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First Law of Thermodynamics

What is the c...

Question

What is the change in internal energy when a gas contracts from $377$ mL to $177$ mL under a constant pressure of 2 atm, while at the same time being cooled by removing $124 J$ heat?
[Take: $1 L a t m$ = $100 J$ ]

- 24 J

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- 84 J

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- 164 J

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- 24 J

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Solution

The correct option is B $- 84 J$
From the first law of thermodynamics,
$△ U = Q + W$
$Q = - 124 J$ (given)
$W = - P_{e x t} (v_{2} - v_{1})$
$- 2 (177 - 377) = 400 a t m m L = 0.4 a t m L$

Since, $1 a t m L = 100 J$
$0.4 a t m L = 40 J$
Substituting the values of $Q a n d W$ , we get,
$△ U = - 124 + 40 = - 84 J$

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First Law of Thermodynamics

Standard XII Chemistry

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What is the change in internal energy when a gas contracts from 377 mL to 177 mL under a constant pressure of 2 atm, while at the same time being cooled by removing 124 J heat? [Take: 1 L atm = 100 J]

The correct option is B −84 JFrom the first law of thermodynamics, △U=Q+W Q=−124 J (given) W=−Pext (v2−v1) −2(177−377)=400 atm mL=0.4 atm L Since, 1 atm L = 100 J 0.4 atm L=40 J Substituting the values of Q and W, we get, △U=−124+40=−84 J

What is the change in internal energy when a gas contracts from $377$ mL to $177$ mL under a constant pressure of 2 atm, while at the same time being cooled by removing $124 J$ heat?
[Take: $1 L a t m$ = $100 J$ ]