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] = 0.100 M; [H*] = 2.00 x 10-5 M; [HCO; = 2.00 x 10-3 M Which one of the statements below describes the relationship between Q and K and then the correct direction 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. Oc. Q > K, so the reaction moves to the right. O d. Q = K, so the reaction is at equilibrium. O e. Q< K, so the reaction moves to the left.

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] = 0.100 M; [H*] = 2.00 x 10-5 M; [HCO; = 2.00 x 10-3 M Which one of the statements below describes the relationship between Q and K and then the correct direction 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. Oc. Q > K, so the reaction moves to the right. O d. Q = K, so the reaction is at equilibrium. O e. Q< K, so the reaction moves to the left.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 61QRT

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