1 O e. Ke =- [N2O]? Consider the following equilibrium reaction: H2CO3 (aq) = H* (aq) + HCO; (aq); K = 5.0 x 10-7 If the initial concentrations of the species are: [H,CO3] = 0.020 M; [H*] = 6.00 x 10-5 M; [HCO;] = 4.00 x 10-5 M Which one of the statements below describes the relationship between Q and Kand 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 is at equilibrium. O C Q>K so the reaction moves to the left. O d. Q

1 O e. Ke =- [N2O]? Consider the following equilibrium reaction: H2CO3 (aq) = H* (aq) + HCO; (aq); K = 5.0 x 10-7 If the initial concentrations of the species are: [H,CO3] = 0.020 M; [H*] = 6.00 x 10-5 M; [HCO;] = 4.00 x 10-5 M Which one of the statements below describes the relationship between Q and Kand 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 is at equilibrium. O C Q>K so the reaction moves to the left. O d. Q

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A1.
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