Temperature of a system decreases during

Isothermal compression

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Adiabatic compression

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Adiabatic expansion

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Isothermal expansion

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Solution

The correct option is C Adiabatic expansion
In adiabatic systems, there is no heat exchanged with the system and the surrounding since $q = 0$ . Hence, $Δ U = w$
So the temperature would decrease if the internal energy decreases, since $Δ U$ is directly proportional to $Δ T$ .
this means that the gas would expand! This is a direct consequence of the fact that $w = - P Δ V$ if $w$ has to have a -ve value, then the final volume MUST be greater than the initial volume.

Suggest Corrections

	Column I		Column II
a.	Temperature of a system always decreases	p.	$C H_{2} = C H - C H = C H_{2}$
b.	${(\begin{matrix} \frac{\partial U}{\partial V} \end{matrix})}_{T} = 0$	q.	Internal energy increases
c.	Temperature of the system increases	r.	Ideal gas
d.	$Δ H_{h y d r o g e n a t i o n (e x p e r i m e n t a l)}$ $< Δ H_{h y d r o g e n a t i o n (c a l c u l a t e d)}$	s.	Adiabatic expansion