On complete combustion of a hydrocarbon 0.88g of carbon (iv) oxide and 0.36g of water
were formed (i) calculate the molecular formula of the hydrocarbon given that relative
molecular mass of the hydrocarbon is 70. (c = 12, O= 16)

the volume increases

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.