1. Sketch an electrochemical cell that uses the given reaction. Label the anode and cathode; indicate the direction of electron flow; write a balanced equation for the cell reaction; and calculate E°cell, AG° and K. NO3^- (aq) + H^+(aq) + Zn(s) -> Zn^2+ (aq) + NO(g) + H20(l) 2. The given cell reaction is spontaneous at standard state. True or False? 3. Which is favored by the cell reaction? Reactants or Products?

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:

Can you break down the problem attached?

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:

For the cell: Zn(s) + 2H† (aq) →→ Zn2+(aq) + H2 (g) If [Zn2+] = 1 M, PH2 = 1 atm, and E = 0.123 V what is pH?

A galvanic cell is prepared using copper and silver. Its cell notation is shown below: Cu(s) | Cu2+(aq) || Ag+(aq) | Ag(s)  Which of the following processes occurs at the cathode?    A. Cu(s) → Cu2+(aq) + 2e-   B. Cu2+(aq) + 2e-  → Cu(s)   C. Ag+(aq) + e-  → Ag(s)    D. Ag(s)  → Ag+(aq) + e-   E. Cu(s) + 2Ag+(aq)  → Cu2+(aq) + 2Ag(s)       Copper is electroplated from a CuSO4 solution. A constant current of 4.54 A is applied by an external power supply. How long (minutes) will it take to deposit 0.985 g of Cu? (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 120. and -123 and 123. and 12.3)     DOnt need work shown just answer asap        Predict the sign of ΔSorxn (positive or negative) for the following reactions:                                       CH3OH(l)  →  CH3OH(s)                                       CH4(g) + H2O(g)  →  CO(g) + 3…

Write the cell notation for an electrochemical cell consisting of an anode where Ni (s) is oxidized to Ni2+ (aq) and a cathode where Cu2+ (aq) is reduced to Cu (s) . Assume all aqueous solutions have a concentration of 1 mol/L.

Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these

A voltaic cell is based on a nitrate/NO half-cell and a NiCl2/Ni half-cell. (Heads up, the chloride ions in this reaction are bystander ions.) Eo for NO-3 (aq) → NO(g) = +0.96 Eo for NiCl2 (aq) → Ni(s) = –0.28  What is the cell potential of the reaction when pH = 2.7, [NO3-] = 1.5 M, PNO = 0.010 atm and [Ni2+] = 0.21 M