1. Which of the following gas samples would have the largest
volume, if all samples are at the same temperature and
pressure?
A. 0.309 moles CH4
B. 9×1023 molecules of N2
C. 65.7 grams of Xe
D. they would all have the same volume
2. Which of the following gas samples would have the largest
volume, if all samples are at the same temperature and
pressure?
A. 174.5 grams of Xe
B. 8×1023 molecules of N2
C. 1.33 moles CO2
D. they would all have the same volume
1. Higher number of moles will have high volume
Moles of N2 = number of particle/ avagadro number
= (9*10^23)/(6.022*10^23)
= 1.495
Moles of Xe = mass / molar mass
65.7 / 131.3
= 0.5
CH4 = 0.309
So, option B is correct.
2. Moles of Xe = 174.5 / 131.3
= 1.33
Moles of N2 = ( 8*10^23 ) / ( 6.022*10^23)
= 1.33
Moles of CO2 = 1.33
All have same moles so same volume .
Option D
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