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Problem
Problem
Consider the following reaction:
2
CO(g)
+
O
2
(g)
⇌
2
CO
2
(g)
Δ
H
⊖
=
−
566
kJ mol
−
1
2\text{CO(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{CO}_2\text{(g)} \quad \Delta H^\ominus = -566 \text{ kJ mol}^{-1}
2
CO(g)
+
O
2
(g)
⇌
2
CO
2
(g)
Δ
H
⊖
=
−
566
kJ mol
−
1
Outline how the following changes will affect the equilibrium position and the
K
K
K
value of this reaction:
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