Zn(s)|ZnO(s)|KOH(aq)||Ag2O(s)||Ag(s) Write the half‑reaction equation that involves silver. half‑reaction: Write the half‑reaction equation which involves zinc. half‑reaction: Write the balanced equation for the net cell reaction equation. net cell reaction:   Calculate the value of ?∘cellEcell∘ . Standard potentials can be found in the hint.   ?∘cell :

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Br2(1) + Mn(s) 2Br"(aq) + Mn2+(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 the Mn electrode the Br2 electrode. Anions migrate the salt bridge the Br2 compartment.

Write the net cell equation for the electrochemical cell. Phases are optional. Do not include the concentrations. Co(s)|Co #(aq, 0.0155 M) || Ag*(aq, 1.50 M)|Ag(s) net cell equation:

A particular voltaic cell operates on the reaction Zn(s) + Cl, (9) → Zn+ (aq) + 2C1 (aq) giving a cell potential of 0.763 V. Calculate the maximum electrical work generated when 17.0 g of zinc metal is consumed. Maximum electrical work-

Calculate the cell potential for a Galvanic cell based on the reaction described by the following unbalanced equation at 25 C (assume standard, acidic conditions). Cu(s) + MnO4-(aq) -> Cu2+(aq) + MnO2(s)

Write the half-reactions as they occur at each electrode and the net cell reaction for this electrochemical cell containing indium and cadmium.   In(s)||In3+(aq)‖‖Cd2+(aq)||Cd(s)In(s)⁢|In3+⁢(aq)‖Cd2+⁢(aq)|Cd(s)   anode:   cathode:   net cell reaction:

Consider a voltaic cell in which the reaction is Zn (s) + 2H+ (aq) → Zn2+ (aq) + H2 (g)   It is found that the cell voltage is +0.530 V when [Zn2+] = 1.0 M, PH2 = 1.0 atm. What must be the concentration of H+ in the cell? (Use the following information)   (Show your work)                                                                                        2H+ (aq) + 2e- → H2 (g)          Eºred = 0.000 V   Zn2+ (aq) + 2e- → Zn(s)         Eºred = -0.762 V

Consider the voltaic cell with a standard potential of 0.25V: Ni | Ni2+ (1.0 M) | H+ (1.0 M) | H2 (1 atm) | Pt   what is the value of the equilibrium constant for the reaction at 298 K?

Write the net cell equation for this electrochemical cell. Phases are optional. Do not include the concentrations. Cu(s)|Cu2+(aq, 0.0155 M)‖Ag+(aq, 3.50 M)|Ag(s) net cell equation:  Calculate Ecell∘, ΔGrxn∘, ΔGrxn, and Ecell at 25.0 ∘C

Will the cell reaction proceed spontaneously as written for the following cell?    Sn (s)  |  Sn2+ (0.50 M)  ||  Pb2+ (0.0010 M)  |  Pb (s)                 b) What is the value of for the cell reaction?