Q37.One mole of an ideal gas is expanded isothermally and reversibly to half of its initial pressure. ΔS for the process in JK−1 mol−1 is [ln 2 = 0.693 and R = 8.314, J/(molK)] (1) 6.76 (2) 5.76 (3) 10.76 (4) 8.03
What This Question Tests
This question requires applying the formula for entropy change of an ideal gas undergoing an isothermal and reversible expansion, using given values of moles, gas constant, and pressure ratio.
Concepts Tested
Formulas Used
ΔS = nR ln(P₁/P₂)
📚 NCERT Sections This Tests
3.21 — The Following Data Were Obtained During The First Order Thermal
Chemistry Class 11 · Chapter 3
3.21 The following data were obtained during the first order thermal decomposition of SO2Cl2 at a constant volume. SO2 Cl 2 g SO 2 g Cl 2 g Experiment Time/s–1 Total pressure/atm 1 0 0.5 2 100 0.6 Calculate the rate of the reaction when total pressure is 0.65 atm.
3.23 — The Rate Constant For The Decomposition Of Hydrocarbons Is 2.418 × 10–5S–1
Chemistry Class 11 · Chapter 3
3.23 The rate constant for the decomposition of hydrocarbons is 2.418 × 10–5s–1 at 546 K. If the energy of activation is 179.9 kJ/mol, what will be the value of pre-exponential factor.
3.20 — For The Decomposition Of Azoisopropane To Hexane And Nitrogen At 543
Chemistry Class 11 · Chapter 3
3.20 For the decomposition of azoisopropane to hexane and nitrogen at 543 K, the following data are obtained. t (sec) P(mm of Hg) 0 35.0 360 54.0 720 63.0 Calculate the rate constant.
📋 Question Details
- Chapter
- Thermodynamics & Thermochemistry
- Topic
- Entropy change for ideal gas
- Year
- 2012
- Shift
- 26 May Online
- Q Number
- Q37
- Type
- MCQ
- NCERT Ref
- Class 11 Chemistry Ch 6: Thermodynamics
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