the enthalpy change ,del H ,due to reversible adiabatic expansion of an ideal gas from p1,v1,t1 to p2,v2,t2 is?

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Please find the solution to the asked query:

$$\begin{gathered} Enthalpy H is given by \\ H=U +PV \\ Thus \\ In moving from states P1 toP2 and V1 to\hspace{0.17em}V2 \\ the enthalpy change is given by : \\ ∆H =U +PV \\ that is \\ ∆H =∆U +P∆V+V∆P \\ For an adiabatic process \\ q=0, so from the first law of thermodynamics we have \\ ∆U =q+w =q-P∆V \\ ∆U =w=-P∆V \\ When we substitute this in the first equation we get: \\ ∆H =V∆P \end{gathered}$$
or 
$∆H =V(P_2-P_1)$

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