Answer:
4.67g
Step-by-step explanation:
Step 1:
The balanced equation for the reaction. This is given below:
Ca(OH)2 + 2HCl —> CaCl2 +2H2O
Step 2:
Determination of the mass of Ca(OH)2 that reacted and the mass of H2O produced from the balanced equation. This is illustrated below:
Molar Mass of Ca(OH)2 = 40 + 2(16 + 1) = 40 + 2(17) = 40 + 34 = 74g/mol
Molar Mass of H2O = (2x1) + 16 = 2 + 16 = 18g/mol
Mass of H2O from the balanced equation = 2 x 18 = 36g
From the balanced equation above,
74g of Ca(OH)2 reacted to produce 36g of H2O.
Step 3:
Determination of the mass of water (H2O) produced by the reaction 9.6g of calcium hydroxide, Ca(OH)2.
This is illustrated below:
From the balanced equation above,
74g of Ca(OH)2 reacted to produce 36g of H2O.
Therefore, 9.6g of Ca(OH)2 will react to produce = (9.6 x 36)/74 = 4.67g of H2O.
Therefore, the mass of the water (H2O) produced by reaction of 9.6g of calcium hydroxide, Ca(OH)2 is 4.67g.