For chemical reactions involving ideal gases, the equilibrium constant K can be

Question

For chemical reactions involving ideal gases, the equilibrium constant K can be expressed either in terms of the concentrations of the gases (in M) or as a function of the partial pressures of the gases (in atmospheres). In the latter case, the equilibrium constant is denoted as Kp to distinguish it from the concentration-based equilibrium constant K.

Part A

For the reaction

2CH4(g)?C2H2(g)+3H2(g)

K = 0.170 at 1795?C . What is Kp for the reaction at this temperature?

Express your answer numerically.

Part B

For the reaction

N2(g)+3H2(g)?2NH3(g)

Kp = 4.90

Explanation / Answer

Kp=K(RT)^n

A.) n = (3+1) - 2 = 2

So Kp=0.17*(2068*0.0821)^2 = 4900

B.) n= 2 -(1+3) = -2

So K=Kp(RT)^2 = 4.9x10^-3*(0.0821*617)^2= 12.57

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