Solution
Step
1- Find the pressure the gas exerts.
Step
2- Convert the temperature
from Celsius to Kelvin.
Step
3- Convert the volume from
millilitres to litres.
Step
4- Solve for the numb er of mole
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The pressure of the gas is 1.5
atm. We must convert the pressure from atmospheres to kilopascals.
1 atm = 101.3kPa
So
1.5 atm = 1.5 X 101.3 = 151.95kPa
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23 degrees Celsius is (273 + 23) 296o K
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The volume is already given in
litres
4.5 litres.
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Place the values of each variable in the formula and solve for the number of mole
n = (151.95 X 4.5) / (8.31 X 296) = 0.278 mole
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The
ideal gas equation
 (1) |
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A pure sample of nitrogen gas was placed in an empty 4.5 litre container at 23oC and sealed. The pressure exerted on the walls of the container by the gas was measured at 1.5atm. What is the number of moles of nitrogen gas present? (Atomic
mass of N= 14)
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