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:

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation:

answer; economic order quantity;