Chemistry about gas and molars, works needs to be explained.?

Question

a gas weighing 22.40 g occupies a 10.00-l flask a 27C and 722 torr of pressure. What is the molar mass of the gas?

Answer 1

You have V, T and P, so you can find n, the moles of gas. If n moles weights 22.4 g, you can find what 1 mole weights by proportion.

Answer 2

Okay, so this should be an ideal gas question
So basically you use the ideal gas equation:
PV=nRT
and you know that n is the number of moles, and you know that moles=mass/molar mass

so you replace n with mass/molar mass to get:
PV=(m/MM)RT
and you isolate MM
to get MM=mRT/PV
and you already know mass (22.40 g) and R (the constant: 0.0821 L atm/molK) and you know the Volume (10.00 L)

and you know the temperature is 27C, and you need to convert it to K, you do this by adding 273 to the degrees celsius, and you get 300K. so now you know the temperature

and you know the pressure is 722 torr. so just convert to atm.
by dividing by 760.
so your pressure is 722/760 atm

and just plug in everything you know and you should get your molar mass in g/mol. ^^

Answer 3

To answer at this question we have to know the moles of the gas .
We use the equation n = pV / RT
p = 722 / 760 = 0.95 atm
T = 27 + 273 = 300 K
n = 0.95 x 10.00 / 0.0821 x 300 = 0.386
Molar mass = 22.40 g / 0.386 = 58.1 g/mol

Answer 4

PV=nRT where n= mols = gm/Mwt.

Thus g/Mwt)(PV)=RT Thus

(gPV)/(RT)= Mwt

22.4g(722 torrx10.0L)/(R x300k)=mwt.

Look up the value for R (liter torr/(mol K)

Answer 5

2.24g/L is the density.

2.24g/L =(MM)(722torr)/(62.37)(300.15K)

41933.596 = 722MM

58.079 = Molar Mass, g/mol

As you see, I and Dr A. have given you two different ways to come to the same answer. ( 62.37 is Liters Torr/mols K )