The internal energy change in a system that has absorbed $2 ext{ kcal}$ of heat and done $500 ext{ J}$ of wo

Question

The internal energy change in a system that has absorbed $2	ext{ kcal}$ of heat and done $500	ext{ J}$ of work is

Accepted Answer

According to the first law of thermodynamics, $\Delta Q = \Delta U + \Delta W$.
Given:
Heat absorbed by the system, $\Delta Q = 2	ext{ kcal} = 2 	imes 1000 	imes 4.2	ext{ J} = 8400	ext{ J}$ 
Work done by the system, $\Delta W = 500	ext{ J}$
Therefore, the change in internal energy is:
$\Delta U = \Delta Q - \Delta W = 8400	ext{ J} - 500	ext{ J} = 7900	ext{ J}$.

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