The vapour pressure of water at 80-C is 355 mm of Hg- The total pressure of a 1-5 L vessel containing O2 saturated with water at 80-C is 760 mm of Hg- The contents of the vessel are pumped into a 3 L vessel at the same temperature- What is the partial pressure of O2-

A sample of $O_{2}$ gas is collected over water at $23^{\circ}$ C at a barometric pressure of 751 mm Hg (vapour pressure of water at $23^{\circ}$ C is 21 mm Hg). The partial pressure of $O_{2}$ gas in the sample collected is ......

Join BYJU'S Learning Program

The vapour pressure of water at 80∘C is 355 mm of Hg. The total pressure of a 1.5 L vessel containing O2 saturated with water at 80∘C is 760 mm of Hg. The contents of the vessel are pumped into a 3 L vessel at the same temperature. What is the partial pressure of O2?

The correct option is A 202.50 mm of HgVolume of O2=1.5 L PO2=760−355=405 mm of Hg Since the temperature is constant, Using Boyle's law, PO2VO2=P′O2V′O2 1.5 L×405 mm=3 L×P′O2 ∴ P′O2=202.5 mm of Hg

The correct option is A $202.50 mm of Hg$
Volume of $O_{2} = 1.5 L$
$P_{O_{2}} = 760 - 355 = 405 mm of Hg$
Since the temperature is constant,
Using Boyle's law,
$P_{O_{2}} V_{O_{2}} = P_{O_{2}}^{'} V_{O_{2}}^{'}$
$1.5 L \times 405 mm = 3 L \times P_{O_{2}}^{'}$
$∴ P_{O_{2}}^{'} = 202.5 mm of Hg$