In the reaction to prepare chlorine gas,4.35g of manganese dioxide (MnO2) reacted with concentrated hydrochloric acid (HCI) according to the following equation: MnO2 + 4HCI = MnCL2 + 2H2O + Cl2
i) how many moles of manganese dioxide were there in the 4.35 g sample?
ii) how many moles of hydrochloric acid were required to reacy with 4.35g of manganese dioxide.
iii) Calculate the maximum number of water molecules that could be produced.
iv) how many atoms of hydrigen did this number of water molecules contain?

mncL2 is the water molecule

the answer is c. nacl

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.