When the following reaction reaches equilibrium, the concentrations are 2.26 M A, 0.50 M B, and 2.00 M C. Calculate the equilibrium constant.
A+2B<=====>3C
Kc=0.884 with no unit
A+2B<=====>3c
Kc=[c]3/[A][b]2
Kc=[2.00]3 /[2.26][0.5]2
Kc=8.365/[2.26][0.25]
Kc=8.365/0.565
Kc=14.8
To calculate the equilibrium constant (K) for the given reaction, you need to use the concentrations of the reactants and products at equilibrium.
The equilibrium constant is determined by the ratio of the concentrations of the products to the concentrations of the reactants, with each concentration raised to the power of their stoichiometric coefficients in the balanced chemical equation.
The balanced chemical equation for the reaction is:
A + 2B ⇌ 3C
According to the information given, the concentrations at equilibrium are:
[A] = 2.26 M (concentration of A)
[B] = 0.50 M (concentration of B)
[C] = 2.00 M (concentration of C)
Now, let's substitute these values into the equilibrium expression:
K = ([C]^3) / ([A] * [B]^2)
Substituting the given concentrations:
K = (2.00^3) / (2.26 * 0.50^2)
Calculating this expression will give you the value of the equilibrium constant (K).