Why is Q = ∆U (heat = change in thermal energy)?

Answer 1

From the first law of thermodynamics,

#delQ = delU + delW#

Where #delQ#, #delU# and #delW# are differentials in heat, internal energy and work respectively.

Then if there is no work done by/upon the system, #delW = 0#

Then the above relationship reduces to #delQ = delU# and heat transfer is equal to change in internal energy of the gas.

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Answer 2

The equation Q = ΔU represents the first law of thermodynamics, stating that heat transfer (Q) is equal to the change in internal energy (ΔU) of a system. It accounts for energy conservation in thermodynamic processes.

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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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