The equilibrium constant, K_c, is calculated using molar concentrations. For gas

Question

The equilibrium constant, K_c, is calculated using molar concentrations. For gaseous reactions another form of the equilibrium constant, K_P, is calculated from partial pressures instead of concentrations. These two equilibrium constants are related by the equation K_p = K_C(RT)^Delta n where R = 0.08206 L atm/(K mol), T is the absolute temperature, and Delta n is the change in the number of moles of gas (sum moles products -sum moles reactants). For example, consider the reaction N_2(g) + 3H_2(g) 2NH_3(g) for which Delta_n = 2 -(1 + 3) = -2. For the reaction 3A(g) + 3B(g) C(g) K_c = 53.0 at a temperature of 153 degree C Calculate the value of K_p. Express your answer numerically. For the reaction X(g) + 3Y(g) 3Z(g) K_p = 2.28 times 10^-2 at a temperature of 389 degree C. Calculate the value of K_c. Express your answer numerically.

Explanation / Answer

part A

Kp = Kc(RT)^Dn

x = 53 (0.08206*426.15)^(-5)

x = kp = 1.01*10^(-6)

part B

53 = Kc(RT)^Dn

(2.28*10^(-2)) = x(0.08206*662.15)^(-1)

Kc = 1.24

x = kc = 4.2*10^-4

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