± Relating Different Forms of the Equilibrium Constant For chemical reactions in

Question

± Relating Different Forms of the Equilibrium Constant

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 = 0.165 at 1687 C . What is Kp for the reaction at this temperature?

Express your answer numerically.

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Part B

For the reaction

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

Kp = 4.25×103 at 348 C . What is K for the reaction at this temperature?

Enter your answer numerically.

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Explanation / Answer

A)

T= 1687.0 oC

= (1687.0+273) K

= 1960 K

delta n = number of gaseous molecule in product - number of gaseous molecule in reactant

delta n = 2

Kp= Kc (RT)^delta n

Kp = 0.165*(0.0821*1960.0)^(2)

Kp = 4.27*10^3

Answer: 4.27*10^3

B)

T= 348.0 oC

= (348.0+273) K

= 621 K

delta n = number of gaseous molecule in product - number of gaseous molecule in reactant

delta n = -2

Kp= Kc (RT)^deltan

0.00425 = Kc *(0.0821*621.0)^(-2)

Kc = 11.0

Answer: 11.0

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