Consider the equilibrium: A B + C. K is measured as 0.50 at 25 degree C. Which s

Question

Consider the equilibrium: A B + C. K is measured as 0.50 at 25 degree C. Which statement(s) are true for the reverse reaction? the reverse reaction is not at equilibrium K = 0.50 for the reverse reaction K = 2.0 for the reverse reaction for the reverse reaction, K = [A]/([B] + [C]) both (c) & (d) are true Consider the equilibrium: A B. K is measured as 0.25 at 25 deg C. The reverse reaction is run and it is found that [A] = 0.20 M and [B] = 1.00 M. Which statement is true? the reaction is at equilibrium the reaction must shift right to attain equilibrium the reaction must shift left to attain equilibrium it is impossible for the reaction to attain equilibrium K = 1 Consider the equilibrium: A B. K is measured as 5.00 at 25 deg C. A reaction is run and the initial concentration of [A] is 1.00 M. At equilibrium, the concentrations of A and B are? [A] = 0.167 M and [B] = 0.833 M [A] = [B] = 1.00 M [A] = 0.833 M and [B] = 0.167 M [A] = 0.00 M and [B] = 1.00 M none of the above are true

Explanation / Answer

1. A <--->B+C, K= Equilibrium constant = K1/K2= [B][C]/[A], K1 rate constant for the forward reaction and K2 rate constant for the reverse reaction

for the reverse reacrtion B+C<--->, K'= [A]/[[B][C]= 1/K= 1/0.5= 2

hence only C is correct.

2. for the reaction B<--->A, K' = [A]/[B] =1/K= 1/0.25= 4

Q= reaction coefficient = 0.2/1.013 =0.19 < K', So the reaction shifts to A side. The reaction shifts to right . More A is formed. ( B is correct)

3. A<---> B, K= [B]/[A] =5

let x= drop in concentration of A to reach equilibrium

hence at equilibrijm [A] =1-x and [B] = x , K= equilibirum constnat x/(1-x)= 5, x= 5-5x

6x= 5, x= 5/6 =0.833

At equilibrium [A] = 1-0.833= 0.167 and [B]= 0.833 ( A is correct)

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