Assertion : In an isolated system,the entropy | vedclass

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(B) According to the $Second$ $Law$ of $Thermodynamics$,for any spontaneous process in an isolated system,the entropy of the system must increase $(dS

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If both $Assertion$ and $Reason$ are correct but $Reason$ is not a correct explanation of the $Assertion$.

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(B) According to the $Second$ $Law$ of $Thermodynamics$,for any spontaneous process in an isolated system,the entropy of the system must increase $(dS > 0)$.An isolated system is defined as a system that cannot exchange energy (heat or work) or matter with its surroundings.Since an adiabatic process is defined as a process where there is no exchange of heat $(dQ = 0)$ between the system and the surroundings,all processes occurring within an isolated system are indeed adiabatic.However,the fact that the processes are adiabatic does not directly explain why the entropy must increase; the increase in entropy is a consequence of the $Second$ $Law$ of $Thermodynamics$ regarding spontaneous processes.Therefore,both statements are correct,but the $Reason$ is not the correct explanation for the $Assertion$.

$Assertion :$ In an isolated system,the entropy increases.
$Reason :$ The processes in an isolated system are adiabatic.

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$Assertion :$ In an isolated system,the entropy increases.$Reason :$ The processes in an isolated system are adiabatic.