Reaction produces 74.10 g Ca(OH)2 after 56.0 g CaO is added to 36.04 g H2O. How should the difference of masses of reactants and products be explained? CaO+ H2O -> Ca(OH)2 A. Not all of the calcium oxide reacted, because it is the limiting reactant

B. A side reaction produced gaseous CO2 that escaped from the system

C. The reaction that occurred was a nuclear change in which some matter was converted into energy

D. Some water was an excess and makes up the difference in mass

Cao +  H2O  >Ca(OH)2

Calculate   the  number  of  each   reactant  and  the  moles  of  the  product

that  is

moles = mass/molar mass

The  moles  of  CaO=  56.08g/  56.08g/mol(molar  mass  of  Cao)=  1mole

the  moles  of  water=  36.04 g/18  g/mol=  2.002moles

The   moles  of Ca (OH)2=74.10g/74.093g/mol= 1mole

The  mass  of differences  of  reactant  and  product  can   be  therefore  

explained  as  

1  mole   of  Cao  reacted  completely   with   1  mole   H2O  to  produce  1 mole  of  Ca(OH)2. The  mass  of  water   was  in  excess  while  that  of  CaO  was  limited

Explanation:

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