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JEE Main levelSingle correct optionDifficulty 2 of 3td023

One mole of a diatomic ideal gas (no vibrational contribution) is heated at constant pressure from $300 K$ to $420 K$ . With $R = 8.314 J mo l^{- 1} K^{- 1}$ , the change in internal energy is

A $3492 J$
B $998 J$
C $- 2494 J$
D $2494 J$

Answer: D

Δ U = n C_{V} Δ T

for an ideal gas regardless of path:

(1) (\frac{5}{2}) (8.314) (120) = 2494 J

. The value

q_{P} = C_{P} Δ T = 3492 J

is the heat, not

Δ U

.

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