Question

What is the density (in g/L) of a gas with a molar mass of 16.01 g/mol at 1.75 ATM and 337 K?

Answer 1

you can use this formula to solve for density--> Density= PM/ RT, where P is pressure, M is molar mass, R is the gas constant and T is temperature.

P= 1.75 atm
M= 16.01 g/ mol
R= 0.0821 atm·L/ mol·K
T=337 k

density= (1.75 x 16.01)/ (0.0821 x 337)= 1.01 g/L

Answer 2

Answer : The density of a gas is, 1.013 g/L

Solution : Give,

Molar mass of gas = 16.01 g/mole

Pressure of gas = 1.75 atm

Temperature of gas = 337 K

Using ideal gas law equation,

`PV=nRT`

`PV=(w)/(M)* RT\\\\P=(w)/(V)* (RT)/(M)\\\\P=\rho* (RT)/(M)\\\\\rho=(PM)/(RT)`

As we know that
`Density=(Mass)/(Volume)`

where,

P = pressure of the gas

V = volume of the gas

T = temperature of the gas

n = number of moles of the gas

w = given mass of gas

M = molar mass of gas

R = gas constant = 0.0821 Latm/moleK

`\rho` = density of gas

Now put all the given values in the above formula, we get the density of the gas.

`\rho=(PM)/(RT)`

`\rho=((1.75atm)* (16.01g/mole))/((0.0821Latm/moleK)* (337K))=1.013L`

Therefore, the density of a gas is, 1.013 g/L