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?
I found
heat in the positive, heat out the negative, and work in the positive
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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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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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