Question

# Consider the following reaction and associated equilibrium constant: aA(g)+bB(g)⇌cC(g), Kc = 5.0 a.) Find the equilibrium...

Consider the following reaction and associated equilibrium constant: aA(g)+bB(g)⇌cC(g), Kc = 5.0

a.) Find the equilibrium concentrations of A, B, and C for a=1, b=1, and c=2. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction.

b.) Find the equilibrium concentrations of A, B, and C for a=1, b=1, and c=1. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction.

x= change due to equilibrium

[A] [B [C]

Initial 1 1 0

Equilibrium 1-x 1-x 2x

Equilbrium constant for A+B----> 2C ( a=1, b= 1 and c=2

K =[C] 2/ [A] [B] =5.

4x2/(1-x)2= 5

x2/ (1-x)2 =5/4 =1.25

taking square root both sides

x/(1-x)= 1.12

x= 1.12-1.12x 2.12x = 1.12 , x =1.12/2.12 =0.53

At Equilibrium [A] =[B] =1-0.53 =0.47 [C] =2*0.53= 1.06

b) for a= 1, b=1 and c=1

C will be x instead of 2x

Kc= x2/(1-x)2= 5

taking square root both side

x/(1-x) =2.24

x= 2.24- 2.24x

3.24x =2.24

x= 2.24/3.24 =0.69

At equilibium [A] =[B] = 1-0.69= 0.31 [C] =0.69

b) for a= 1 b= 1 and c=1 at equilibrium there will be 1x rather than 2x

x2/(1-x)2= 5.0

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