Question

What is the mass of ${H_2}O$ in $1000kg$ of $CuS{O_4}.10{H_2}O$ ? (Atomic weight of $Cu = 63.5$ ).

Answer 1

We have to know that mass is the measure of issue in an article. Move to an alternate planet and an item's weight will change, however its mass will be something similar. There are few different ways to gauge mass. The most well-known technique is to utilize an equilibrium.

Complete answer:
The balanced chemical equation is given below,
$CuS{O_4}.10{H_2}O \to CuS{O_4} + 10{H_2}O$
We have to know that, in the given details,
The mass of $CuS{O_4}.10{H_2}O$ = $1000kg$
First we have to calculate the number of moles of $CuS{O_4}.10{H_2}O$ .
By using the following expression,
$No.{\text{ of moles = }}\dfrac{{Mass}}{{Molarmass}}$
Where,
Mass = $1000kg$
Molar mass of $CuS{O_4}.10{H_2}O$ = $339.76$
Applying both the values in the above mole formula,
$No.{\text{ of moles = }}\dfrac{{1000}}{{339.76}} = 2.94mol{\text{ }}\left( {kilo{\text{ moles}}} \right)$
Now, we have to calculate the number of moles of water. The number of moles of $CuS{O_4}.10{H_2}O$ is multiplied by the value ten, then, we have to get the number of moles of water.
$No.{\text{ of moles of }}{{\text{H}}_2}O = 10 \times 2.94 = 29.4mol{\text{ }}\left( {kilo{\text{ moles}}} \right)$
Therefore,
The number of moles of water molecules is $29.4mol$ .
Finally, we have to calculate the mass of water.
By using the following expression,
$Mass = No.{\text{ of moles}} \times {\text{Molar mass}}$
Where,
The number of moles = $29.4mol$
The molar mass of water = $18$
Applying both the values in the above mass expression,
$Mass{\text{ of }}{{\text{H}}_2}O = 29.4 \times 18 = 529.78kg$ .
Hence, the mass of water is $529.78kg$ .

Note:
We have to know that the mole unit is vital and valuable in science. It is the foundation of stoichiometry and it is giving the most-ideal choice to communicating measures of reactants and items devoured and shaped during any synthetic response. We may compose every one of the synthetic responses as a mole connection.