Electrochemistry
EMF, Nernst equation, galvanic cells, conductance, Faraday's laws.
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Take a full mock →Q1 · Electrochemistry · MEDIUM
The number of Faradays of electricity required to deposit 1 mole of copper from a Cu²⁺ solution is:
Q2 · Electrochemistry · EASY
The function of a salt bridge in a galvanic cell is to:
Q3 · Electrochemistry · EASY
A galvanic cell is constructed with a zinc electrode (Zn²⁺/Zn) and a silver electrode (Ag⁺/Ag). Given that E°(Zn²⁺/Zn) = -0.76 V and E°(Ag⁺/Ag) = +0.80 V, what is the standard EMF of the cell?
Q4 · Electrochemistry · MEDIUM
Calculate the EMF of the cell at 25°C: Zn | Zn²⁺(0.01 M) || Cu²⁺(0.1 M) | Cu. Given: E°(Zn²⁺/Zn) = -0.76 V, E°(Cu²⁺/Cu) = +0.34 V, and 2.303RT/F = 0.059 V at 25°C.
Q5 · Electrochemistry · HARD
During the electrolysis of aqueous copper sulfate solution using copper electrodes, 0.635 g of copper is deposited at the cathode. How many coulombs of electricity were passed through the solution? (Atomic mass of Cu = 63.5 g/mol, F = 96500 C/mol)