JEE Mains · Chemistry · STD 11 - 5. Thermodynamics and thermochemistry
A piston filled with \(0.04\, mol\) of an ideal gas expands reversibly from \(50.0\, mL\) to \(375\, mL\) at a constant temperature of \(37.0\,^oC.\) As it does so, it absorbs \(208\, J\) of heat. The values of \(q\) and \(w\) for the process will be \((R = 8.314 \,J/mol\,K)\,(\ln 7.5 =2.01)\)
- A \(q = +208\,J, \,w =-208\,J\)
- B \(q =-208\,J, w =-208\,J\)
- C \(q =-208\,J, w = +208\,J\)
- D \(q = +208\,J, w = +208\,J\)
Answer & Solution
Correct Answer
(A) \(q = +208\,J, \,w =-208\,J\)
Step-by-step Solution
Detailed explanation
Solution:- As the heat is absorbed. \(\therefore q =+208 J\) Now for reversible isothermal process, \(q =- W\) \(\therefore W =- q =-208 J\) Hence the values of \(q\) and \(W\) for the process will be \(+208 J\) and \(-208 J\) respectively.
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