In an adiabatic process, which of the following is true?

q = w

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q = 0

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Δ E = q

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P Δ V = 0

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Solution

The correct option is A $q = 0$
In an adiabatic process, $q = 0$ as there is no exchange of heat energy between system and surrounding.

Hence, option B is correct.

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For the process to occur under adiabatic conditions, the correct condition is:
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(ii) $Δ p = 0$
(iii) q = 0
(iv) w = 0

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\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}

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