Question

A system delivers 222 J of heat to the surroundings while delivering 645 J of work. What is the change in the internal energy, ΔU, of the system?

Answer 1

Answer:

-867 J

Explanation:

∆E (internal energy) = q (heat flow) + w (work)

The question says that heat is delivered to the surroundings (therefore lost by the system so (-)). Also, It says in the same statement work is being delivered, so work is also negative.

∆E = -222J + (-645J)

= -867J

Answer 2

Answer:

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