Answer:
The answer to your question is Kc = 0.26
Explanation:
Data
Kc = ?
[CO] = 0.20 M
[CO₂] = 0.052 M
For this problem, do not consider the concentration of the reactants and products in a solid-state.
Formula
Kc = [tex]\frac{[CO_{2}]}{[CO]}[/tex]
Substitution
Kc = [tex]\frac{0.052}{0.2}[/tex]
Simplification and result
Kc = 0.26
Answer:
The equilibrium constant Kc is 0.26
Explanation:
Step 1: Data given
The equilibrium mixture contains 0.20 M of CO and 0.052 M of CO2
Step 2: The balanced equation
FeO(s) + CO(g) ⇌ Fe (s) + CO2 (g)
Step 3: Calculate Kc
Pure solids and liquids are not included in the equilibrium constant expression. This is because they do not affect the reactant amount at equilibrium in the reaction, so they are disregarded and kept at 1. Remember that the activity, a, of any solid or liquid in a reaction is equal to 1
Kc = [CO2] / [CO]
⇒with [CO] = 0.20 M
⇒with [CO2] = 0.052 M
Kc = 0.052 / 0.20
Kc = 0.26
The equilibrium constant Kc is 0.26
