The reversible chemical reaction A+B⇌C+D has the following equilibrium constant: Kc=[C][D][A][B]=3.4 Initially, only A and B...

The reversible chemical reaction

A+B⇌C+D

has the following equilibrium constant:

Kc=[C][D][A][B]=3.4

Initially, only A and B are present, each at 2.00 M. What is the final concentration of A once equilibrium is reached?

What is the final concentration of D at equilibrium if the initial concentrations are [A] = 1.00 M and [B] = 2.00 M ?

Solutions

Expert Solution

A + B ⇌ C + D

initial 2 2 0 0

at equi (2-x) (2-x) x x

Kc=[C] [D] / [A] [B]

3.4 = (x) * (x) / (2-x) * (2-x)

x = 1.844 = [C] = [D]

[A] = 2 - 1.84 = 0.16 = [B]

A + B ⇌ C + D

initial 1 2 0 0

at equi (1-x) (2-x) x x

Kc=[C] [D] / [A] [B]

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

x = 0.781 = [C] = [D]

[A] = 2 - 0.781 = 1.219 = [B]

queen_honey_blossom answered 1 year ago

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