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...

See similar textbooks

Similar questions

Help me please
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
4- help pls
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.
3
need it with detailed explanation don't copy from other sources I will downvote
Please answer fast I'll rate you sure
What is the answer?
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+…