12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction...
Calculate the standard cell potential and determine if the reaction is spontaneous in the forward direction(as written). Identify each oxidizing agent and reducing agent. Ni (s) + Zn2+(aq) ----> Ni2+(aq) + Zn (s) Ni (s) + Pb2+(aq) -------> Ni2+(aq) + Pb (s) Al (s) + 3 Ag+(aq) ---------> Al3+(aq) + Ag (s) Pb (s) + Mn2+(aq) ----------> Pb2+(aq) + Mn (s)
Based on the sign of the standard cell potential, Ecell, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Refer to the list of standard reduction potentials. Spontaneous as written Nonspontaneous as written Answer Bank Au + (aq) + 3 Ag(s) Au(s) + 3 Ag* (aq) 1,(s) + Cu() — 21(aq) + Cu2+ (aq) Ni2+ (aq) + Pb(s) Ni(s) + Pb2+ (aq)
2. Calculate the standard cell potential for each of the following redox reactions, and then predict whether each will occur spontaneously as written. a. Sr(s) + Fe2+(aq) → Sr2+ (aq) + Fe(s) b. 2Cr(s) + 3Cd2+ (aq) → 2Cr3+ (aq) + 3Cd(s) 3. Calculate the standard cell potential, Eºcell, for each of the voltaic cells in Part II of the experiment. a. Zn(s) | Zn2+ (aq, 1.0 M) || Cu2+ (aq, 1.0 M) Cu(s) b. Zn(s) | Zn2+(aq, 1.0 M)...
Consider the following redox reactions. For each reaction, calculate the standard cell potential. See Table 12-2 from your book for a list of standard reduction potentials (or lecture notes CH12). A. Ag+ + Fe2+à Fe3+ + Ag(s) B. Zn2+ + Ni(s) à Ni2+ + Zn(s) C. 2Al3+ + 3Cu(s) à 2Al(s) + 3Cu2+
Calculate the cell potential for the following reaction as written at 25.00 °C, given that [Zn2+ ] = 0.850 M and [Ni2+ ] = 0.0130 M. Standard reduction potentials can be found here. Zn(s) + Ni2+(aq)Zn2+(aq) + Ni(s)
Based on the sign of the standard cell potential, Eco, classify these reactions as spontaneous or nonspontaneous as written. Assume standard conditions. Spontaneous as written Nonspontaneous as written Au + (aq) + 3 Ag(s) + Au(s) + 3 Ag+ (aq) Ni²+ (aq) +52- (aq) Ni(s) +S(s) Pb2+ (aq) + H, (g) → Pb(s) + 2 H+ (aq) Answer Bank
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.800 M and [Ni2+] = 0.0110 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+ (aq) = Zn2+ (aq) + Ni(s) E = _______ V
Calculate the cell potential for the reaction as written at 25.00 °C, given that (Zn2+] = 0.885 M and [Ni2+] = 0.0190 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+ (aq) = Zn2+ (aq) + Ni(s) Ev
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.839 M and [Ni2+] = 0.0150 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+(aq) = Zn2+ (aq) + Ni(s) E = V
Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn2+] = 0.777 M and (Ni2+1 = 0.0190 M. Use the standard reduction potentials in this table. Zn(s) + Ni2+ (aq) = Zn2+ (aq) + Ni(s) V E=