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

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Snoopycatlover Snoopycatlover · Answer 1 · 2021-09-20T06:38:38+02:00

Answer:

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:

AarushiAanand AarushiAanand · Answer 2 · 2022-07-12T08:16:48+02:00

The mass difference between reactant and product in the given reaction is " Some water was an excess and makes up the difference in mass".

The quantity of matter that makes up every object or body is the greatest way to understand mass. Everything that we can see has mass.

In a chemical reaction, reactants were chemicals that have been initially present and are utilized to create products.

Calculation of moles

Moles can be determined by a formula.

Moles = Mass / molar mass

Given data

Mass of CaO = 56.0 g

Mass of water = 36.04 g

Moles of CaO = Mass / molar mass

Moles of CaO = 56.0 g / 56.0 g = 1 mole.

Moles of water = 36.04 g / 18 g/mol = 2.002 moles.

Moles of Ca(OH)2 = 74.10 g / 74.10 g/mol = 1 mole.

It can be seen that 1 mole of calcium oxide (CaO ) will be reacted completely. The water was an excess and makes up the difference in mass.

To know more about the mass.

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