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Statement -1: The magnitude of the work ...

Statement -1: The magnitude of the work involved in an isothermal expansion is greater than that involved in an adiabatic expansion.
Statement -2: P-v curve (P on y -axis and V on X-axis) decrease more rapidly for reversible adiabatic expansion compared to reversible isothermal expansion starting from same initial state.

A

Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1

B

Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-1

C

Statement-1 is True, Statement-2 is False.

D

Statement-1 is False, Statement-2 is True.

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Staetement -1: The magniyude of the work involed in an isothermal expansion is greater than that involved in an adiabatic expansion. Statement -2: P-v cure (pon y -axas and V on X-axas) decrease more repidly for reversible asiabatic expansion compared to reversible isothermal expansion starting from same initial state.

Statement-1: The amount of work done in the isothermal expansion is greater than work done in the adiabatic system for same final volume. Statement-2: In the adiabatic expansion of a gas temperature and pressure both decrease due to decrease in internal energy of the system.

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The magnitude of enthalpy changes for irreversible adiabatic expansion of a gas from 1 L to 2 l is Delta H_(1) and for reversible adiabatic expansion for the same expansion is Delta H_(2) . Then

The magnitudes of enthalpy changes for irreversible adiabatic expansion of a gas from 1L to 2L is ∆H_(1) and for reversible adiabatic expansion for the same expansion is ∆H_(2) . Then

State true or false. Work done by an ideal gas in adiabatic expansion is less than that in isothermal process (for same temperature range)

The correct figure representing isothermal and adiabatic expansions of an ideal gas from a particular initial state is :

Calculate the work done during isothermal reversible expansion expansion of one mol of an ideal gas from 10 atm to 1 atm at 300K.

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