Question

I will give brainliest!!! What is the density of a sample of chlorine gas that exerts a pressure of 4.5 atm in a 12.6 L container at 36 c (Answer in 4 digits)
Please help I'm so confused!

Answer 1

Answer : The density of a sample of chlorine gas is, 12.59 g/L

Explanation :

To calculate the density of chlorine gas we are using ideal gas equation.

$PV=nRT\\\\PV=\frac{w}{M}RT\\\\P=\frac{w}{V}\frac{RT}{M}\\\\P=\frac{\rho RT}{M}$

where,

P = pressure of chlorine gas = 4.5 atm

V = volume of chlorine gas = 12.6 L

n = number of moles of chlorine gas

w = mass of chlorine gas

R = gas constant = 0.0821 L.atm/mol.K

T = temperature of chlorine gas = $36^oC=273+36=309K$

M = molar mass of chlorine gas = 71 g/mol

Now put all the given values in the above formula, we get:

$P=\frac{\rho RT}{M}$

$4.5atm=\frac{\rho \times (0.0821L.atm/mol.K)\times (309K)}{71g/mol}$

$\rho=12.59g/L$

Therefore, the density of a sample of chlorine gas is, 12.59 g/L