MHT CET · Chemistry · Thermodynamics (C)
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
- D -66 J
Answer & Solution
Correct Answer
(D) -66 J
Step-by-step Solution
Detailed explanation
Work done on the system \(=+62 \mathrm{~J}\)
Heat released to the surrounding \(=-128 \mathrm{~J}\)
From first law of thermodynamics,
\(\begin{aligned}
& \Delta \mathrm{U}=\mathrm{q}+\mathrm{W} \\
& =-128+62 \\
& =-66 \mathrm{~J}
\end{aligned}\)
Heat released to the surrounding \(=-128 \mathrm{~J}\)
From first law of thermodynamics,
\(\begin{aligned}
& \Delta \mathrm{U}=\mathrm{q}+\mathrm{W} \\
& =-128+62 \\
& =-66 \mathrm{~J}
\end{aligned}\)
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