Question

A solution is made by mixing 30.0 mL of 0.150 M compound A with 25.0 mL of 0.200 M compound B. At equilibrium, the concentration of C is 0.0454 M. Calculate the equilibrium constant, K, for this reaction.

Answer 1

Answer:

Equilibrium Constant K=6.10574

Explanation:

Consider the general form of reaction:

aA+bB⇌ cC+dD

Equilibrium Constant of above reaction is:

$K=\frac{[C]^c[D]^d}{[A]^a[B]^b}$

Where:

[C] and [D] is the concentration of Products

[A] and [B] is the concentration of reactants

a,b,c,d are number of moles

In our case above reaction will become:

A+B⇌ C

Total Concentration of reactant=0.030 L+0.025 L=0.055 L

Equilibrium Constant will become:

$K=\frac{[C]^}{[A][B]}$

Now,

$[A]=\frac{(0.030L)*(0.150)}{0.03+0.025}=0.0818M$

$[B]=\frac{(0.025L)*(0.200)}{0.03+0.025}=0.0909M$

$[C]=0.0454 M$

$K=\frac{0.0454}{(0.0818*0.0909)} \\K=6.10574$

Equilibrium Constant K=6.10574