Q/ The value of the equilibrium constant Kp for the reaction H2 (g) +CO2(g) =H2O

Question

Q/ The value of the equilibrium  constant Kp for the reaction

H2 (g) +CO2(g) =H2O(g)+CO(g)     is 0.573 at 900C

a. Calculate the value of delta G of the reaction

Q2/The equilibrium constant Kp for the thermal

decomposition of NO2 is 6.5x10^-6 at

450 C.

2 NO2(g) = 2 NO(g) + O2(g)

If reaction vessel at this tempruture initally contains 0.500 atm NO2, what will be the partial pressure of NO2, NO, and O in the vessel when equillibrium has been attained ?

Can someone please tell me how to solve these questions?

Thanks

Explanation / Answer

1) Kp = Kc for this reaction as (delta)n is equal to zero

Hence

G = -RTlnK = -8.314 * (273 + 900) * ln(0.573) = 5.431 kJ

2) Kp = 6.5 * 10^-6

Equilibrium partial pressure be: pNO2 = 0.5 - 2x

pNO = 2x

pO2 = x

Hence

x * 4x^2/(0.5 - 2x)^2 = 6.5 * 10^-6

Solve for x to get the results.

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