1)Consider the following reaction and associated equilibrium constant: a A( g )

Question

1)Consider the following reaction and associated equilibrium constant: aA(g)bB(g), Kc = 3.4

Find the equilibrium concentrations of A and B for a = 2 and b = 1. Assume that the initial concentration of A is 1.0 Mand that no B is present at the beginning of the reaction.

2)

Consider the reaction for the decomposition of hydrogen disulfide:

2H2S(g)2H2(g)+S2(g),  
Kc = 1.67×107 at 800C

The reaction is carried out at the same temperature with the following initial concentrations:

[H2S]=4.30×10^4

[H2]=0.00M

[S2]=0.00M

Find the equilibrium concentration of S2.

3)Consider the following reaction: N2O4(g)2NO2(g),Kc=0.36 at 2000C

The reaction mixture initially contains only the reactant, [N2O4]=0.0260M , and no NO2.

a.Find the equilibrium concentration of N2O4.

b.Find the equilibrium concentration of NO2.

Explanation / Answer

Q1.

aA = bB

Kc = 3.4

Kc = [B]^b / [A]^a

for

3.4 = [B] / [A]^2

[A] = 1

[B] = 0

in equilibrium

[A] = 1 - 2x

[B] = 0 +x

3.4 = [B] / [A]^2

3.4 = x / (1 - 2x)^2

3.4*(1-4x+4x^2) = x

(4*3.4)*x^2 + (-1 -4*3.4)x +3.4 = 0

x = 0.34 or 0.73; 0.73 can't be so

[A] = 1 - 2x = 1-2*0.34 = 0.32

[B] = 0 +x = 0.34

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