Law of constant proportions

Chemistry Level 1

When 1.375 g of cupric oxide is reduced on heating in a current of hydrogen, the weight of copper remaining is 1.098 g. In another experiment, 1.179 g of copper is dissolved in nitric acid and the resulting copper nitrate is converted into cupric oxide by ignition. The weight of cupric oxide formed is 1.476 g.

Does this situation verify law of constant proportions?

Yes No

2 solutions

Anusha Gupta
May 10, 2021

In the first method of preparation , the percentage composition of Cu is found out to be 79.8% ( $\frac{1.098}{1.375}$ *100 ). In the second method of preparation , the the percentage composition of Cu is also found out to be 79.8% ( $\frac{1.179}{1.476}$ *100 ). As Cu is present in constant proportion in both the methods , the law is satisfied.

Yep nicely written

Md Zuhair - 5 days, 19 hours ago

Rigveda Gupta
Jul 16, 2020

in 1.375 g CuO the proportion is 1/1 in both first reaction and second reaction proportion of Cu is 1 in both first and second reaction So, this reaction follows law of constant proportion

Law of constant proportions

2 solutions

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