Problem: At 327ºC, the equilibrium concentrations are [CH 3OH] = 0.15 M, [CO] = 0.24 M, and [H2] = 1.1 M for the reactionCH3OH(g) ⇌ CO(g) + 2H2(g)Calculate Kp at this temperature.

We are being asked to calculate K_pat 327°C for the reaction:

CH₃OH(g) ⇌ CO(g) + 2H₂(g)

When dealing with equilibrium:

• K_c → equilibrium units are in molarity
• K_p → equilibrium units in terms of pressure

Kp and Kc are related to one another by the following equation below:

$K_{p} = K_{c} {(RT)}^{∆ n}$

R = gas constant = 0.08206 (L∙atm)/(mol∙K)
T = temperature, K
Δn = moles of gas products – moles of gas reactants

Step 1. Calculate Kc:

$K_{c} = \frac{[products]}{[reactants]} K_{c} = \frac{[CO] {[H_{2}]}^{2}}{[{CH}_{3} OH]} K_{c} = \frac{(0.24) {(1.1)}^{2}}{0.15} K_{c} = 1.936$

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At 327ºC, the equilibrium concentrations are [CH ₃OH] = 0.15 M, [CO] = 0.24 M, and [H₂] = 1.1 M for the reaction

CH₃OH(g) ⇌ CO(g) + 2H₂(g)

Calculate K_p at this temperature.

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 Chemical Equilibrium concept. You can view video lessons to learn Chemical Equilibrium. Or if you need more Chemical Equilibrium practice, you can also practice Chemical Equilibrium practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Griffith's class at UMD.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.