During an adiabatic process, if 37 J of work is done on the system, the work done by the system is -37 J. This indicates that the change in internal energy (ΔU) is equal to 37 J, as per the equation ΔU = -W, where W is the work done on the system. The discussion clarifies that negative work does not imply impossibility; rather, it reflects the energy transfer direction. Therefore, the scenario presented is feasible and aligns with the principles of thermodynamics.
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Where does "it" say that? Do you think that the work done on the gas during an adiabatic process should always be positive?traveler7 said:I think it is impossible because it says work is negative. I am not sure though.
Explain your reasoning. If positive 37 Joules of work is done ON the system then the work done BY the system is -37 Joules. This means \Delta W = -37J. You correctly state that \Delta U = -\Delta W if \Delta Q = 0 (no heat flows into or out of the system). So what must be the change in internal energy here? Why can this not occur?traveler7 said:Homework Statement
Is this impossible: (yes or no)
During an adiabatic process, 37 J of work was done on the system.
Homework Equations
Delta U=-W
The Attempt at a Solution
I think it is impossible because it says work is negative. I am not sure though.