Calculating final temp & enthalpy for an ideal monatomic gas

[Jia Hao Liu 3L]

Can someone guide me through this problem?

"Suppose that 1.00 kJ of heat is transferred to 2.00 mol argon. What will the final temperature be if the heat is transferred at a constant pressure? Calculate the enthalpy change for the process and describe the thermodynamic reaction. Assume an ideal, monatomic gas at STP (25 Celcius, 1 atm)."

Any help is appreciated. Thanks!

[Jenna Kovsky 1I]

The first part (calculating the final temperature) is fairly straightforward. I used the equation q=n*C*deltaT. For the heat capacity (C), you were told to assume that it is an ideal, monatomic gas at constant pressure, so you would use 5/2 R as your heat capacity (this is given on the formula sheet). So you just plug in 5/2*8.314J/Kmol for C, 1.00kJ for q, 2.00mol for n, and 298K (because you're assuming STP) for T initial. Then you just solve for T final. Don't forget to convert q from kilojoules to joules (because the gas constant uses joules)

As for the part about calculating the enthalpy change, I'm still working on that personally, I'll post here again if I get it.
Hope that helped!

[Jenna Kovsky 1I]

Actually, now that I think about it, doesn't q=deltaH at constant pressure?

[Jia Hao Liu 3L]

Yeah, that's what i was thinking... So delta H = 1.00 kJ and the reaction is endothermic?

[Jenna Kovsky 1I]

That seems right to me! Where did you get this problem, maybe you can look up the solution online or something?

[Jia Hao Liu 3L]

It was on my quiz! Thanks for your help!

[Jenna Kovsky 1I]

That seems right to me! Where did you get this problem, maybe you can look up the solution online or something?

[Chem_Mod]

Correct, is true always. Since this process is indeed constant pressure, then