29 Points!!
2 answers:
You might be interested in
0.11 moles of the gas are present in the sample of dry gas.
Explanation:
Data given:
mass of the gas = 2.1025 grams
volume of the gas = 2.850 litres
temperature = 22 degrees (273.15+22) = 295.15 K
Pressure = 740 mm Hg or 0.973 atm
moles of the gas =?
R = 0.08206 atmL/Mole K
From the ideal gas law the number of moles can be calculated in the sample of dry gas. Number of moles will be determined by the pressure exerted, volume and temperature of the gas.
The formula:
PV = nRT
n =
putting the values in the above equation:
n =
= 0.11 moles
0.11 moles of the dry gas is present in the sample given.
Answer: The partial pressure of oxygen is 187 torr.
Explanation:
According to Raoult's law, the partial pressure of a component at a given temperature is equal to the mole fraction of that component multiplied by the total pressure.
where, x = mole fraction
= total pressure
,
,
Thus the partial pressure of oxygen is 187 torr.