A sample of oxygen collected over water at a temperature of 29.0 °C and a pressu

Question

A sample of oxygen collected over water at a temperature of 29.0 °C and a pressure of 764 torr has a volume of 0.560 L. What volume would the dry oxygen have under the same conditions of temperature and pressure? Answer: 0.583 L hemical Stoichiometry and Gases hemical stoichiometry describes the quantitative relationships between reactants and products in chemical We have previously measured quantities of reactants and products using masses for solids and volumes in conjunction with the molarity for solutions; now we can also use gas volumes to indicate quantities. If we know the volume, pressure, and temperature of a gas, we can use the ideal gas equation to calculate how many moles of the gas are present. If we know how many moles of a gas are involved, we can calculate the volume of a gas at any temperature and pressure.

Explanation / Answer

The water vapour pressure is the partial pressure of water vapour in any gas mixture in equilibrium with solid or liquid water.

Vapor Pressure of Water at 29°C = 30 torr

Ptot = PO2 + PH2O

764 = PO2 + 30

PO2 = 734 torr

Using combined gas law equation.

P1V1 = P2V2

764 torr x 0.56 L = 734 torr x V2

V2= 0.583 L

Thank You

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