intro Thermodynamic question

[KKAK]

Hi all , I have 2 questions, I dunno how to derive the equations, please help.
Thank you.
1)A reversible adiabatic expansion of 2.5 moles or He from a volume 9L at 300K to a final volume of 28L.
Find work(W), heat(Q), internal energy(U) and enthalpy change(H) and final temperature. (He is a monatomic ideal gas)

2)A reversible isobaric expansion of an ideal gas from P1,V1,T1 to P1,V2,T2, assume Cv = 5/2nR
Find W, change in internal energy, Heat and enthalpy.

I know for #1 heat = 0, therefore delta U = W = integral P*dV, but I don't know since we don't know pressure , I don't know how to continue.

For #2, it is constant pressure, therefore W= -P*delta V
delta U = Q - (p*delta V)
Q = delta U + (p*delta V) = enthalpy
Am I right ? it looks so weird, I need some help thanks !

[Gokul43201]

1. Adiabatic work done, W = \int PdV . But PV^{\gamma} = const, ~C gives :

W = C~\int \frac{dV}{V^{\gamma}}

Integrate that out, find P using the Ideal Gas Law, use the value of \gamma for an ideal monoatomic gas, and hence find the value of the adiabatic constant C. Plug in values of C, Vf and Vi to find the work done.

2. For an isobaric process, Q is easily found. Recall what Cp is ?