Bro honestly I don’t understand either
Answer: The molar mass of the gas is 31.6 g/mol
Explanation:
According to ideal gas equation:
P = pressure of gas = 3.0 atm
V = Volume of gas = 25.0 L
n = number of moles = ?
R = gas constant =
T =temperature =
Moles =![\frac{\text {given mass}}{\text {Molar mass}}](https://tex.z-dn.net/?f=%5Cfrac%7B%5Ctext%20%7Bgiven%20mass%7D%7D%7B%5Ctext%20%7BMolar%20mass%7D%7D)
![3.04=\frac{96.0g}{\text {Molar mass}}](https://tex.z-dn.net/?f=3.04%3D%5Cfrac%7B96.0g%7D%7B%5Ctext%20%7BMolar%20mass%7D%7D)
![{\text {Molar mass}}=31.6g/mol](https://tex.z-dn.net/?f=%7B%5Ctext%20%7BMolar%20mass%7D%7D%3D31.6g%2Fmol)
The molar mass of the gas is 31.6 g/mol
Answer:
Such molecule must have molecular formula of C15N3H15
Explanation:
Mass of carbon in such molecule
![0.7595*240_{g/mol} =182.28_{g C/mol}](https://tex.z-dn.net/?f=0.7595%2A240_%7Bg%2Fmol%7D%20%3D182.28_%7Bg%20C%2Fmol%7D)
The atomic mass of carbon is 12.01 g/mol, so in 182.28 g of carbon there is 15.18 mols of carbon.
Mass of Nitrogen in such molecule
![0.1772*240_{g/mol} =37.73_{g C/mol}](https://tex.z-dn.net/?f=0.1772%2A240_%7Bg%2Fmol%7D%20%3D37.73_%7Bg%20C%2Fmol%7D)
The atomic mass of nitrogen is 14.01 g/mol, so in 42.53g of nitrogen there is 3.04 mols of nitrogen.
Mass of Hydrogen in such molecule
![0.0633*240_{g/mol} =15.19 {g C/mol}](https://tex.z-dn.net/?f=0.0633%2A240_%7Bg%2Fmol%7D%20%3D15.19%20%7Bg%20C%2Fmol%7D)
The atomic mass of Hydrogen is 1.00 g/mol, so in 15.19 g of Hydrogen there is 15.19 mols of Hydrogen.
Such molecule must have molecular formula of C15N3H15
Answer:
The answer is SiO2
Explanation:
Silocon dioxide is written without a 1 after the silocon and with a 2 after the oxygen.