Two moles of an ideal gas undergoes Isothermal expansion when heat is

1.	Two moles of an ideal gas undergoes Isothermal expansion when heat is supplied to It. If the gas is at room temperature (298K) and the final volume is thrice the Initial volume, find the total heat supplied.
Answer» No of moles, n = 2 temperature, T = 298K let initial volume = V_i ∴ final volume, V_f = 3V_i The work done for isothermal process is given by, W = 2.303 nRT log₁₀ \((\frac{v_2}{v_1})\) where V₂ is the final volume and V₁ is the initial volume. Here \(\frac{v_2}{v_1}\) = \(\frac{v_f}{v_i}\) = 3 ∴ W = 2.303 × 2 × 8.314 × 298 × \({log^3_{10}}\) W = 5.44kJ Since, for isothermal process, Heat supplied is equal to work done by the gas, the total heat supplied is 5.44 kJ.

Two moles of an ideal gas undergoes Isothermal expansion when heat is supplied to It. If the gas is at room temperature (298K) and the final volume is thrice the Initial volume, find the total heat supplied.

Answer»

No of moles, n = 2

temperature, T = 298K

let initial volume = V_i

∴ final volume, V_f = 3V_i

The work done for isothermal process is given by,

W = 2.303 nRT log₁₀ \((\frac{v_2}{v_1})\)

where V₂ is the final volume and V₁ is the initial volume.

Here \(\frac{v_2}{v_1}\) = \(\frac{v_f}{v_i}\) = 3

∴ W = 2.303 × 2 × 8.314 × 298 × \({log^3_{10}}\)

W = 5.44kJ

Since, for isothermal process, Heat supplied is equal to work done by the gas, the total heat supplied is 5.44 kJ.

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Two moles of an ideal gas undergoes Isothermal expansion when heat is supplied to It. If the gas is at room temperature (298K) and the final volume is thrice the Initial volume, find the total heat supplied.

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