2. Decide if the following reactions are spontaneous based on the calculated E° value for the cell. a. Rb + CsCs + Rb+ b. Ag + Au³+ <> Au + Ag+ c. H2Te + Mn2+ Mn + Te + 2H+ d. H₂+ Sn4+ Sn2+ + 2 Ht

Consider the reaction below:2 Ag(aq) + +Fe(s) → 2 Ag(s) + Fe^2+(aq) ΔG° = −241.0kJmol a. Calculate the equilibrium constant for this reaction.b. Calculate the standard cell potential for this reaction.

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…

6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.

Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.

Use cell potential to calculate the standard free energy change for this reaction.  MnO4- (aq) + 8 H+ (aq) + 5 Fe2+ (aq) --> MN2+ (aq) + 4 H2O (l) +5 Fe3+ (s)  a. -357 kJ  b. 357 kJ c. 941 kJ  d. -941 kJ  e. 1130 kJ