Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | ||
2 to 3 | 20000 J | ||
3 to 1 | 0 | ||
Complete cycle | 0 | -19400 J |
Can we fill in anything else at this point or do we need to calculate something first?
We can apply the First Law of Thermodynamics to the entire cycle. Because DEint for an entire cycle is always zero, over an entire cycle we get Q = W, which in this case is -19400 J.
Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | ||
2 to 3 | 20000 J | ||
3 to 1 | 0 | ||
Complete cycle | -19400 J | 0 | -19400 J |
At this point we need to do a calculation of something. Without integrating or using logarithms, what could we calculate?
To find the work in the adiabatic 1 to 2 process would require an integral. To find the work, or the heat, in the isothermal 3 to 1 process would require logarithms.
We can find either of the two changes in internal energy, however. Finding the heat (Q) for the 2 to 3 process is also possible.
For the 2 to 3 process:
DEint = n CV DT
DEint = (5/2) nR DT = 2.5*100*200 = 50000 J.
Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | ||
2 to 3 | 50000 J | 20000 J | |
3 to 1 | 0 | ||
Complete cycle | -19400 J | 0 | -19400 J |
From there we can get to:
Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | -50000 J | |
2 to 3 | 70000 J | 50000 J | 20000 J |
3 to 1 | 0 | ||
Complete cycle | -19400 J | 0 | -19400 J |
Which leads to:
Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | -50000 J | 50000 J |
2 to 3 | 70000 J | 50000 J | 20000 J |
3 to 1 | -89400 J | 0 | |
Complete cycle | -19400 J | 0 | -19400 J |
Finally, we get the complete table:
Process | Q | DEint | W |
---|---|---|---|
1 to 2 | 0 | -50000 J | 50000 J |
2 to 3 | 70000 J | 50000 J | 20000 J |
3 to 1 | -89400 J | 0 | -89400 J |
Complete cycle | -19400 J | 0 | -19400 J |