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=
Volume= 22.4 L
so: n=(1atm*22.4L)/ (0.082057 L.atm/K.mol* 273.15 K)=
n=22.4/22.1= 1 mole
b. What is the molar mass of this gas?
M=(5.861g/L*0.082057 L.atm/ K.mol*273.15 K)/1 atm)
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?
P=2026.5 milibars=2.0265 bars*1atm/1.013 bars=2.00atm
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
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
T=PV/nR= (2.00 atm*0.282L)/( 0.0234 moles*0.082057 L.atm/ K.mol)=(0.564)/(0.00385L)=293.7K
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