Let 25.6 J of heat be added to a particular ideal gas. As a result, its volume changes from 41.0 to 82.0 cm3 while the pressure remains constant at 1 atm(= 101 kPa).
a) By how much did the internal energy of the gas change? -- 21.5 J got this part
b) What is the molar specific heat at constant pressure?
c) Find the molar specific heat at constant volume.
d) For this gas, what is the effective number of degrees of freedom? (may not be an integer)
C_p = C_v + R
Q = nC_p ΔT
The Attempt at a Solution
I think I have a handle on everything except part b. I know I need to find the change in temperature and the moles of the gas, at least that's what I think. After part b is found, c is just C_p + R where R is 8.314 if i remember correctly. And part d is just C_p = ((f+2)k N_a)/2 where k is Boltzman's constant and N_a is avagadro's number.
Any help is appreciated! Thanks!