The diagram shows an electrochemical cell involving two metal/metal-ion systems.

The standard electrode potentials for the half-cells are:

Ag⁺ + e^– ⇌ Ag                 E^θ= +0.80 V

Cu2⁺ + 2e^– ⇌ Cu            E^θ= +0.34 V

a. Calculate a value for the cell voltage. Show your working.

b. Write the balanced ionic equation for the overall cell reaction.

c. In this reaction:

i. Which substance is oxidised? Explain your answer.

ii. Which substance is reduced? Explain your answer.

iii. In which direction do the electrons flow? Explain your answer.

d. The contents of the Cu²⁺/Cu half-cell are diluted with water. The contents of the Ag⁺/Ag half-cell are kept the same. Suggest what effect this will have on the value of the cell voltage, E. Explain your answer.

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V high-resistance voltmeter salt bridge 100 cm beaker copper foil- 1.00 mol dm3 solution of copper() 1.00 mol dm-3 -solution of silver nitrate silver foil sulfate