Let Q be the energy added to the gas by heat and ΔU be the change in internal energy of the process from the final energy UF to the initial energy UI. We are given the value of the energy added to the gas. Noting the sign on the value calculated for W above and the sign on the change in internal energy ΔU, for the change in internal energy, we haveΔU = UF − UI = Q + W = J − 506.5 J = J.
Question
Let Q be the energy added to the gas by heat and ΔU be the change in internal energy of the process from the final energy UF to the initial energy UI. We are given the value of the energy added to the gas. Noting the sign on the value calculated for W above and the sign on the change in internal energy ΔU, for the change in internal energy, we haveΔU = UF − UI = Q + W = J − 506.5 J = J.
Solution
It seems like there is a missing value in your question. The equation ΔU = UF - UI = Q + W is correct for the first law of thermodynamics, where ΔU is the change in internal energy, Q is the heat added to the system, and W is the work done by the system. However, you have not provided the value for Q, the energy added to the gas by heat.
Once you have the value for Q, you can substitute it into the equation along with the value for W (which is -506.5 J, as per your question). The result will be the change in internal energy, ΔU.
So, if you provide the value for Q, I can help you calculate ΔU.
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