Consider the following cell: Pt|H2(g, 1.985 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.05 V at 25

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Consider the following cell: Pt|H2(g, 0.405 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.15 V at 25 °C and the standard reduction potential of the Ag /Ag half-reaction couple is 0.80 V, calculate the hydrogen ion concentration in the anode compartment.

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Which one of the following redox reactions (as written) willgenerate the highest cell voltage?

A. Pt / H+ (aq, 1.0 M) / H2 (g, 1 atm) // Ag+ (aq, 1.0 M) /Ag
B. Pt / H+ (aq, 1.0 M) / H2 (g, 1 atm) // Cu2+ (aq, 1.0 M) /Cu
C. Ag / Ag+ (aq, 0.5 M) // Ag+ (aq, 0.5 M) / Ag

How will the measured voltage using a Ca2+ -sensitive electrodechange for a constant Ca2+ concentration but increasing ionicstrength?

A. there is no change
B. EISE will be lower for high ionic strength
C. EISE will be higher for high ionic strength

Given the measured cell potential, Ecell, is â0.3653 V at 25 Â°C in the following cell, calculate the H concentration.

Pt (s)|H2(g, 0.761 atm)|H (aq, ? M)||Cd2 (aq, 1.00 M)|Cd (s)

The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, EÂ°, are as follows.

2H+ (aq)+2e- ---> H2 (g)

Cd2+(aq)+2e- ---> Cd (s)

E0=0.00 v E0=-0.403 v

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Consider the following cell: Pt|H2(g, 1.985 atm)|H (aq, ? M)||Ag (aq, 1.00 M)|Ag(s) If the measured cell potential is 1.05 V at 25

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