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∙ 7y agoThe change in internal energy of a system that does 100 joules of work depends on the heat exchange as well. In general, the change in internal energy is equal to the amount of heat added to the system minus the work done by the system.
The total energy added to the system is 160 Joules, comprising of 100 Joules of heat and 60 Joules of work. This increase in energy will lead to a rise in the system's internal energy.
The change would be 100 joules, because an isochoric system can not perform the work.
The internal energy change of the system would be the sum of the heat absorbed and the work done on the system. Therefore, the internal energy change would be 20000 J (heat absorbed) + 5000 J (work done) = 25000 J.
The internal energy change of the system can be calculated by subtracting the work done by the system from the heat added to the system. In this case, the internal energy change is ΔU = Q - W = 850 J - 382 J = 468 J. Therefore, the internal energy of the system increases by 468 Joules.
400 joules.
-70 Joules
The total energy added to the system is 160 Joules, comprising of 100 Joules of heat and 60 Joules of work. This increase in energy will lead to a rise in the system's internal energy.
The change would be 100 joules, because an isochoric system can not perform the work.
The internal energy change of the system would be the sum of the heat absorbed and the work done on the system. Therefore, the internal energy change would be 20000 J (heat absorbed) + 5000 J (work done) = 25000 J.
The internal energy change of the system can be calculated by subtracting the work done by the system from the heat added to the system. In this case, the internal energy change is ΔU = Q - W = 850 J - 382 J = 468 J. Therefore, the internal energy of the system increases by 468 Joules.
400 joules.
1,000 J
A certain system absorbs 350joules of heart and has 230joules of work done on it. What is the value of Delta?
The change in internal energy can be calculated as the sum of the work done and heat added to the system. The work done is already in Joules, so we need to convert the heat added from calories to Joules: 200 cal = 837.4 J. Thus, the change in internal energy is 1200 J + 837.4 J = 2037.4 J.
The thermal energy change of the system can be calculated using the first law of thermodynamics, which states that the change in internal energy of a system is equal to the heat added to the system minus the work done by the system. Therefore, the thermal energy change would be 100 J (heat added) - 60 J (work done) = 40 J.
The first law of thermodynamics requires that energy input must equal energy output plus energy accumulation. In this case that translates to; 430 J = 120 J + (internal energy change) so Internal energy change = 430 J - 120 J = +310 J (the internal energy increased by 310 Joules)
The internal energy of a system increases when energy is added to the system through heat transfer or work done on the system. This can result in an increase in temperature, change in phase, or other forms of internal energy change.