100 mL of phosphorus pentachloride is totally decomposed to its trichloride at 1 atm and `546^(@)C`. How many molecules of chlorine are formed?

Explanation

Decomposition of phosphorus pentachloride is given as
`PCl_(5)rarrPCl_(3)+Cl_(2)`
`"1 mole of "PCl_(5)="1 mole of"Cl_(2)`
`"1 vol of "PCl_(5)="1 vol fo Cl"_(2)`
`"100 mL of "PCl_(5)="100 mL of "Cl_(2)`
`{:("Given conditions","STP conditions"),(P_(1)="1 atm",P_(2)="1 atm"),(T_(1)="819 K",T_(2)="273 K"),(V_(1)="100 mL",V_(2)=?):}`
The volue of `Cl_(2)` measured at STP
`V_(2)=(P_(1)V_(1))/(T_(1))xx(T_(2))/(P_(2))=(1xx100xx273)/(819xx1)="33.33mL"`
`"22400 mL of "Cl_(2)" at STP"=`
`6.022xx10^(23)" molecules"`
`"33.33 mL of "Cl_(2)" at STP"=?`
Number of molecules of chlorine obtained `=(33.33)/(22400)xx6.022xx10^(23)=8.96xx10^(20)`