Consider the following cell reaction: Cd(s) + 2 H*(? M) Cd2+ (1.00 M) + H2(g)(1.00 atm) If the cell potential at 298 K is 0.212 volts, what is the pH of the hydrogen electrode? pH= =

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

Name: NetID: 5. Determine the standard cell potential (in V to two decimal places) for the following redox reactions. 2+ (a) Al(s) | Al³+ (aq, 1 M) || Cu²+ (aq, 1 M) | Cu(s) (b) Al(s) + NO3(aq) + 4H+ (aq) - Al³+ (aq) + NO(g) + 2H₂O(1) 13+ A: 2.00 A: 2.62

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Zn (aq)+2e - Zn(s) :-0.763 V (red |Cro (aq)+4 H2O(1)+3e Cr(OH)3(s)+5OH (aq) :-0.13 V = - (red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. x10 Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.

Use standard reduction potentials to calculate the equilibrium constant for the reaction: 2+ Cu²+ (aq) + 21 (aq) → Cu(s) + I₂ (s) From the table of standard reduction potentials: Cu²+/Cu 0.337 V, E₁₂/1 Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. Equilibrium constant at 298 K:I AGO for this reaction would be than zero. = = 0.535 V