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JEE Advanced levelOne or more correct optionsDifficulty 3 of 3td072

One mole of a monoatomic ideal gas is heated from $300 K$ to $600 K$ , once at constant volume and once at constant pressure. Use $R = 8.314 J mo l^{- 1} K^{- 1}$ . Select the correct statement(s).

AThe heat absorbed at constant pressure is about $6.2 kJ$
BThe work done by the gas at constant pressure is about $2.5 kJ$
C $Δ U \approx 3.7 kJ$ in both processes
DThe heat absorbed at constant volume is about $6.2 kJ$

Answer: A, B, C

Δ U = n C_{v} Δ T = 1.5 \times 8.314 \times 300 = 3.7 kJ

for any path (ideal gas). At constant volume

q_{V} = Δ U = 3.7 kJ

; at constant pressure

q_{p} = n C_{p} Δ T = 2.5 \times 8.314 \times 300 = 6.2 kJ

and

w_{b y} = n R Δ T = 2.5 kJ

. So the constant-volume heat is not

6.2 kJ

.

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