●Determine the AE°' for this coupled reaction?●• The relevant half-reactions are:Pyruvate + 2H+ +2e → lactateNAD+ + 2H+ + 2e →NADH + H+Eº' = -0.185 VEo = -0.315 V

∆E°is -0.31VExplanation:Approach to solving the question:To find the standard cell potential, you…

Answered: ● Determine the AE°' for this coupled…

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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The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.19 M and [Zn2+] = 7.83×10-3 M, is -133 kJ: Sn2+(1.19 M) + Zn(s)→ Sn(s) + Zn2+(7.83×10-3 M) AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
A certain metal è forms a soluble sulfate salt ₂(so). Suppose the left half cell of a galvanic cell apparatus is filled with a 5.00 M solution of M₂(SO4)3 and the right half cell with a 250. mM solution of the same substance. Electrodes made of M are dipped into both solutions and a voltmeter is connected between them. The temperature of the apparatus is held constant at 35.0 °C. Which electrode will be positive? O left Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. O right What voltage will the voltmeter show? Assume its positive lead is connected to the positive electrode. 0 x10 X
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Subject: chemistry
The chemical reaction that causes iron to corrode in air is given by: 4Fe+3O2→2Fe2O3 in which at 298 K, ΔHorxn = −1684 kJ and ΔSorxn = −543.7 J/K At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium?
The free energy change for the following reaction at 25 °C, when [Pb2+] = 3.82×10-3 M and [Cu2+] = 1.20 M, is 68.1 kJ: Pb2+(3.82×10-3 M) + 2Cu+(aq)Pb(s) + 2Cu2+(1.20 M) ΔG = 68.1 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
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The standard cell potential (E°cell) of the reaction below is -0.55 V. The value of A G° for the reaction is J/mol. 12 (s) + 2Br" (aq) → 21 (aq) + Br2 (1) 0.55 5.5 · 5. 10-6 1.1· 105 0.54 none of the above
Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś
Calculate the K and AG for the following reaction at 25 °C: с Zn(s) + CuSO₂ (aq) = ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °℃ and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. K с Part 2 of 2 = AGO = x10 Round your answer to 4 significant digits. kJ mol X Ś x10
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● Determine the AE°' for this coupled reaction? ● • The relevant half-reactions are: Pyruvate + 2H+ +2e → lactate NAD+ + 2H+ + 2e →NADH + H+ Eº' = -0.185 V Eo = -0.315 V