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(C) According to the first law of thermodynamics,the change in internal energy $(\Delta U)$ is given by the equation: $\Delta U = q + w$. Here,$q$ is

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$-15$

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(C) According to the first law of thermodynamics,the change in internal energy $(\Delta U)$ is given by the equation: $\Delta U = q + w$. Here,$q$ is the heat absorbed by the system and $w$ is the work done on the system. Given: Heat absorbed by the system,$q = +10 \ kJ$ (positive because heat is absorbed). Work done by the system,$w = -25 \ kJ$ (negative because work is done by the system). Substituting these values into the equation: $\Delta U = 10 \ kJ + (-25 \ kJ) = -15 \ kJ$. Therefore,the change in internal energy is $-15 \ kJ$.

Calculate the change in internal energy of the system if $25 \ kJ$ of work is done by the system and it absorbs $10 \ kJ$ of heat. (in $kJ$)

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