A 32.8 g sample of gas occupies 22.414 L at STP. What is the molecular weight of this gas?

32.8g/mole

Explanation:

Given parameters:

Mass of sample of gas = 32.8g

Volume  = 22.4L

Unknown:

Molecular weight  = ?

Solution:

To solve this problem we must understand that at rtp;

             1 mole of gas occupies a volume of 22.4L

Number of mole of the gas  = 1 mole

 Now;

   Mass  = number of moles x molecular weight

    molecular weight  =    =      = 32.8g/mole

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.

hydrocarbons are organic compounds that contain only hydrogens and carbons. they can be saturated (those which contain only carbon-carbon single bonds) or unsaturated (those which contain carbon-carbon double or triple bonds) in nature. hydrocarbons can undergo several reactions like substitution, elimination etc.  

on substituting one or more hydrogen atoms in hydrocarbon it results in the formation of haloalkane. as the halogen atoms are large compared to the carbon and hydrogen atoms, due to which the molecular weight increases and the bond become polar because of presence electronegative halogen atom and results in the increase in boiling point of the haloalkane.

thus, the correct option is (b) that is the boiling point of the new compound increases on substituting a hydrogen atom with a halogen in a hydrocarbon.