1. The problem statement, all variables and given/known data A monatomic ideal gas undergoes the thermodynamic process shown in the PV diagram. Determine whether each of the values ΔU, Q, and W for the gas is positive, negative, or zero. 2. Relevant equations ΔU=Q-W W=integral under the curve PV=nRT T=PV/nR 3. The attempt at a solution direction is negative then the integral negative then work is negative ΔU depends on change in temp, and here pressure increases and volume decreases so it was Ti=P0x2V0/nR and at final it becomes Tf=2P0xV0/nR Tf=Ti then it stays the same no change in temp then ΔU =0 therefore 0=Q-W Q=W but W negative then Q also negative Is that correct? I need only to check my answer... and is there any other way to determine Q from Graph (without looking at W or ΔU) ???