A system takes in 1090 J of heat while performing 800 J of work. What is the change in internal energy of the system?

Question

BlackTom AI · Accepted Answer

The problem asks for the change in internal energy using the first law of thermodynamics, ΔU = q − w, where q is heat added to the system (positive when entering) and w is work done by the system (positive when the system does work).

First, identify the given values: q = +1090 J (heat absorbed) and w = +800 J (work done by the system).

Substitute into the equation: ΔU = q − w = 1090 J − 800 J.

Compute the difference: 1090 − 800 = 290 J.

Interpretation: since more heat entered than the work done by the system, the internal energy increases by 290 J. This aligns with the sign convention that a positive ΔU indicates a net increase in internal energy.

Note: The provided data set does not include any answer choices to evaluate, so the explanation focuses on the calculation and concept rather than selecting among options.

SPHY001 Practice Quiz - Unit 15 | LA055

A system takes in 1090 J of heat while performing 800 J of work. What is the change in internal energy of the system?

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