A mono-atomic ideal gas of $2$ moles undergoes an isothermal expansion which makes its volume double. Then the volume of the gas is doubled again through an isobaric process. Given a starting temperature of $350$ Kelvin:
- how much work is done by the gas during the isobaric expansion?
- how much heat is transferred during the isothermal expansion?
note: R = $8.31$ J/(mol*K) and Cp = $5/2$ * R
The problem gives me this data:
- $n$ = 2 mol
- $T_1$ = $350$ K
- $R$ = $8.31$ J/(mol*K)
- $C_p$ = $\frac5 2$ $R$
- $V_3 = 2V_2 = 4V_1$
The formula that I would use to find the work for the isobaric expansion would be $W = nR(T_3 - T_2)$
But I don't know how to find the temperature at the end of the expansion, because the problem doesn't give me pressure or volume. So I can't use $P_iV_i = nRT_i$ to start finding it. I don't know if I'm missing something very important or the problem is wrong