The system shown in the diagram is at equilibrium at 27oC and the volume of the bulb is 150 mL. At this temperature, the vapour pressure of water is 28 millimetres of mercury. If the bulb contains 0.001 mol of O2(g), the volume of the liquid water is approximately:
Correct answer: B. 10 mL
- A. 34 mL
- B. 10 mL
- C. 30 mL
- D. 60 mL
Explanation
PV = nRT, V = (0.001*0.0821*300)/0.175= 140.6ml Total bulb = 150ml → 140.6-150 ≈ 10ml
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Gas behaviour is explained through the kinetic molecular theory and the relationships among pressure, volume and temperature. Work includes STP, Boyle's and Charles's laws, absolute zero, the ideal gas equation, and the distinction between ideal and real gases, especially the effects of intermolecular forces and molecular volume.
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