What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H, pressure is 3.37×10-3 atm, the H* concentration is 1.04M, and the Mg2+ concentration is 7.01×10-4M ? 2H (аq) + Mg(s)—— Н2(g) + - Mg2*(aq) Answer: The cell reaction as written above is spontaneous for the concentrations give v true false Submit Answer Retry Entire Group 9 more group attempts remaining

Can you please answer these two sub problems and show all of the steps to the solution

Practice: will the reaction be spontaneous? If not write the spontaneous direction, and calculate the Ecell. Sketch the cell and write the line notation of the spontaneous reaction. Zn + Ca2+ → Zn2+ + Ca a) Spontaneous b) Not spontaneous c) Not sure Zn2+(aq) + 2e Zn(s) -0.76 Cr³+ (aq) + 3e Cr(s) -0.73 2 H₂O(l) + 2e Mn2+( Al3+(aq) + 3e Mg2+(aq) + 2e H2(g) +20H(aq) -0.83 +(aq) + 2e¯ Mn(s) -1.18 Al(s) -1.66 Mg(s) -2.37 Na+ (aq) + e Na(s) -2.71 Ca2+ (aq) + 2e →Ca(s) -2.76

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