2.( J Given the standard reduction potentials (E°) for ubiquinone (Q) and NADP+ provided below, consider the following questions. Q+ 2H+ + 2e ---> QH₂ NADP+ + H+ + 2e---> NADPH Eº⁹ = 0.04 V Eº⁹ = -0.32 V (a) ( Calculate the standard AEº for the oxidation of NADPH by Q. From the reactants in your derived redox reaction, indicate the oxidant and reductant. (b): .) Calculate the standard free energy of the redox reaction in part (a) and indicate if the reaction is exergonic or endergonic.

2.( J Given the standard reduction potentials (E°) for ubiquinone (Q) and NADP+ provided below, consider the following questions. Q+ 2H+ + 2e ---> QH₂ NADP+ + H+ + 2e---> NADPH Eº⁹ = 0.04 V Eº⁹ = -0.32 V (a) ( Calculate the standard AEº for the oxidation of NADPH by Q. From the reactants in your derived redox reaction, indicate the oxidant and reductant. (b): .) Calculate the standard free energy of the redox reaction in part (a) and indicate if the reaction is exergonic or endergonic.

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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[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
1 2 B A galvanic cell is composed of these two half-cells, with the standard reduction potentials shown: Co2(aq) + 2e Co(s) E° -0.28 volt; Cd2+ (aq) + 2e-Cd(s) E°--0.42 volt. What is the standard free energy change in kJ for the cell reaction of this galvanic cell? Report your answer in whole number. Do not put unit in your answer. Type your answer...
Pls help ASAP.
(Q86) What is the value (in V) of the standard cell potential (E°CELL) for the following reaction that occurs in an electrochemical cell at 25°C? Fe3+ (aq) + Cu* (aq) ---> Fe²+ (aq) + Cu2+ (aq) The reduction potentials for the two half-reactions involved are: Fe3+ + e- --> Fe2+ (E°RED) = 0.77 V Cu2+ + e- --> Cu* (E°RED) = 0.16 V %3D
Given the following galvanic cell shown with initial concentrations at 25°C, calculate Ecell after 1.50 hrs of operation at a current of 0.750 A. Assume the solution volume in both half-cells is 1.00 L. (Hint: This is not a concentration cell) Fe(s)│Fe2+(0.10 M)║Fe3+(0.35 M), Fe2+(0.15 M)│Pt(s)
You wish to construct a galvanic cell with the anode consisting of a Ni electrode in a 1.0 M Ni(NO,), solution. Which of the following would give you the highest standard cell potential if used as the cathode in this galvanic cell? Select the single best answer. O Ni* (ag) + 2e - Ni (s) E° = -0.257 V O Cu" (ag) + e - Cu (s) E° = +0.521 V © Au" (aq) + 3e Au (s) E° = +1.498 V O Al" (ag) + 3e Al (s) E° = -1.676 V O Cu* (ag) + 2e → Cu (s) E° = +0.3419 V Submit Assignme
Calculate the G in kJ for the following cell: Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Eocell=+1.59 V Al(s)|Al3+(0.0035M)||Fe3+(0.55M)|Fe(s) Group of answer choices -473 -374 -158 -734 -658 Calculate Ecell in volts. Cu(s)|Cu2+(3.00x10-4)||Ag+(0.15M)|Zn(s) Eocell=+0.620 V 0.700 0.544 0.944 0.644 0.800
is 0.085 correct or should it be 0.116? I got two answers and i’m not sure.
Oxidation of lactate by cytochrome C (represented as cytochrome C (Fe3 +)) to pyruvate is an important biological reaction.Below are the reduction reactions and standard reduction potentials (E °) at pH = 7 and 25 ° C.Pyruvate + 2H + + 2e- = Lactate - (E ° = -0.185 V)Cytochrome C (Fe3 +) + e - = Cytochrome C (Fe2 +) (E ° = 0.254 V) Considering the Gibss free energy and Nernst equations, calculate the following equilibrium ratio (K) at 25 ° C, pH = 7.
+2 t- 4) Consider the following redox reactions and their standard cell potentials: (acidic conditions) (basic conditions) S,0, (aq) + Cl2(g) = HCI0(aq) + So,"(aq) (acidic conditions) cell =-1.31 V E°cell = +0.10 V E° cell = +0.37 V E°. C2(g) + Bio*(aq) = Bi(s)+ HCIO(aq) So(aq) + 03(g) = S20 (aq) + 02(g) a) Using the ½ rxn method, balance the three redox reactions under the conditions indicated. b) Write each balanced redox reaction in the spontaneous direction and indicate its corresponding standard cell potential. c) Between these 3 redox reactions there are FOUR oxidizing agents and FOUR reducing agents. (Hint: You may need to consider the balanced equations.) i) Place the FOUR oxidizing agents in order of decreasing oxidizing strength. (From the strongest OA to the weakest OA.) ii) Place the FOUR reducing agents in order of decreasing reducing strength. ( (From the strongest RA to the weakest RA.)
A galvanic cell using Cu"/Cu and Cu?+/Cu was set up at 293 K and the non-standard cell potential was determined to be 0.175 V. Determine the concentration of ions in the cathode's solution if the concentration at the anode is 0.7787 M: (cathode)(M) number (rtol=0.03, atol=1e-08)