Question

1.2g copper powder on heating
gave 6.0g of copper oxide.
another experiment copper oxide
containing 20% of oxygen - Show
that these results illustrate
the law of constant composition​

Answer 1

Answer:

1.2g +x = 6g

= x= 6g- 1.2 g= 4.8

so oxygen is 4.8g

prove,that oxygen is 20 percent

mass of copper/copper oxide×100

1.2g/6g×100=20

so it proved that oxygen is 20 percent and mass of oxygen will be 4.8 g

Answer 2

Answer:

The results from the calculation illustrate the law of constant composition because the percentage of oxygen in the copper oxide is always 20% regardless of the amount of copper oxide that is used. The law of constant composition states that the percentage of the elements in a chemical compound is always the same, regardless of the source or amount of the compound.

Explanation:

The balanced chemical equation of the reaction of copper and oxygen to form copper oxide is 2Cu + O2 → 2CuO. This equation shows that for every 2 moles of copper, 1 mole of oxygen is consumed. By using the molar mass, we can convert the mass of 6g of CuO to moles, which is 6/79 moles. Using the stoichiometry of the balanced equation, we can determine the number of moles of oxygen consumed which is (6/79) * (1/2) = 0.037 moles. We can convert it to mass using the molar mass of oxygen and calculate the percentage of oxygen in the copper oxide, which is (1.184/6) * 100 = 20%.

This illustrates the law of constant composition.

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