Electrochemical Cells & EMF Mock Tests

17 questions available

Electrochemical Cells & EMF Mock Test 1

Questions: 17

Sample Questions

CUET Chemistry

The standard electrode potential for the Cu²⁺/Cu half-cell is +0.34 V. What is the standard Gibbs free energy change (ΔG°) for the reaction Cu²⁺(aq) + 2e⁻ → Cu(s) at 298 K? (F = 96500 C mol⁻¹)

A −65.62 kJ mol⁻¹

B −32.81 kJ mol⁻¹

C +65.62 kJ mol⁻¹

D −329.4 kJ mol⁻¹

CUET Chemistry

The standard electrode potential (E°) of a cell is defined as:

A EMF of the cell when all concentrations are 1 M and pressure is 1 atm

B EMF of the cell at any concentration

C The potential of any single electrode

D Sum of all electrode potentials in the cell

CUET Chemistry

A voltaic cell is constructed using: Cu²⁺/Cu (E° = +0.34 V) and Ag⁺/Ag (E° = +0.80 V). Which statement correctly describes this cell under standard conditions?

A Copper acts as the cathode and silver as the anode

B Silver acts as the cathode and copper as the anode; E°cell = +0.46 V

C Both act as cathodes because both have positive reduction potentials

D Silver acts as the anode; E°cell = −0.46 V

CUET Chemistry

The standard electrode potential (E°) of a cell is defined as:

A EMF of the cell when all concentrations are 1 M and pressure is 1 atm

B EMF of the cell at any concentration

C The potential of any electrode

D Sum of all electrode potentials in the cell

CUET Chemistry

The standard Gibbs free energy change (ΔG°) for a cell reaction with n = 2 and E°cell = 0.5 V is: (F = 96500 C mol⁻¹)

A −96.5 kJ mol⁻¹

B −193 kJ mol⁻¹

C +96.5 kJ mol⁻¹

D −48.25 kJ mol⁻¹

CUET Chemistry

A concentration cell is made of two silver electrodes: Ag|Ag⁺(0.001 M)||Ag⁺(0.1 M)|Ag. What is the cell potential at 298 K?

A 0.118 V

B 0.0591 V

C 0.236 V

D 0.02955 V

CUET Chemistry

A concentration cell is constructed using two hydrogen electrodes: Pt|H₂(1 atm)|H⁺(0.001 M) || H⁺(0.1 M)|H₂(1 atm)|Pt. What is the EMF of this cell at 298 K?

A 0.118 V

B 0.0591 V

C 0.236 V

D 0.02955 V

CUET Chemistry

For the cell reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), the standard electrode potentials are E°(Cu²⁺/Cu) = +0.34 V and E°(Zn²⁺/Zn) = −0.76 V. What is the standard EMF of the cell?

A −1.10 V

B −0.42 V

C +0.42 V

D +1.10 V

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