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121 solutions

The Nernst Equation

Q. At equilibrium, the reaction below is/has ______________. reactant-favored. product-favored. equal amounts of reactants and products.

Solved • Dec 6, 2019

The Nernst Equation

Q. In a galvanic cell, Zn electrode is immersed in 1.00M Zn(NO3)2. Other half cell is Pt electrode with 1 atm H2 bubbling over it. This cathode is immersed in a solution of unknown H+. The cell voltage is 0.473 V at 298.15 K. What is the pH of the solution where the cathode is immersed?

Solved • Dec 5, 2019

The Nernst Equation

Q. What is the cell potential for the reaction Mg(s)+Fe2+(aq)→Mg2+(aq)+Fe(s) at 85 ∘C when [Fe2+]= 3.30 M and [Mg2+]= 0.310 M .

Solved • Dec 5, 2019

The Nernst Equation

Q. A concentration cell is constructed using two metal (M) electrodes with M^2+ concentrations of 0.10 M and 1.00x10^-5 M in the two half-cells. Determine the reduction potential of M^2+ given that the potential of the cell at 25 degrees Celcius is 0.118 V.

Solved • Dec 4, 2019

The Nernst Equation

Q. I need help understanding and basic solution to this problem regarding electrochemistry,

Solved • Dec 4, 2019

The Nernst Equation

Q. The reduction potentials for Ni2+ and Sn2+ are as follows: Ni2+ + 2 e- → Ni E° = -0.233 V Sn2+ + 2e- → Sn E° = -0.140 V Calculate the equilibrium constant at 25°C for the reaction: Sn 2+ + Ni ⇌ Sn + Ni2+

Solved • Dec 4, 2019

The Nernst Equation

Q. Consider an electrochemical cell with a zinc electrode immersed in 1.0M Zn^2+ and a nickel electrode immersed in 0.10 M Ni^2+. Zn^2+ + 2e^-→Zn E° = -0.76 V Ni^2+ + 2e^-→Ni E° = -0.23 V Calculate the concentration of Ni2+ if the cell is allowed to run to equilibrium at 25°C.

Solved • Dec 4, 2019