Answer:
1.35 g/L
Explanation:
1) Use PV = nRT to determine moles of gas present in gas:
(1.10 atm) (2.55 L) = (n) (0.08206) (328 K)
n = 0.104 mol
2) Get molar mass of gas using calculated moles:
0.104 mol x M g/mol = 3.45g
M = 3.45 g / 0.104 mol = 33.17 g/mol
Density = Molar Mass x P / RT
= 33.17 g/mol x 1.10 atm / 0.0821 L mol / atm .K x 328 K
= 1.35 g /L
Answer:
The density of the gas is 1.42g/L and the molar mass is 32.92 g/mol
Explanation:
Mass of the unknown gas=m= 4.05g
Temperature=T= 35C
Pressure exerted upon the unknown gas= P= 1 atm
Volume of the flask=V= 2.85 L
Density= ?
Density= [tex]\frac{mass of the unknown gas}{ volume of the container containing the gas}[/tex]
= [tex]\frac{m}{V}[/tex]
=[tex]\frac{4.05}{2.85}[/tex]
=1.421= 1.42g/L
Molar mass of the gas=M=?
Now,
As the formula is defined
[tex]\frac{n}{V}=\frac{P}{RT}[/tex]
n=[tex]\frac{VP}{RT}[/tex]
(R= 0.082 L atm /K mol)
Since Temperature= 35C= (35+273) K
=308 K
n=[tex]\frac{2.85\times 1}{0.082\times 308}[/tex]
n=[tex]\frac{2.85}{25.26}[/tex]
n=0.1129 moles
Molar mass= M=[tex]\frac{m}{n}[/tex]
=[tex]\frac{4.05}{0.123}[/tex]
=32.92 g/mol
Hence the density of the gas is 1.42 g/L and the molar mass is 32.92 g/mol
