We’re being asked to determine the correct value of K_{p} at 0°C.

CO (g) + 2 H_{2} (g) ⇌ CH_{3}OH (l) K_{p} = 2.25 x 10^{4} at 298 K and ΔH_{rxn} = -128 kJ/mol.

We can use the ** van't Hoff equation** to solve for the K

$\overline{){\mathbf{ln}}{\mathbf{}}\frac{{\mathbf{K}}_{\mathbf{2}}}{{\mathbf{K}}_{\mathbf{1}}}{\mathbf{=}}{\mathbf{-}}\frac{\mathbf{\u2206}{\mathbf{H}}_{\mathbf{rxn}}}{\mathbf{R}}\mathbf{[}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{2}}}\mathbf{-}\frac{\mathbf{1}}{{\mathbf{T}}_{\mathbf{1}}}\mathbf{]}}$

where:**K _{1}** = equilibrium constant at T

For the following reaction, K_{p} = 2.25 x 10^{4} at 298 K and ΔH_{rxn} = -128 kJ/mol.

CO (g) + 2 H_{2} (g) ⇌ CH_{3}OH (l)

Which of the following is the correct value of K_{p} at 0°C?

A. 1.9 x 10^{2}

B. 2.5 x 10^{6}

C. 1.1 x 10^{2}

D. 2.5 x 10^{3}

E. 1.9 x 10^{4}

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.