Consider the cell Cd|CdCl2.2H2O|AgCl(s)| HgThe emf of the cell at 15°C is 0.67531 V and temperature coefficient of emf is 0.00065 V deg–1. Calculate the value of heat flow (in Joules/mol) if the process is carried reversibly: [rounded up to first decimal places]Correct answer is between '36127.0,36133.0'. Can you explain this answer?

Question

Consider the cell Cd|CdCl2.2H2O|AgCl(s)| HgThe emf of the cell at 15&deg;C is 0.67531 V and temperature coefficient of emf is 0.00065 V deg&ndash;1. Calculate the value of heat flow (in Joules/mol) if the process is carried reversibly: [rounded up to first decimal places]Correct answer is between '36127.0,36133.0'. Can you explain this answer?

Answer

Calculation of Heat Flow in a Cell
Heat flow in a cell can be calculated using the equation:
$$ q = -nFE $$

Given Data
- Temperature coefficient of emf ($ \alpha $): 0.00065 V deg$^{-1}$
- EMF at 15°C: 0.67531 V
- Temperature: 15°C

Calculations
- Change in temperature ($ \Delta T $): 15°C - 0°C = 15°C
- Number of electrons transferred (n): 2 (as Cd loses 2 electrons)
- Faraday constant (F): 96485 C/mol
$$ q = -nFE $$
$$ q = -2 \times 96485 \times 0.67531 $$
$$ q = -130299.34 \text{ C/mol} $$

Conversion to Joules
- 1 Faraday is equal to 96485 C/mol or 96485 J/mol
- Therefore, 1 C/mol is equal to 1 J/mol
$$ q = -130299.34 \text{ J/mol} $$

Rounded Value
The rounded up value of heat flow is 130299 J/mol, which is equal to 36127.0 J/mol when rounded to the nearest tenth.
Therefore, the correct answer lies between 36127.0 and 36133.0 J/mol.

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