Consider the following equilibrium reaction: HCO3 (aq) H+ (aq) + HCO3(aq); K = 5.0 x 10-7...

 

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Consider the following equilibrium reaction: H₂CO3 (aq) H+ (aq) + HCO3(aq); K = 5.0 x 10-7 If the initial concentrations of the species are: [H₂CO3] = 0.020 M; [H+] = 6.00 x 10-5 M; [HCO3] = 4.00 x 10-5 M Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change? Select one: O a. Q< K, so the reaction moves to the right. O b. Q< K, so the reaction moves to the left. O c. QK, so the reaction is at equilibrium. O d. Q> K, so the reaction moves to the left. Q> K, so the reaction moves to the right. e. Consider the following equilibrium reaction: H₂CO3 (aq) H+ (aq) + HCO3(aq); K = 5.0 x 10-7 If the initial concentrations of the species are: [H₂CO3] = 0.020 M; [H+] = 6.00 x 10-5 M; [HCO3] = 4.00 x 10-5 M Which one of the statements below describes the relationship between Q and K and then the correct direction of chemical change? Select one: O a. Q< K, so the reaction moves to the right. O b. Q< K, so the reaction moves to the left. O c. QK, so the reaction is at equilibrium. O d. Q> K, so the reaction moves to the left. Q> K, so the reaction moves to the right. e.

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