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 K_P to distinguish it from the concentration-based equilibrium constant K. For the reaction 2CH_4(g) C_2H_2 (g) + 3H_2 (g) K = 30.135 at 1736 degree C. What is K_p for the reaction at this temperature? Express your answer numerically. For the reaction N_2 (g) + 3H_2 (g) 2NH_3(g) K_P = 2.95 times 10^-3 at 327 degree C. What is K for the reaction at this temperature? Enter your answer numerically.

Explanation / Answer

A)

Kc = 0.135 at T = 1736°C = 1736+273 = 2009 K

Kp = Kc*(RT)^dn

dn = mol of product - mol of reactant = 3+1 - 2 = 2

Kp = 0.135*(0.082*2009)^2

Kp = 3663.7121

B)

similar...

Kp = Kc*(RT)^dn

dn = 2 - (3+1) = 2-4 = -2

Kc = Kp*(RT)^-dn

T = 327 °C = 600K

Kc = (2.954*10^-3)*((0.082*600)^2)

Kc = 7.1505

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