If I have 0.275 moles of a gas at a temperature of 75K and a pressure of 1.75 atm what is the volume of the gas?
First of all we have to assume that this gas behaves as an ideal gas and hence we can apply the ideal gas law to this particular incident.
`PV = nRT`
`V = (nRT)/(P)`
here n = 0.275 mol
T= 75 K
P= 1.75 atm
and the gasconstant R = 0.082057 lit.atm/(K.mol)
`V = ((0.275 mol)(0.082057( l.atm)/(K.mol))(75K))/1.75 atm`
` ` V = 0.967 liters
Therefore the volume of the gas is 0.967 liters