In: Chemistry
Consider the following reaction and associated equilibrium
constant: |
Part A Find the equilibrium concentrations of A and B for a=1 and b=1. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. Express your answers using two significant figures separated by a comma.
Part B Find the equilibrium concentrations of A and B for a=2 and b=2. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. Express your answers using two significant figures separated by a comma.
Part C Find the equilibrium concentrations of A and B for a = 2 and b = 1. Assume that the initial concentration of A is 1.0 M and that no B is present at the beginning of the reaction. Express your answers using two significant figures separated by a comma.
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aA(g)bB(g)
For above reaction, gas equilibrium constant is given by
Kc=([C]c[D]d)/([A]a[B]b)
Part A
a=1, b=1
A(g)B(g)
Initial concentration 1.0M 0
Change -x +x
Equilibrium concentration 1.0-x x
So Kc=[B]/[A]
4.0=x/(1.0-x)
4.0(1.0-x)=x
4.0-4x=x
4.0=5x
x=4/5=0.8M
So [A]=1.0-x=1.0-0.8=0.20M
[B]=x=0.80 M
Part B
a=2, b=2
2A(g)2B(g)Initial concentration 1.0M 0
Change -2x +2x
Equilibrium concentration 1.0-2x 2x
So Kc=[B]2/[A]2
4.0=(2x)2/(1.0-2x)2
4.0(1.0-2x)2=4x2
4.0(1+ 4x2-4x)= 4x2
4.0+16x2-16x=4x2
4+16x2-16x-4x2= 0
12x2-16x+4=0
12x2-12x-4x+4=0
12x(x-1)-4(x-1)=0
(12x-4)(x-1)=0
So x=4/12 or x=1
Now x cannot be 1.0M so x=4/12=1/3 M=0.33M
So [A]=1.0-x=1.0-0.33=0.67M
[B]=x=0.33 M
Part C
a=2, b=1
2A(g)B(g)
Initial concentration 1.0M 0
Change -2x +x
Equilibrium concentration 1.0-2x x
So Kc=[B]2/[A]2
4.0=x2/(1.0-2x)2
4.0(1.0-2x)2=x2
4.0(1+ 4x2-4x)= x2
4.0+16x2-16x=x2
4+16x2-16x-x2= 0
15x2-16x+4=0
15x2-10x-6x+4=0
5x(3x-2)-2(3x-2)=0
(5x-2)(3x-2)=0
So x=2/5 or 2/3
x=0.4 M or 0.66M
x cannot be 0.66M because then [A] will be 1.0-2x0.66M=1.0-1.22M=-0.22M which is not possible
So [A]=1.0-2x=1.0-2x0.4=1-0.8=0.2M
[B]=x=0.4M