Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon mo

Question

Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:
CO(g)+2H2(g)CH3OH(g).
An equilibrium mixture in a 2.50 L vessel is found to contain 2.62×102 mol CH3OH, 0.170 mol CO, and 0.303 mol H2 at 500 K.

Part A

Calculate Kc at this temperature.

Methanol (CH3OH) is produced commercially by the catalyzed reaction of carbon monoxide and hydrogen:
CO(g)+2H2(g)CH3OH(g).
An equilibrium mixture in a 2.50 L vessel is found to contain 2.62×102 mol CH3OH, 0.170 mol CO, and 0.303 mol H2 at 500 K.

Part A

Calculate Kc at this temperature.

Explanation / Answer

Solution :-

Balanced reaction equation

CO(g)+2H2(g)CH3OH(g)

Lets first calculate the molarity of the each gas

Molarity = moles / volume in liter

Molarity of the CO = 0.170 mol / 2.50 L = 0.068 M

Molarity of the H2 = 0.3030 mol / 2.50 L = 0.1212 M

Molarity of the CH3OH = 2.62*10^-2 mol / 2.50 L = 1.048*10^-2 M

Kc equation is as follows

Kc= [CH3OH] /[CO][H2]^2

Kc = [1.048*10^-2] /[0.068][0.1212]^2

Kc= 10.5

Therefore Kc= 10.5

Related Questions

Navigate

• Browse (All)
• Browse M
• Subjects