Based on the sign of the standard cell potential, E, 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 Ni* (aq) + Pb(s) → Ni(s) + Pb²*(aq) 3 Fe?+ (aq) + 2 Cr(s) →3 Fe(s) + 2 Cr*(aq) AP*(aq) + 3 Na(s) → Al(s) + 3 Na* (aq)

A galvanic (voltaic) cell consists of an electrode composed of aluminum in a 1.0 M aluminum ion solution and another electrode composed of gold in a 1.0 M gold(III) ion solution, connected by a salt bridge. Calculate the standard potential for this cell at 25 °C. Refer to the list of standard reduction potentials. Excell V

Calculate the cell potential for the reaction as written at 25.00 degrees * C , given that [Zn^ 2+ ]=0.81 and [Sn^ 2+ ]=0.0190M M. Use the standard reduction potentials in this table. Zn(s)+ Sn ^ 2+ (aq) rightleftharpoons Zn^ 2+ (aq)+Sn(s)

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. 21 (aq) + Cl2(g) → 2(s) + 2CI(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: In the external circuit, electrons migrate v the Cl2 electrode v the I electrode. Anions migrate v the salt bridge v the Cl2 compartment.