(25 pts) For the generic reaction 2A(g) 26(g) + C(g), when 1.75 mol of A is adde

Question

(25 pts) For the generic reaction 2A(g) 26(g) + C(g), when 1.75 mol of A is added to a flask at a temperature of 345 K and fixed volume of 12.0 L, at equilibrium the ratio of B:A is 0.523. You may treat all gases in the reaction as ideal. (a) What is the equilibrium partial pressure of each substance? (b) What is the value of the equilibrium constant for this reaction at 345 K? [Note: although p° is formally defined as 1 bar, you may use 1 atm as standard pressure.] (c) what is AnnG at this temperature? (d) what is the extent of reaction () at equilibrium? (e) what is AnnG when = 0.15 mol for this reaction at 345 K? rxn

Explanation / Answer

a)

in equilibrium

A = 1.75 - 2x

B = 2x

C = x

get x

B/A = 0.523

2x / (1.75 - 2x) = 0.523

3.824x = 1.75 - 2x

5.824x = 1.75

x = 1.75/5.824 = 0.3

A = 1.75 - 2*0.3 = 1.15

B = 2*0.3 = 0.6

C = x = 0.3

total mol = 1.15 +0.6+0.3 = 2.05 mol

P = nRT/V

P = (2.05 )(0.082)(3459)/12 = 48.45 atm

b)

Keq

Keq = P-B^2 * P-C / (P-A)^2

P-A = 1.15/2.05 * 48.45 = 27.18 atm

P-B = 0.6/2.05 *48.45 = 14.180 atm

P-c = 0.3/2.05 *48.45 = 7.09 atm

Keq = (14.180 ^2)(7.09 )/(27.18 ^2)

Kp = 1.929

c)

dG = -RT*ln(K)

dG = -8.314*345*ln(1.929)

dG = -1884.4 J/mol

d)

extent of reaction, "x" shown before is 0.3

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