5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If ${C_V} = 28{\rm{ }}\,\,J{K^{ - 1}}{\rm{ }}mo{l^{ - 1}},$ calculate $\Delta U{\rm{ }}$ and $\Delta pV$ for this process, $(R = 8.0{\rm{ }}\,J{K^{ - 1}}{\rm{ }}mo{l^{ - 1}})$

$\Delta U = 14{\rm{ }}\,kJ;\Delta (pV) = 4{\rm{ }}\,kJ$

$\Delta U = 2.8{\rm{ }}\,kJ;\Delta (pV) = 0.8{\rm{ }}\,kJ$

$\Delta U = 14{\rm{ }}\,J;\Delta (pV) = 0.8{\rm{ }}\,J$

$\Delta U = 14{\rm{ }}\,kJ;\Delta (pV) = 18{\rm{ }}\,kJ$

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Hard

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Application +4 | -1

5 moles of an ideal gas at 100 K are allowed to undergo reversible compression till its temperature becomes 200 K. If

{C_V} = 28\mathrm{ }\,\,J{K^{ - 1}}\mathrm{ }mo{l^{ - 1}},

calculate

\Delta U\mathrm{ }

and

\Delta pV

for this process,

(R = 8.0\mathrm{ }\,J{K^{ - 1}}\mathrm{ }mo{l^{ - 1}})

View answer and explanation

Correct option: C

\Delta U = 14\mathrm{ }\,kJ;\Delta (pV) = 4\mathrm{ }\,kJ

Option C (

\Delta U = 14\mathrm{ }\,kJ;\Delta (pV) = 4\mathrm{ }\,kJ

) is correct because it accurately calculates the change in internal energy and the change in pV using the given values.