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If \Delta U and \Delta W  represent the increase in internal energy and work done by the system respectively in a thermodynamical process, which of the following is true? 

  • Option 1)

    \Delta U=-\Delta W, in an adiabatic process

  • Option 2)

    \Delta U=\Delta W, in an isothermal process

  • Option 3)

    \Delta U=\Delta W, in an adiabatic process

  • Option 4)

    \Delta U=-\Delta W, in an isothermal process

 

Answers (1)

best_answer

Using

First law in Isothermal Process -

Delta Q= Delta U+Delta W
 

- wherein

Isothermal process

Delta T= 0

Delta U= 0

Heat supplied is equal to work done.

 

 and

Adiabatic Process -

When a Thermodynamic System undergoes a change in such a way that no exchange of heat takes place.

- wherein

Delta Q= 0

 

 In adiabatic process, \Delta Q=0

\therefore \Delta U =-\Delta W

In isothermal process, \Delta U = 0


Option 1)

\Delta U=-\Delta W, in an adiabatic process

This option is correct

Option 2)

\Delta U=\Delta W, in an isothermal process

This option is incorrect

Option 3)

\Delta U=\Delta W, in an adiabatic process

This option is incorrect

Option 4)

\Delta U=-\Delta W, in an isothermal process

This option is incorrect

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Aadil

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