A quantity of CO gas occupies a volume of 0.66 L at 1.3atm and 303 K . The pressure of the gas is lowered and its temperature is raised until its volume is 2.9 L .Find the density of the CO under the new conditions.
Given,
Initial Volume of CO = V = 0.66 L
Initial Pressure of CO = P = 1.3 atm
Initial Temperature of CO = T = 303 K
We know that,
PV = nRT
=> 1.3 x 0.66 = n x 0.0821 x 303
=> n = 0.0345 moles
New Volume = 2.9 L
PV = nRT
=> PV = (m/M) RT
=> PM = dRT
where, d = m / V = density
=> d = P' x M / R x T'
where P' and T' are new Pressure and Temp.
PV / T = P'V' / T'
=> 1.3 x 0.66 / 303 = P' x 2.9 / T'
=> P' / T' = 9.76 x 10^-4
=> d = (M / R) x (P' / T')
=> d = (28 / 0.0821) x (9.76 x 10^-4)
=> d = 0.333 g / L = 3.33 x 10^-4 g / mL
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