Equilibrium Constant and Reaction Quotient At equilibrium, the concentrations of
ID: 814651 • Letter: E
Question
Equilibrium Constant and Reaction Quotient At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant K, which is a mathematical expression based on the chemical equation. For example, in the reaction where a, b, c, and d are the stoichiometric coefficients, the equilibrium constant is where [A], [B], [C], and [D] are the equilibrium concentrations. If the reaction is not at equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Qc, instead of the equilibrium constant, Kc. where each concentration is measured at some arbitrary time t. Part A A mixture initially contains A, B, and C in the following concentrations: [A] = 0.650M, [B] = 1.20M, and [C] = 0.450M. The following reaction occurs and equilibrium is established: At equilibrium, [A] = 0.450M and [C] = 0.650M. Calculate the value of the equilibrium constant, Kc.Explanation / Answer
A+2B------->C
intial concentrations [A]=0.65M,[B]=1.2M,[C]=0.45
at equilibrium [A]=0.45,[B]=?,[C]=0.65
-d(A)/dt=-1/2d(B)/dt=d(C)/dt
d(C)/dt=0.65-0.45=0.2M
-1/2d(B)/dt=d(C)/dt
-d(B)/dt=2*0.2=0.4M
[B]in-[B]eq=0.4
[B]eq=0.8m
Kc=[C]/[A][B]^2
Kc=0.65/0.45*0.8^2
kc=2.26M
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.