The free energy change for the following reaction at 25 °C, when [Pb²*] = 1.15 M and [Fe²*] = 5.40×103 M, is -73.9 kJ: Pb"(1.15 M) + Fe(s)→ Pb(s) + Fe²*(5.40×10³ M) AG=-73.9 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?

The free energy change for the following reaction at 25 °C, when [Pb²] = 1.15 M and [Fe²] = 5.40×103 M, is -73.9 kJ: Pb"(1.15 M) + Fe(s)→ Pb(s) + Fe²*(5.40×10³ M) AG=-73.9 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?

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

The free energy change for the following reaction at 25 °C, when [Hg2+] = 1.11 M and [H+] = %3D 8.68x10-3 M, is -177 kJ: Hg2+(1.11 M) + H2(g) Hg(1) + 2H+(8.68×10-3 M) AG = -177 kJ %3D 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? forward reverse Submit Answer Retry Entire Group 6 more group attempts remaining V.
A constant current is passed through an electrolytic cell containing molten MgCl2 for 13.0 h. If 5.80 x 105 g of Cl2 are obtained, what is the current in amperes?
The free energy change for the following reaction at 25 °C, when [Ag+] = 1.13 M and [Fe2+] = 7.24×10-3 M, is -252 kJ:2Ag+(1.13 M) + Fe(s)2Ag(s) + Fe2+(7.24×10-3 M) ΔG = -252 kJWhat is the cell potential for the reaction as written under these conditions?Answer: VWould this reaction be spontaneous in the forward or the reverse direction? _________forwardreverse
Calculate the non-standard cell potential (in V) for the following reaction at 65.86 ℃ with the following concentrations: [Mg+2Mg+2] = 1.00×10−71.00×10-7 M; [Cu+2Cu+2] = 5.522 MCu+2Cu+2(aq) + Mg(s) --> Cu(s) + Mg+2Mg+2(aq)
The free energy change for the following reaction at 25 °C, when Sn²+ 2+ [Zn²+] = 0.00776 M, is -133 kJ: [Sn²+] = 1.11 M and Sn²+ (1.11 M) + Zn(s) → Sn(s) + Zn²+ AG = -133 kJ What is the cell potential for the reaction as written under these conditions? Ecell V Sn(s) + Zn²+ (0.00776 M) Would this reaction be spontaneous in the forward or the reverse direction? O forward direction O reverse direction
The cell potential for the following galvanic cell is 1.15 V. The standard cell potential is 1.16 V. If [Au³+] = 0.50 M, what is the concentration of Cu2+? (R = 8.314 J/K mol, F = 96,500 C.mol-¹) 3Cu + 2Au3+→ 3℃u²+ + 2Au O 1.61 M O1.37 M O 258 M O 5.16 M
Calculate the cell potential, at 298 K, for the following reaction under the conditions given.Pb(s) + Fe2+(aq, 0.0100 M) → Pb2+(aq, 0.150 M) + Fe(s) Pb2+(aq) + 2 e‒ → Pb(s) E°red = ‒0.13 VFe2+(aq) + 2 e‒ → Fe(s) E°red = ‒0.44 V Group of answer choices: ‒0.75 V ‒0.80 V ‒0.34 V ‒0.27 V ‒0.44 V ‒0.50 V
The free energy change for the following reaction at 25 °C, when [H*] = 1.11 M and [Sn2+] = 1.21x10-3 M, is -43.9 %3D kJ: 2H*(1.11 M) + Sn(s) H2(g) + Sn2+(1.21x10-3 M) AG = -43.9 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
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?
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?
The aerosols caused a 0.590.6 °C drop in surface temperature in thenorthern hemisphere. What is the mechanism by which this occurs?
The free energy change for the following reaction at 25 °C, when [Cr**]= 2.80×103 M and [H= 1.11 M, is 94.0 kJ: 2Cr*(2.80×10³ M) + H,(g)2Cr*(aq) + 2.00H*(1.11 M) AG = 94.0 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?