For an adiabatic process

Δ S = 0

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Δ U = 0

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Q = 0

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W = 0

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Solution

The correct option is A $Δ S = 0$
During an adiabatic process, there is no exchange of energy between system and its surrounding.
Thus, $Δ Q = 0$
Thus, the entropy also does not change, and $Δ S = 0$

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For the process to occur under adiabatic conditions, the correct condition is:
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(iii) q = 0
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Δ U .

For an isolated system, $Δ U = 0$ , what will be $Δ S$ ?

\begin{matrix} Column - I & Column - II (a) & Reversible cooling of an ideal gas at & (P) & w = 0; q < 0; Δ U < 0 constant volume (b) & Reversible isothermal expansion of an & (Q) & w < 0; q > 0; Δ U > 0 ideal gas (c) & Adiabatic expansion of non-ideal gas into & (R) & w = 0; q = 0; Δ U = 0 vacuum (d) & Reversible melting of sulphur at normal & (S) & w < 0; q > 0; Δ U = 0 melting point \end{matrix}

q, w, Δ U

1.0 b a r

0.1 b a r

273 K

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