I ReviewT ConstantsTPenodic Tabie At 298 K a cell reaction has a standard emf of +0.16 V. The equilibrium constant for the cell reaction is 5.8 x 105. You may want to reference (Pages 868 - 871) Section Part A 20.5 while completing this problem. What is the value of n for the cell reaction? Express your answer using one significant figure. να ΑΣφ n = 3 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining The number of moles of electrons transferred can be calculated using the formula AG° = -NFE°, where AG is the standard free energy, F is Faraday's constant, and E° is the standard emf. Because you are given the equilibrium constant (K) and not the free energy, you need to substitute an equality between AG and K.

I ReviewT ConstantsTPenodic Tabie At 298 K a cell reaction has a standard emf of +0.16 V. The equilibrium constant for the cell reaction is 5.8 x 105. You may want to reference (Pages 868 - 871) Section Part A 20.5 while completing this problem. What is the value of n for the cell reaction? Express your answer using one significant figure. να ΑΣφ n = 3 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining The number of moles of electrons transferred can be calculated using the formula AG° = -NFE°, where AG is the standard free energy, F is Faraday's constant, and E° is the standard emf. Because you are given the equilibrium constant (K) and not the free energy, you need to substitute an equality between AG and K.

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 [Ag*] = 1.20 M and [Cu2+] = 8.38x10-3 M, is -101 kJ: 2Ag*(1.20 M) + Cu(s)2Ag(s) + Cu2+(8.38x10-3 M) AG = -101 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 v forward reverse
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)
(a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a current of 91.2 A for a period of 60.1 min? The unbalanced chemical reaction representing this electrolysis is shown below.NaCl(aq) + H2O(l) Cl2(g) + H2(g) + NaOH(aq)__________ liters of Cl2(g) is generated by this electrolysis.(b) How many moles of NaOH(aq) are formed in the solution in this process? _______moles of NaOH(aq) are formed.
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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(9)+4 H,0(1)+4e → N,H,(aq)+4 OH (aq) - 1.16 V ʼred 2+ Zn"(aq)+2e - Zn(s) =-0.763 V ʼred Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. х10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
+ Cell Potential and Equilibrium The equilibrium constant, K, for a redox reaction is related to the standard potential, E, by the equation In K FE RT where 72 is the number of moles of electrons transferred, F (the Faraday constant) is equal to 96,500 C/(mol e-). R (the gas constant) is equal to 8.314 J/(mol K), and T is the Kelvin temperature. Standard reduction potentials ▾ Part A Use the table Express your answer numerically. ▸ View Available Hint(s) K= ΥΠΙ ΑΣΦ 9 Reduction half-reaction Ag+ (aq) +eAg(s) Cu²+ (aq) +201 >Cu(s) Sn+ (aq) + 4e →→Sn(s) 2H+ (aq) +2e →H₂(g) Ni2+ (aq) + 2e →Ni(s) Fe²+ (aq) + 2e →Fe(s) Zn²+ (aq) +2e →Zn(s) Al³+ (aq) + 3e →Al(s) Mg²+ (aq) + 2e →Mg(s) standard reduction potentials given above to calculate the equilibrium constant at standard temperature (25 °C) for the following reaction: Fe(s) + Ni²+ (aq) →>Fe²+ (aq) + Ni(s) ? E (V) 0.80 0.34 0.15 0 0.26 -0.45 0.76 -1.66 2.37 29 o Review | Constants | Period
Half-Reaction E° (V) 2H* (aq) + 2e¯ - H2 (9) 0.000 Ag* (aq) + e¯ → Ag (s) 0.7996 2H20 (I) + 2e¯ - H2 (g) + 20OH" (aq) -0.8277 AI3+ (aq) + 3e¯ → Al (s) -1.676 H2O2 (aq) + 2H* (aq) + 2e¯ → 2H20 (1I) 1.776 Au+ (aq) + e¯→ Au (s) 1.692 I2 (s) + 2e¯ → 21¯ (aq) 0.5355 Au3+ (aq) + 3e¯ → Au (s) 1.498 2103- (aq) + 12H* (aq) + 10e¯ → I2 (s) + 6H2O (1) Mg2+ (aq) + 2e - Mg (s) 1.195 Ba2+ (aq) + 2e¯ → Ba (s) -2.912 -2.372 Br2 (1) + 2e¯ → 2B1¯ (aq) 1.066 Mn2+ (aq) + 2e" → Mn (s) -1.185 Ca2+ (aq) + 2e¯ → Ca (s) -2.868 Mno2 (s) + 4H+ (aq) + 2e¯ → Mn2+ (aq) + 2H20 (1) 1.224 Cl2 (g) + 2e¯ → 2C1- (aq) 1.35827 Mno4- (aq) + 8H* (aq) + 5e¯ → Mn2+ (aq) + 4H2O (1) 1.507 Co2+ (aq) + 2e¯ → Co (s) -0.28 Mnog- (aq) + 2H20 (I) + 3e¯ → MnO2 (s) + 40H¯ (aq) 0.595 Co3+ (aq) + e¯ → Co2+ (aq) 1.92 HNO2 (aq) + H+ (aq) + e¯ → NO (g) + H2O (I) 0.983 Cr2+ (aq) + 2e¯ → Cr (s) -0.913 N2 (g) + 4H2O (1) + 4e¯ → 40H" (aq) + N2H4 (aq) -1.16 Cr3+ (aq) + 3e¯ → Cr (s) -0.744 NO3- (aq) + 4H* (aq) + 3e¯ → NO (g) + 2H2O (1) 0.957 Cr3+…
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