[mandii27]

5.0 mol of an ideal gas is expanded reversibly and adiabatically from an initial volume of 2.5 L to 6.0 L at an initial temperature of 298 K. Calculate the following:
(a)The work (in J) done on the system.
(b) The heat added (in J) to the system.
(c) The internal energy change (in J) for the system.

What equation can I use to find T(final)  if I am not given the name of the gas?

will T(final)= T(initial) (V(initial)/V(final) 2/3 work?  Do I need to find the work (in J) done on the system before I can proceed to find the internal energy change for the system?

[juanrga]

5.0 mol of an ideal gas is expanded reversibly and adiabatically from an initial volume of 2.5 L to 6.0 L at an initial temperature of 298 K. Calculate the following:
(a)The work (in J) done on the system.
(b) The heat added (in J) to the system.
(c) The internal energy change (in J) for the system.

What equation can I use to find T(final)  if I am not given the name of the gas?

What is an ideal gas?

[Enthalpy]

Sometimes "ideal gas" may also include polyatomic gases, but depending on conventions, this one could be monoatomic.

Search keywords, for instance at Wiki:
"ideal gas"
adiabatic
"isentropic coefficient"
"Cp/Cv"

You should clarify you comprehension of heat, work, internal energy, (enthalpy if already learnt) and adiabatic, as (b) and (c) result logically from the words. These notions are in fact more elementary than the computation of an adiabatic expansion, so you might begin with that.

Take heart!