Consider the following equilibrium: CH₄(g)+ H₂O(g)$\leftrightarrows$ CO(g)+ 3 H₂(g).When 1.00 M CH₄ and 1.00 M H₂O are placed in a reaction vessel at 1400.0 K,their equilibrium concentrations are 0.530 M.Calculate K_p at 1400 K.

Question

Quizplus · Accepted Answer

To calculate Kp, first determine the equilibrium concentrations of CO and H2. Since CH4 and H2O both decrease by 0.470 M (1.00 M - 0.530 M), CO increases by 0.470 M and H2 increases by 3 times that, 1.41 M. Use the equilibrium expression Kp = (PCO * (PH2)^3) / (PCH4 * PH2O) and convert concentrations to partial pressures using the ideal gas law. Solving gives Kp ≈ 6.19 x 10^4.

Consider the Following Equilibrium: CH4(g)+ H2O(g) ⇆\leftrightarrows⇆ CO(g)+ 3 H2(g) ×\times× 10-4 C)6

Consider the Following Equilibrium: CH₄(g)+ H₂O(g) $\leftrightarrows$ CO(g)+ 3 H₂(g) $\times$ 10^-4
C)6