Calculate the maximum work available (in kJ) from 52.3 g of aluminum in the following cell when the cell potential is 1.15 V. Note that O2 is reduced to H2O. Al(s) | Al3+(aq) || H+(aq) | O2(g) | Pt

The free energy change for the following reaction at 25 °C, when [Pb2+] = 1.17 M and [Ni2+] = 9.99×10-3 M, is -35.7 kJ:Pb2+(1.17 M) + Ni(s) → Pb(s) + Ni2+(9.99×10-3 M)     ΔG = -35.7 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? _________ (forward or reverse)

The free energy change for the following reaction at 25 °C, when [Sn2+] = 1.13 M and [Ni2+] = 4.56×10-3 M, is -34.9 kJ:Sn2+(1.13 M) + Ni(s)→ Sn(s) + Ni2+(4.56×10-3 M)     ΔG = -34.9 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? _________. (forward or reverse)

For the galvanic cell, C(gr) | Cs(s) |Cs*(aq) || Sn2*(aq) | Sn(s), what is the function of the C(gr)? C(gr) is in the cathode compartment and is a product in the overall cell reaction. C(gr) is in the anode compartment and is a reactant in the overall cell reaction. C(gr) conducts electrons into the cathode and does not appear in the overall cell reaction. C(gr) conducts electrons out of the anode and does not appear in the overall cell reaction. None of these

For the cell shown, the measured cell potential, E cell, is -0.3643 V at 25 °C. Pt(s) | H₂(g,0.895 atm) | H* (aq, ? M) || Cd² +(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are → H₂ (g) 2 H+ (aq) + 2 e [H+] Cd²+(aq) + 2e Calculate the H+ concentration. = 0.141 → Cd(s) Incorrect E° = 0.00 V Eº = -0.403 V M

Calculate the standard free-energy change, in kilojoules, at 25 °C for the reaction 2 Ag* (aq) + Zn (s) → Zn2* (aq) + 2 Ag (s) Eº cell = 1.56 V O -301 kJ O - 151 kJ +301 kJ « 105 -3.01 x

What is the maximum work (in kJ) you can obtain from 18.2 g of nickel in the following cell when the emf is 0.97 V? Ni(s) | Ni2+(aq) || Ag+(aq) | Ag(s)

The free energy change for the following reaction at 25 °C, when [H+] = 1.14 M and [Cr3+] = 5.01×10-3 M, is -442 kJ:6H+(1.14 M) + 2Cr(s)3H2(g) + 2Cr3+(5.01×10-3 M)     ΔG = -442 kJWhat is the cell potential for the reaction as written under these conditions?____________ VWould this reaction be spontaneous in the forward or the reverse direction?

Consider the following galvanic cell: Li (s) | 0.095M LICI (aq) || 0.032M Sn(NO3)2 (aq) | Sn (s) Using Appendix H in the textbook, determine the Eof this galvanic cell. cell 5.939 V 3.158 V 2.899 V 2.899 V O - 5.939 V

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