Question

Can someone let me know f my calculations are correct. Thanks!

You have 22.4 L of an unknown noble gas at standard temperature
and pressure with a density of 5.861 g/L

a. How many moles of this gas are in the
container?

i. n= PV/RT=

R=0.082057 L.atm/K.mol

T=273.15 K

Volume= 22.4 L

Density=5.861 g/l

P=1 atm

so: n=(1atm*22.4L)/ (0.082057 L.atm/K.mol* 273.15 K)=

n=(22.4)/(0.082057 mol*273.15)

n=22.4/22.1= 1 mole

b. What is the molar mass of this gas?

i. M=dRT/P

M=(5.861g/L*0.082057 L.atm/ K.mol*273.15 K)/1 atm)

(131.3g/mol)/1=131.2g/mol

c. Which noble gas is it? Xenon

A 0.75 g sample of oxygen gas has a volume of 286 mL sample of
under a pressure of 2026.5 millibars.

a. How many moles of oxygen are in this sample?

i. PV=nRT

P=2026.5 milibars=2.0265 bars*1atm/1.013 bars=2.00atm

V=282 ml=.286L

R=0.082057 L.atm/ K.mol

Moles= 0.75 grams O2*(1 mole O/32 grams O)=0.0234 moles oxygen

b. What pressure is the gas under in units of
atmospheres?

P=2026.5 milibars=2.0265 bars*1 atm/1.013 bars=2.00atm

c. What is the volume of the sample in Liters?

Volume= 282 ml*1L/1000ml=0.282 L

d. What is the temperature of the sample in degrees
celsius?

i. PV=nRT

T=PV/nR= (2.00 atm*0.282L)/( 0.0234 moles*0.082057 L.atm/
K.mol)=(0.564)/(0.00385L)=293.7K

Celcius=293.7-273.15=20.55C

Answer #1

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Please check my answers and let me know if they correct.
Thanks
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