Question

Statement 1 : For an isothermal reversible process Q = –W
i.e. work done by the system equals the heat absorbed by
the system.
Statement 2 : Enthalpy change (DH) is zero for isothermal
process. [AIIMS 2013]

Answer 1

Assertion is correct but Reason is wrong

Answer 2

Assertion is correct bu reason is incorrect.

Step by step explanation:

• According to the thermodynamics,internal energy is expressed by the following expression.

         $\bold{Q+W=\Delta E}$..........................(1)

• Change in internal energy is indicated by $\bold{\Delta E}$.
• The internal energy is zero in isothemal reversible process.
• Substitute the internal energy value in equation (1)

                                 $Q+W=0$

                                            $\Rightarrow Q= -W$

• If a system undergoes a change in which internal energy of the system remains constant

Then we get, $\Rightarrow -W=Q$

Hence, statement -1 is correct.

• When internal energy is zero, $\Delta H$ need not to be zero as work done may or may not be zero.

Hence, statement -2 is incorrect.

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