Question

32.05 ml of phosphorus vapour weigh 0.06225 g at 546° and 1 bar pressure .what is the molar mass of phosphorus?​

Answer 1

Answer:

Explanation:

p=0.1bar\\

V=34.05mL=34.05×10  

−3

L=34.05×10  

−3

dm  

3

R=0.083bardm  

3

k  

−1

mol  

−1

 

T=546°C=(546+273)K=819K

We can calculate the number of moles (n) by using the ideal gas equation : pV=nRT.

Replacing n by  

M

m

​  

, where, m=mass=0.0625g

M=Molecularmass, which we need to find.

pV=  

M

mRT

​  

 

So,M=  

PV

mRT

​  

=  

(0.1X34.05×10  

−3

)

(0.0625X0.083X819)

​  

 

=1247.5gmol  

−1