Calculate the emf (in Volt) of the above cell. Assume the temperature of the laboratory to be 2 5 ∘ C and the solutions are dilute enough so that molar concentrations can be used instead of activities of the solutions.

1.109 = 1.100 − 2 0.06 lo g [ C u 2 + ] 0.1 [ C u 2 + ] = 0.2 M Δ n = 0.2 × 0.1 − 0.1 × 0.1 = 0.01 w = 0.01 × 135 = 1.35 g m

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ChemistryElectrochemistryGalvanic cells/Nernst Equation/Concentration CellsMedium2 minQB

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Passage / Comprehension

The most popular electrochemical cell, Daniel cell was originally developed by the English chemist John F. Daniel. The general assembly of the cell is as given below

An undergraduate student up a Daniel cell using 100 cm³ of 0.100 M $C u S O_{4}$

and 0.100 M $Z n S O_{4}$ solution respectively. The two compartments are connected by suitable salt bridge.

[Given: $E_{C u^{2 +} / C u}^{\circ} = 0.34 V$ , $E_{Z n^{2 +} / Z n}^{\circ} = - 0.76 V$ , $\frac{2.303 RT}{F} = 0.06$ , $lo g 2 = 0.3$ ]

Calculate the emf (in Volt) of the above cell. Assume the temperature of the laboratory to be $2 5^{\circ} C$ and the solutions are dilute enough so that molar concentrations can be used instead of activities of the solutions.

Options:

Answer:

Solution:

$1.109 = 1.100 - \frac{0.06}{2} lo g \frac{0.1}{[ C u ^{2 +} ]}$

$[C u^{2 +}] = 0.2 M$

$Δ_{n} = 0.2 \times 0.1 - 0.1 \times 0.1 = 0.01$

$w = 0.01 \times 135 = 1.35 g m$

Stream:JEESubject:ChemistryTopic:ElectrochemistrySubtopic:Galvanic cells/Nernst Equation/Concentration Cells

⏱ 2mℹ️ Source: QB

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