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Question: The density of phosphorus vapor at 310\[^{o}C\] and 775 torr is 2.64\[g\text{ }d{{m}^{-3}}\]. What i...

The density of phosphorus vapor at 310oC^{o}C and 775 torr is 2.64g dm−3g\text{ }d{{m}^{-3}}. What is the molecular formula of phosphorus?

Explanation

Solution

Using the density, we can find the ratio of mass by volume which will be used in the formula to calculate the molar mass. We can calculate the molar mass of gas vapor using the below formula.
PV= nRT
P = pressure, V = volume, R = gas constant, T = temperature
n = massmolar mass\dfrac{mass}{molar\text{ }mass}

Complete answer:
In the question it is given that density ρ\rho = 2.64 g dm−3g\text{ }d{{m}^{-3}}= 2.64 g/L
The pressure of the vapour P = 775 mm
Temperature of the phosphorus vapor = 310 +273 = 583 K
We have to convert pressure in mm into atm.
775 mm = 775760=1.02atm\dfrac{775}{760}=1.02atm
Gas constant R = 0.0821 liter/atm. K. mol
Now substitute all the above formulas in the equation PV = nRT

& PV=\dfrac{mass}{molar\text{ }mass}RT \\\ & molarmass=\dfrac{mass}{P\times V}RT \\\ \end{aligned}$$ We know that density = $$\dfrac{mass}{volume}$$ Therefore molar mass = $$\dfrac{\rho }{P}RT$$(where$$\rho $$= density) $$\begin{aligned} & =\dfrac{2.64\times 0.0821\times 583}{1.02} \\\ & =123.88g \\\ \end{aligned}$$ We know that Molar mass of the one phosphorus atom = 31 g There is a formula to calculate the number of phosphorus atoms Number of atoms $$\begin{aligned} & =\dfrac{molar\text{ }mass}{atomic\text{ }weight} \\\ & =\dfrac{123.88}{31} \\\ & =4 \\\ \end{aligned}$$ That means there are four phosphorus atoms in the phosphorus molecule. So, the molecular formula of phosphorus molecules is$${{P}_{4}}$$. **Note:** The structure of the white phosphorus molecule is as follows. ![](https://www.vedantu.com/question-sets/ff41684c-3b28-4f5e-b430-2cee7dddf2983745645722348548957.png) The phosphorus atoms are arranged in a tetrahedral structure. Phosphorus molecules exist in two allotropic forms. One is white phosphorus and another is red phosphorus. While solving this problem, remember to convert the pressure given here in mm to atm. Use the value of R which has the unit atm in it i.e 0.0821 liter/atm. K. mol. There are other values also for R, but since the pressure is converted here into atm, we have to use the above value.