Use standard reduction potentials to calculate the equilibrium constant for the reaction: Cd²+ (aq) + Hg(1)→ Cd(s) + Hg²+ (aq) From the table of standard reduction potentials: E =-0.403 V, EHg²+ /Hg = = 0.855 V Cd²+/Cd Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K: AGO for this reaction would be than zero.

Balance the following reaction in acidic solution. Fe?+ (ag) + MnO, (aq) → Fe+ (ag) + Mn²+(aq) Fill in the coefficients and substances for the balanced overall equation. Note: Do NOT leave any coeffient fields empty. If the coefficient is 1, choose "1" as opposed to leaving it blank. Fe2+ + MnO,¯ + 4 Fe3+ + Mn2+ +

For the cell shown, the measured cell potential, Ecell, is -0.3619 V at 25 °C. Pt(s) | H₂(g, 0.721 atm) | H¹ (aq, ? M) || Cd²+ (aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are 2 H+ (aq) + 2 e H₂(g) Eº = 0.00 V Cd²+ (aq) + 2e → Cd(s) E° = -0.403 V Calculate the H+ concentration. [H+] = TOOLS x10 M

Give only typing answer with explanation and conclusion

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy for the following redox reaction. Round your answer to 3 significant digits. The final units should be in kj

Using the following standard reduction potentials: Ag+ (aq) + e- ⇌ Ag (s) E o = +0.80 V Pb2+ (aq) + 2e - ⇌ Pb (s) Eo = -0.13 V i. Write a balanced redox reaction that represents the overall cell reaction for the feasible galvanic cell. ii. Calculate the standard cell potential. iii. Draw a fully labelled galvanic cell for this redox system. Your labels should show (but not limited to): the electron and ion flow; the anode and cathode, the half cells where oxidation and reduction take place. B. Describe the process involved in electroplating a silver coin.

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)

Mn(s)|Mn2+(aq)||Cr3+(aq)| Cr(s) Calculate the cell potential at 25oC if the concentration of Mn2+(aq) is 2.40 M and the concentration of Cr3+(aq) is 0.500 M. Report your answer to 3 significant figures. Use theStandard Reduction Potentials Table as needed.

Calculate the equilibrium constant, K, for the reaction shown at 25 °C. Fe+(aq)+B(s) + 6 H, O(1) → Fe(s) + H,BO,(s) + 3 H,O*(aq) The balanced reduction half-reactions for the equation and their respective standard reduction potential values (E") are Fe3+ (aq) + 3 e- → Fe(s) H,BO, (s) + 3 H,0*(aq) + 3 e- – B(s) + 6 H, O(1) E' = -0.04 V E' = -0.8698 V K =

I need hand written solution only otherwise I will down vote