Calculating temperature change

[IsabelMurillo3K]

Under constant pressure conditions the expansion of 0.17 moles, causes an ideal gas to experience a 3.4 atm·L increase in its internal energy. If the system performed 2.26 atm·L of work, what was the temperature change of the gas?
Hey guys! This problem was from my discussion section practice quiz. I was wondering if anyone knows which formula to use to solve this problem and how to manipulate it if necessary.
Thank you!

[Nicole Huang 3F]

Hi!
For this problem, you're gonna wanna use deltaU=w+q; since deltaU=+3.4 atmL, and work is -2.26atmL, then q would be 5.66 atmL. You can convert it to joules, and use the equation q=nCpdeltaT, where Cp is 5/2R, hope that helps!

[Carolina 3E]

at constant P, (delta)U = qp + w
(delta)U = (3.4 atm.L)(101.325 J/atm.L)
w = (2.26 atm.L)(101.325 J/atm.L)
qp = (delta)U - w
qp = nCp(delta)T
(delta)U - w = (0.17 mol)(5/2 R)(delta)T

[Gwendolyn Hill 2F]

Hi!
So because we have constant pressure, and we are given work, mols, and given delta U, we can calculate the temperature change by using the equation for q where q = nC∆T. We know it is an ideal gas, so I believe that we can say that Cp = 5/2 assuming it is monoatomic? Someone else can feel free to comment on that but yeah!

[Juliet Cushing_2H]

Ya! You should use ΔU = q + w