What is the mass of a gas that occupies 48.9 liters, has a pressure of 724 torr,a temperature of 25°C and a..

What is the mass of a gas that occupies 48.9 liters, has a pressure of 724 torr, a temperature of 25°,C and a molecular weight of 345 g/mole?

Answer:
PV = nRT
P = Pressure = 724 torr = 724/760 atm
V = Vol = 48.9 L
n = no. of moles of gas
R = universal ags const = 0.0821 L atm / mol K
T= temp in absolute scale = 273 + 25 = 298 K

but, n = m/M
m = mass of the gas
M = molecular mass of the gas = 345 g/mole
=> PV = (m/M)RT
=> m = PVM/RT
putting the values,

m = 724 * 48.9 * 345/(0.0821 * 298*760)

=674.0276 g (ans)

check the calculations. I may have committed some silly mistakes.

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