A system performs 354 J of work on its surroundings while losing 133 J of internal energy. How would you determine the heat transferred to the system during this process?

Answer 1

I found #Q=221J#

We could use the First Law of Thermodynamics: #DeltaE_("int")=Q-W# where the variation of internal energy #DeltaE_("int")# is equal to the difference between heat #Q# and work #W#. I use the convention that:

heat in the positive, heat out the negative, and work in the positive

In our case internal energy decreases so: #DeltaE_("int")<0#: #-133=Q-(+354)# so #Q=354-133=221J#
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Answer 2

The heat transferred to the system during this process is 221 J, calculated using the first law of thermodynamics: ΔU = Q - W, where ΔU is the change in internal energy, Q is the heat transferred, and W is the work done. Rearranging the equation gives Q = ΔU + W.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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