Posted: Thu Feb 07, 2019 10:00 am
Calculate the heat released by 5.025 g of Kr(g) at 0.400 atm as it cools from 97.6 C to 25.0 C at
(a) constant pressure and
(b) constant volume. Assume that krypton behaves as an ideal gas.
Could someone please explain this?
Re: Textbook Question
Posted: Thu Feb 07, 2019 12:40 pm
So for this problem you're gonna wanna use the ideal gas equations, Cp (constant pressure) is 5/2 of the gas constant (which is 8.314) and Cv (constant volume) 3/2 of the same gas constant. One you calculate the C for each scenario you'll plug it into equation nCdeltaT to solve for q which is the heat released.
Cp = 5/3(8.314) = 20.875
5.025 g Kr/83.798 g/mol = .05997 moles Kr
q=(.05997)(20.785)(25.0-97.6) = -90.5 J
Then you'll just do the same thing for Cv all that changes is the heat capacity
Hope this helps:)