6.) Consider the following half-reaction containing acid HX below.3 N2 (g) +2 H* (aq) +2 e → 2 HX (aq) E°red = -3.09 VA. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HXbehave like an active metal?B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, O3.O: (g) + 2 H* (aq) +2 e → 02 (g) + H2O (1) E°red= 2.076 VCould HX be applied to mitigate ozone, O3 (g), depletion in the atmosphere? Write the balanced equation for the reactionused and explain why or why not using your calculated E°cell Value.C. How does your reaction equation in B support your answer to A?D. Calculate both AGº support your answer to B.I need part C to be explained clearly. Thank you!

The standard reduction potential is known as the standard electrode potential. The standard cell…

6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H* (aq) +2 e → 2 HX (aq) E°red = -3.09 v A. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HX behave like an active metal? B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, O3. O; (g) + 2 H* (aq) +2 e¯ → 02 (g) +H2O (1) E°rod=2.076 V Could HX be applied to mitigate ozone, 0: (g), depletion in the atmosphere? Write the balanced equation for the reaction used and explain why or why not using your calculated E°cell value. C. How does your reaction equation in B support your answer to A? D. Calculate both AG° support your answer to B.

6.) Consider the following half-reaction containing acid HX below. 3 N2 (g) +2 H* (aq) +2 e → 2 HX (aq) E°red = -3.09 v A. Though acids possess little in common with metals, how according to the standard-reduction potential above, does HX behave like an active metal? B. In Appendix 6 of your textbook, you discover the following half reaction which contains ozone, O3. O; (g) + 2 H* (aq) +2 e¯ → 02 (g) +H2O (1) E°rod=2.076 V Could HX be applied to mitigate ozone, 0: (g), depletion in the atmosphere? Write the balanced equation for the reaction used and explain why or why not using your calculated E°cell value. C. How does your reaction equation in B support your answer to A? D. Calculate both AG° support your answer to B.

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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QUESTION 1 Match the following terms to the correct definition. standard reduction potential (E°) Anode Cathode oxidation half-reaction Galvanic cell Cell potential reduction half-reaction electrical potential - A. difference in electrical potential that arises when dissimilar metals are connected; the driving force for the flow of charge (current) in oxidation-reduction reactions B. "the half of an oxidation-reduction reaction involving oxidation; the half-reaction in which electrons appear as products; balanced when each atom type, as well as the charge, is balanced" C. electrode in an electrochemical cell at which oxidation occurs; information about the anode is recorded on the left side of the salt bridge in cell notation D. electrochemical cell that involves a spontaneous oxidation-reduction reaction; electrochemical cells with positive cell potentials; also called à voltaic cell E. "energy per charge; in electrochemical systems, it depends on the way the charges are distributed…
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