Find (a) the energy absorbed as heat and (b) the change in entropy of a 2.00 kg block of copper whose
temperature is increased reversibly from 25°C to 100°C. The specific heat of copper is 386 J/kg K .
dS=nRln(final volume/initial volume) **for an ideal gas**
The Attempt at a Solution\
Well I got the first part. The energy is just
which is (386)(2)(75K)= 57900J
however, when i got to the second part, I didn't know what to do since the copper isn't an ideal gas, and it has a non-constant temperature so I can't use the first equation. Any help would be appreciated!!!