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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Cr3+(aq) + 3e- = Cr(s) -0.763 V Au+(aq) + e- = Au(s) 1.680 V 1. Construct a galvanic cell from the standard reduction potential above. Label ALL the parts of your galvanic cell. To ensure that electrons are flowing properly, you need to show clearly the flow of electrons and ions in your electrochemical cells. 2. Give the half-cell reactions and the over-all reaction of the galvanic cell above. Identify to which electrode the half reactions are occurring.
Cr3+(aq) + 3e- à Cr(s) -0.763 V Au+(aq) + e- à Au(s) 1.680 V Determine the products of the aqueous salt solution of your choice from the standard reduction potential above, if it undergoes electrolysis.
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I need an answer D.
3. Using standard reduction potentials from Table L1 of Appendix L in your textbook: Chemistry: Atom's First 2e, answer the following questions considering only the following species (at standard conditions). Give reasons for your answers. Na", Cl, Ag, Ag, Zn, Zn, Pb a) Which is the strongest oxidizing agent? b) Which is the strongest reducing agent? ) Which species can be oxidized by SO (aq) in acid given the following information? so 4H 2e-HS0 HO Eat0.20 V d) Which species can be reduced by Al(s)?
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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…
Consider the following two half-reactions and their standard reduction potentials. N2(g) +H,0(1) E° = 1.766 V MnO, (s) + 2H,0(1) E° = 1.673 V N,0(g) + 2H*(aq) + 2e¯ → MnO,(aq) + 4H*(aq)+3e¯ 1st attempt l See Calculate E°for the spontaneous redox reaction that occurs when these two half-reactions are coupled. V
3.) Consider the following standard reduction potentials, which statement is correct at standard conditions? Ni?* (aq) + 2 e → Ni (s) E°red = -0.26 V I2 (s) + 2 e -> 2 (aq) E°red = 0.54 V I. Ni²* (aq) is a stronger oxidizing agent than I2 (s), and I is a stronger reducing agent than Ni (s) II. I2 (s) is a stronger oxidizing agent than Ni2", and Ni (s) is a stronger reducing agent than I (aq) III. Ni (s) is a stronger oxidizing agent than I (aq), and Ni2* is a stronger reducing agent than I2 (s) IV. I(aq) is a stronger oxidizing agent than Ni (s), and I2 (s) is a stronger reducing agent than Ni2+ (aq) А. IV В. Ш С. П D. I
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Which of the following half-reactions has been assigned a standard reduction potential, E°, of 0.00 Volts? A.) O2(g) + 4 e- → 2 O2-(aq) B.) 2 H2O(l) + 2 e- → H2(g) + 2 OH-(aq) C.) Pt + H+(aq) + e- → H-Pt D.) 2 H+(aq) + 2 e- → H2(g)