Equilibrium constant, K_c, is calculated using molar concentrations. For gaseous

Question

Equilibrium constant, K_c, is calculated using molar concentrations. For gaseous another form of the equilibrium constant, K_p, is calculated from partial instead of concentrations. These two equilibrium constant are related by the K_p = K_c (RT)^Delta n R = 0.06206 L. atm/(K mol), T is the absolute temperature, and Delta n is the the number of moles of gas (sum moles products - sum moles reactants). For consider the reaction N_2(g) + 3H_2(g) 2NH_3(g) Delta n = 2 - (1 + 3) = -2. For the reaction 3A(g) + 3B(g) C(g) K_c = 63.4 at a temperature of 79 degree C. Calculate the value of K_p. Express your answer numerically. For the reaction X(g) + 2Y(g) 3Z(g) K_p = 1.90 Times 10^-2 at a temperature of 43 degree C. Calculate the value of K_c.

Explanation / Answer

Kc = 63.4 at T = 79°C = 352 K

Find Kp for

3A + 3B = C

dn = 1- (3+3) = 1-6 -5

R = 0.082 ant T =352

Kp = Kc*(RT)^dn

Kp = (63.4)((0.082*352)^(-5))

Kp = 3.1645*10^-6

B)

Kp = 1.9*10^-2

T = 43°C = 316 K

Find Kc

Kp = Kc*(RT)^dn

then

Kc = Kp*(RT)^-dn

for reaction

X + 2Y = 3Z

dn = 3-(1+2) = 3-3 = 0

then

Kp = Kc*(RT)^0

Kp = Kc

Kc = 1.9*10^-2

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