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Electrochemical Cells & EMF Mock Tests

17 questions available

Electrochemical Cells & EMF Mock Test 1

Questions: 17

नमूना प्रश्न

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
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
For a galvanic cell at equilibrium, which of the following is true?
A E_cell = 0 and ΔG = 0
B E_cell = 0 and ΔG < 0
C E_cell > 0 and ΔG = 0
D E_cell < 0 and ΔG < 0
CUET Chemistry
The Nernst equation for a half-cell reduction reaction is used to calculate:
A Electrode potential at non-standard conditions
B Standard electrode potential
C Cell entropy change
D Equilibrium constant only
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
CUET Chemistry
For the cell reaction Zn(s) + Cu²⁺(0.1 M) → Zn²⁺(0.01 M) + Cu(s), given E°cell = 1.10 V, what is Ecell at 298 K? (Use 2.303RT/F = 0.059 V)
A 1.10 V
B 1.08 V
C 1.12 V
D 0.98 V
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
For the Daniel cell (Zn|Zn²⁺(1 M)||Cu²⁺(1 M)|Cu), E° = 1.10 V. What happens to E_cell when the concentration of Zn²⁺ is increased to 10 M while Cu²⁺ remains at 1 M?
A E_cell increases to 1.159 V
B E_cell decreases to 1.070 V
C E_cell remains 1.10 V
D E_cell becomes zero

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