What is the cell potential at 25 oC for the following voltaic cell? Cr(s)│Cr3+(1.0 M)║Cu2+(0.001 M│Cu(s)

What is the cell potential of the following electrochemical cell? (Report your answer to 2 significant figures.) Co(s) | Co²+ (aq, 0.31 M || Co²+ (aq, 0.035 M) | Co(s) Co²+/Co(s) = -0.28 V Eºred 1 2 4 7 +/- 5 8 v 3 6 9 0 X с x 100

Use an inactive electrode when needed. Consider the following cell reactions and its standard cell potential: 3 Hg22+(aq) + 2 Cr3+(aq) ⟶⟶2 Cr(s)  + 6 Hg2+(aq)       E°cell = -1.66 V a) Write the cell notation for the voltaic cell.  b) What are the stoichiometric number of moles of electrons delivered from the one electrode compartment to the other? c) Draw a diagram of the voltaic cell.  Label the anode and cathode compartments and the sign of each.Label what ions, gases, and solids are in each compartment.Label the electrode in each compartment. In other words, what is conducting electrons in and out of each compartment.Label the direction of electron flow.Label the salt bridge and what ionic compound is being used in the salt bridge.  Label the direction of the ion flow for the cation and anion of the salt bridge.

MnO4– + Sn ----> MnO2 + Sn2+ A) Identify the half-reaction that occurs at the cathode. B) Identify the oxidizing agent and anode. C) standard cell potential? D) What will be the potential of a cell constructed using 57.0 g MnO2, 1.57 M MnO4–, 14.8 g Pt, 12.5 g Sn and 0.87 M Sn2+ at pH 2.5?

The cell potential was 1.271 V at 25oC and a Al3+(aq) concentration of 0.178 M. What was the hydronium ion concentration? The H2(g) pressure was 1 atm at 25oC.6H+(aq) + 2Al(s) ↔ 2Al3+(aq) + 3H2(g) Ecoell = 1.660 V

Use the tabulated half-cell potentials to calculate ΔG° for the following reaction. (Hint: Before you being, you must determine whether or not the reaction is balanced.)I2(s) + Fe(s) → Fe3+(aq) + I⁻(aq) (a)‒1.1×102kJ (b) +4.9×101kJ (c) ‒9.7×101kJ (d) ‒3.3×102kJ