Q4 / 150 · MHT CET 2021 (24 Sep Shift 2) · Chemistry

What is internal energy change when $62 \mathrm{~J}$ of work is done on the system and $128 \mathrm{~J}$ of heat is transferred to surrounding?

  • A
    -62 J
  • B
    -190 J
  • C
    -128 J
  • Correct answer
    D
    -66 J

Solution

Work done on the system $=+62 \mathrm{~J}$ Heat released to the surrounding $=-128 \mathrm{~J}$ From first law of thermodynamics, $\begin{aligned} & \Delta \mathrm{U}=\mathrm{q}+\mathrm{W} \\ & =-128+62 \\ & =-66 \mathrm{~J} \end{aligned}$

Hence, the correct answer is option: 'D'.

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