Question

Determine the value of Kp at 1565 K for the conversion of carbon dioxide to carbon monoxide: Overall: CO2 (g) + H2 (g) <--> H2O (g) + CO (g), using the two equations below. Equation 1: 2 H2O (g) <--> 2 H2 (g) + O2 (g), Kp = 1.6x10^-11 Equation 2: 2 CO2 (g) <--> 2 CO (g) + O2 (g), Kp = 1.3x10^-10

Determine the value of Kp at 1565 K for the conversion of carbon dioxide to carbon monoxide:
Overall: CO2 (g) + H2 (g) <--> H2O (g) + CO (g), using the two equations below.
Equation 1: 2 H2O (g) <--> 2 H2 (g) + O2 (g), Kp = 1.6x10^-11
Equation 2: 2 CO2 (g) <--> 2 CO (g) + O2 (g), Kp = 1.3x10^-10

Answer 1

To find Kp for the conversion of CO2 to CO using the provided reactions, Equation 1 is reversed and divided by 2 to match the stoichiometry, and its Kp is modified accordingly. This modified Equations 1 is then added to Equation 2, yielding the overall reaction. The Kp for the overall reaction is calculated by multiplying the modified Kp' of Equation 1 with the Kp of Equation 2.

Step-by-step explanation:

The value of Kp for the reaction CO2 (g) + H2 (g) <--> H2O (g) + CO (g) at 1565 K can be found using the given information for two related reactions. Here is a step-by-step explanation:

1. Start with given reactions and their respective Kp values:
   Equation 1: 2 H2O (g) <--> 2 H2 (g) + O2 (g), Kp = 1.6x10^-11
   Equation 2: 2 CO2 (g) <--> 2 CO (g) + O2 (g), Kp = 1.3x10^-10
2. To obtain the overall reaction, reverse Equation 1 and divide it by 2, which will invert its equilibrium constant (Kp).
3. Multiply this reversed Equation 1 by 1/2 to get H2O (g) <--> H2 (g) + 1/2 O2 (g), with Kp' = 1 / sqrt(1.6x10^-11).
4. Add this modified Equation 1 to Equation 2 without any changes, resulting in the overall equation: CO2 (g) + H2 (g) <--> H2O (g) + CO (g).
5. The equilibrium constant (Kp) for the overall reaction is then found by multiplying the Kp' of the modified Equation 1 with the Kp of Equation 2.
   Kp = Kp' * Kp (Equation 2) = (1 / sqrt(1.6x10^-11)) * (1.3x10^-10).