Two moles of an ideal gas are expanded isothermally and reversibly from $1$ litre to $10$ litre at $300 K$ . The enthalpy change (in $k J$ ) for the process is:

11.4 k J

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- 11.4 k J

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0 k J

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4.8 k J

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Solution

The correct option is C $0 k J$
$S i n c e, H = E + P V S o, Δ H = Δ E + Δ (P V) S i n c e, P V = n R T S o, Δ H = Δ E + n R Δ T F o r i s o t h e r m a l p r o c e s s, Δ T = 0 F o r r e v e r s i b l e p r o c e s s, Δ E = 0 S o, Δ H f o r t h i s e x p a n s i o n = 0 k J S o, c o r r e c t a n s w e r i s o p t i o n C .$

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