AP EAMCET · PHYSICS · Thermodynamics
As ideal monoatomic gas of 1.5 moles is heated at a constant pressure \(2 \mathrm{~atm}\) so that its temperature increases from \(30^{\circ} \mathrm{C}\) to \(130^{\circ} \mathrm{C}\) work done by the gas is (Universal gas constant \(\left.=8.3 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right)\)
- A \(2500 \mathrm{~J}\)
- B \(1450 \mathrm{~J}\)
- C \(1245 \mathrm{~J}\)
- D \(555 \mathrm{~J}\)
Answer & Solution
Correct Answer
(C) \(1245 \mathrm{~J}\)
Step-by-step Solution
Detailed explanation
Work done by a gas in a constant pressure process is \(W=n R \Delta T\)...(i) Here, \(n=1.5\) moles \(\begin{aligned} R & =8.3 \mathrm{~J} \mathrm{~mole}^{-1} \mathrm{~K}^{-1} \\ \Delta T & =\{(130+273)-(30+273)\}=100 \mathrm{~K}\end{aligned}\) So,from eq. (i)…
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