[Shark 774]

I got a bit stumped by a practice question I was doing regarding enthalpy change:

The temperature of one mole of gas was increased adiabatically from 273K to 548K (Cvm = 20.8J/k/mol).
For the system calculate the change in enthalpy (∆H).

So obviously ∆Q = 0 as it is adiabatic and therefore the change in internal energy of the system (∆U) = the work done on the system = n x Cvm x ∆T = 1×20.8×275 = 5720J/mol

I tried using ∆H = ∆U + P∆V = ∆U + nR∆T = 5270 + 2286 = 7556J/mol
But I'm pretty sure this is incorrect.

Any ideas?

Thanks in advance!

[curiouscat]

Looks ok to me. I could be wrong.