An ideal gas expands against a constant external pressure of $2.0$ atmosphere from $20$ litre to 40 litre and absorbs $10 k J$ of heat from surrounding. What is the change in internal energy of the system? (Given : 1 atm litre $= 101.3 J$ )

4052 J

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5948 J

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14052 J

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9940 J

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Solution

The correct option is B $5948 J$
Here gas is expanded against constant pressure. So, it is a irreversible system.
$∴$ work done $= - P \times Δ V$
$\Rightarrow w = - 2 a t m \times 20 L i t r e$
$= - 40 a t m . L i t r e = - 40 \times 101.3 J = - 4052 J$
$Δ U = q + w$
$= 10 \times 1000 - 4052 = 5948 J$

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An ideal gas expands against a constant external pressure of 2.0 atmosphere from 20 litre to 40 litre and absorbs 10 kJ of heat from surrounding. What is the change in internal energy of the system? (Given : 1 atm litre =101.3 J)

The correct option is B 5948 JHere gas is expanded against constant pressure. So, it is a irreversible system. ∴ work done =− P×ΔV ⇒w=−2 atm× 20 Litre =−40 atm. Litre =−40×101.3 J=−4052 J ΔU=q+w =10×1000−4052=5948 J

An ideal gas expands against a constant external pressure of $2.0$ atmosphere from $20$ litre to 40 litre and absorbs $10 k J$ of heat from surrounding. What is the change in internal energy of the system? (Given : 1 atm litre $= 101.3 J$ )