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The Nernst Equation

Solved • Apr 21, 2020

The Nernst Equation

#### Q. Calculate E cell of this electrochemical cell under non-standard conditions: Zinc-Copper

Solved • Apr 21, 2020

The Nernst Equation

#### Q. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the H2 pressure is 8.70×10-3 atm, the H+ concentration is 1.18M, and the Pb2+ concentration is 3.41×10-4M ? 2H+(aq) + Pb(s) H2(g) + Pb2+(aq) Answer: ____V The cell reaction as written above is spontaneous for the concentrations given: true/false

Solved • Apr 14, 2020

The Nernst Equation

#### Q. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the Cl2 pressure is 7.61×10-4 atm, the Cl- concentration is 1.19M, and the Ni2+ concentration is 1.03M ? Cl2(g) + Ni(s)2Cl-(aq) + Ni2+(aq) Answer: ___V The cell reaction as written above is spontaneous for the concentrations given:true/false

Solved • Apr 14, 2020

The Nernst Equation

#### Q. For the reaction °= 2Co^3+ (aq) + 2Cl^-(aq) → 2Co^2+ (aq) + Cl2(g) • E° = 0.483 V what is the cell potential at 25 °C if the concentrations are [Co^3+] = 3.40x10^-2 M, [Co^2+] = 4.40x10^-2 M, and [Cl^-] = 0.846 M, and the pressure of Cl2 is PCl2 = 9.40 atm? Express your answer with the appropriate units.

Solved • Apr 6, 2020

The Nernst Equation

#### Q. Consider the reaction Mg(s) + Fe^2+(aq) → Mg^2+(aq) + Fe(s) at 47°C, where [Fe^2+] = 3.10 M and [Mg^2+] = 0.310M. What is the value for n? Express your answer as an integer and include the appropriate units (i.e. enter mol for moles).

Solved • Apr 6, 2020

The Nernst Equation

#### Q. What is the calculated value of the cell potential at 298K for an electrochemical cell with the following reaction, when the F2 pressure is 1.26 atm, the F^- concentration is 7.88 x 10^-3 M, and the Ag^+ concentration is 6.24 x 10^-4 M? F2(g) + 2Ag(s) → 2.00F^-(aq) + 2Ag^+(aq) The cell reaction as written above is spontaneous for the concentrations given:

Solved • Apr 1, 2020