14, Problem 46P(choose chapter or problem)
Consider the following equilibrium process at \(686^{\circ} \mathrm{C}\):
\(\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\ \leftrightharpoons\ C O(g)+\mathrm{H}_{2} O(g)\)
The equilibrium concentrations of the reacting species are \([\mathrm{CO}]=0.050 \mathrm{M},\ \left[\mathrm{H}_{2}\right]=0.0450 \mathrm{M},\ \left[\mathrm{CO}_{2}\right]=0.086 \mathrm{M},\ \text { and }\left[\mathrm{H}_{2} \mathrm{O}\right]=0.040 \mathrm{M}\). (a) Calculate \(K_{c}\) for the reaction at \(686^{\circ} \mathrm{C}\). (b) If we add \(\mathrm{CO}_{2}\) to increase its concentration to 0.50 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
Questions & Answers
QUESTION:
Consider the following equilibrium process at \(686^{\circ} \mathrm{C}\):
\(\mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\ \leftrightharpoons\ C O(g)+\mathrm{H}_{2} O(g)\)
The equilibrium concentrations of the reacting species are \([\mathrm{CO}]=0.050 \mathrm{M},\ \left[\mathrm{H}_{2}\right]=0.0450 \mathrm{M},\ \left[\mathrm{CO}_{2}\right]=0.086 \mathrm{M},\ \text { and }\left[\mathrm{H}_{2} \mathrm{O}\right]=0.040 \mathrm{M}\). (a) Calculate \(K_{c}\) for the reaction at \(686^{\circ} \mathrm{C}\). (b) If we add \(\mathrm{CO}_{2}\) to increase its concentration to 0.50 mol/L, what will the concentrations of all the gases be when equilibrium is reestablished?
ANSWER:Step 1 of 3
Given data:
