Question

In an experiment, 18.5 g of copper sulphate reacted with 11.0 g of sodium hydroxide
to form 10.0 g of copper hydroxide and 19.5 g of sodium sulphate. How would you
explain this observation by relating to an appropriate law of chemical combination?​

Answer 1

Total mass of reactants are equal to the total mass of the products. Hence the law of chemical combination is valid here.

Step by step explanation:

Law of chemical combination:

"Sum of masses of the reactants is always equal to the masses of products."

In the given experiment,

The chemical reaction is as follows.

$\bold{CuSO_{4}+NaOH\rightarrow Cu(OH)_{2})+NaSO_{4}}$

From the given,

Masses of reactants:

Mass of copper sulphate = 18.5 g

Mass of sodium hydroxide = 11.0 g

Total mass                          = (18.5 +11.0)g =29.5 g

Masses of products:

Mass of copper hyroxide = 10.0 g

Mass of sodium sulphate = 19.5 g

Total mass                          = (10.0 +19.5)g =29.5 g

Here, mass of reactants are equal to the mass of products.

Hence, Law chemical combination can be proved.

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