Consider the following equilibrium reaction:
H 2 CO 3 (aq) ⇌ H + (aq) + HCO 3 – (aq); K = 5.0 x 10 –7
If the initial concentrations of the species are:
[H 2 CO 3 ] = 0.080 M; [H + ] = 1.00 x 10 –5 M; [HCO 3 – ] = 4.00 x 10 –3 M
Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?

Question

Consider the following equilibrium reaction: 
 H 2 CO 3  (aq)  ⇌  H +  (aq) + HCO 3 –  (aq);      K  = 5.0 x 10 –7 
  If the initial concentrations of the species are: 
 [H 2 CO 3 ] = 0.080 M;   [H + ] = 1.00 x 10 –5  M;   [HCO 3 – ] = 4.00 x 10 –3  M 
 Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change?

Accepted Answer

Q = K, so the reaction is at equilibrium.

Answer

Q < K, so the reaction moves to the right.

Answer

Q > K, so the reaction moves to the left.

Answer

Q < K, so the reaction moves to the left.

Answer

Q > K, so the reaction moves to the right.

Crowdly

Consider the following equilibrium reaction: H 2 CO 3 (aq) ⇌ H + (aq) + HC...

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