A system absorbs 196 kJ of heat and the surroundings do 117 kJ
of...

Question

A system absorbs 196 kJ of heat and the surroundings do 117 kJ
of work on the system. What is the change in internal energy of
the system?

Accepted Answer

hey everyone in this example we need to calculate the change in internal energy for our system. If it's releasing 268 kg joules of heat and has 94 kg joules of work done on it. So we should recall our formula that our change in internal energy delta U. Is going to be equal to our value for heat which is represented by Q. Added to our value for work represented by W. So what we would say is that our change in internal energy is equal to our value for heat. Which in the problem is given as a release of kg joules. So that would be therefore negative to 68 kg joules so we can plug that in And this is going to be added to our value for work. So work is going to be done on the system. So we add positive 94 kg jewels. And this quantity is going to give us a value of -174. Kill it jules as our change in internal energy of our system. So this is our final answer. To complete this example. If you have any questions, please leave them down below and I will see everyone in the next practice video

A system absorbs 196 kJ of heat and the surroundings do 117 kJ of work on the system. What is the change in internal energy of the system?

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