BotanyThe equilibrium constant k p for the reaction H2(g)+CO2(g)⇌H2O(g)+CO(g) is 4.0 at 1660oc. Initially 0.80 mole H2, and 0.80 mole CO2, are injected into a 5.0 liter flask. What is the equilibrium concentration of CO2(g)?

The equilibrium constant k _p for the reaction $H_{2} (g) + {CO}_{2} (g) ⇌ H_{2} O (g) + CO (g)$ is 4.0 at 1660^oc. Initially 0.80 mole H₂, and 0.80 mole CO₂, are injected into a 5.0 liter flask. What is the equilibrium concentration of ${CO}_{2} (g) ?$

A
0.533 M
B
0.0534 M
C
0535 M
D
None of these

Solution:

$H_{2} (g) + {CO}_{2} (g) ⇌ H_{2} O (g) + CO (g) moles of eq . 0.8 - x 0.8 - x x x conc, at eq . \frac{0.8 - x}{5} (\frac{0.8 - x}{5}) (\frac{x}{5}) (\frac{x}{5}) ∵ {Δn}_{g} = 0 ∴ K_{c} = \frac{{(\frac{x}{5})}^{2}}{{(\frac{0.8 - x}{5})}^{2}} \Rightarrow 2 = \frac{x}{0.8 - x} \Rightarrow x = 0.533 [{CO}_{2} (g)] = \frac{0.8 - 0.533}{5}$