A 150 mL container of nitrogen gas is collected at 758 mm Hg and 28.3 celicuis by displacement of water from the container. The vapor of water at 28.3 celicuis is 23.2 mm Hg. How many miles it nitrogen gas are in the flask
First, we need to calculate the partial pressure of nitrogen gas in the flask:
Total pressure in the flask = pressure of nitrogen gas + pressure of water vapor
758 mm Hg = pressure of nitrogen gas + 23.2 mm Hg
Pressure of nitrogen gas = 758 mm Hg - 23.2 mm Hg
Pressure of nitrogen gas = 734.8 mm Hg
Now we can use the ideal gas law to calculate the number of moles of nitrogen gas in the flask:
PV = nRT
(734.8 mm Hg)(150 mL) = n(0.0821 L.atm/mol.K)(28.3 + 273.15 K)
110220 = n(23.2)
n = 4746.55 moles
Finally, we can convert moles of nitrogen gas to molecules using Avogadro's number:
1 mole of gas = 6.022 x 10^23 molecules
4746.55 moles = 4746.55 * 6.022 x 10^23
2.858 x 10^26 molecules
Therefore, there are 2.858 x 10^26 molecules of nitrogen gas in the flask.