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Standard XII

Chemistry

Relation between Cp and Cv

In the figure...

Question

In the figure, a cyclic process ABCA of 3 moles of an ideal gas is given. The temperatures of the gas at B and C are 500 K and 1000 K respectively. If the work done on the gas in process CA is 2500 J, then find the net heat absorbed or released by an ideal gas. Take $R = 25 / 3 J / m o l - K$

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Solution

The change in internal energy during the cyclic process is zero. Hence, the heat supplied to the gas is equal to the work done by it. Hence,
$Δ Q = W_{A B} + W_{B C} + W_{C A}$ .....(i)
The work done during the process AB is zero
$W_{B C} = P_{B} (V_{C} - V_{B})$
$= n R T (T_{C} - T_{B})$
$= (3 m o l) (25 / 3 J / m o l - K) (500 K)$
$= 12500 J$
As $W_{C A} = - 2500 J (g i v e n)$
$∴ Δ Q = 0 + 12500 - 2500$ [From .....(i)]
$Δ Q = 10 k J$

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In the figure, a cyclic process ABCA of 3 moles of an ideal gas is given. The temperatures of the gas at B and C are 500 K and 1000 K respectively. If the work done on the gas in process CA is 2500 J, then find the net heat absorbed or released by an ideal gas. Take R=25/3J/mol−K

In the figure, a cyclic process ABCA of 3 moles of an ideal gas is given. The temperatures of the gas at B and C are 500 K and 1000 K respectively. If the work done on the gas in process CA is 2500 J, then find the net heat absorbed or released by an ideal gas. Take $R = 25 / 3 J / m o l - K$