Weight of copper oxide obtained by heating `2.16 g` of metallic copper with `HNO_(3)` and subsequent ingnition was `2.70 g` In another experient, `1.15 g` of copper oxide on reduction yielded `0.92 g` of copper. Show that the results illustrance the law of definite proportions.

Weight of copper oxide obtained by treating 2.16 g metallic copper with nitric acid and subsequent ignition was 2.70 g. In another experiment, 1.15 g of copper oxide on reduction yielded 0.92 g of copper. Show that these results illustrate the law of definite proportions.

2.16 of copper metal when treated with nitric acid followed by ignition of the nitrate gave 2.70 g of copper oxide. In another experiment 1.15 g of copper oxide upon reduction with hydrogen gave 0.92 g of copper. Show that the above data illustrate the Law of Definite Proportions.

In an experiment, 1.288g of copper oxide was obtained from 1.03 g of copper. In another experiment 3.672 g of copper oxide gave, on reduction, 2.938 g of copper. Show that these figures verify the law of constant proportions.

A simple iron oxide was found to contain 72.17% iron. 2 g of the oxide from another source gave 1.44 g of iron. Show that the results illustrate law of definite proportions.

In an experiment, 4.90 g of copper oxide was obtained from 3.92 g of copper. In another experiment, 4.55 g of copper oxide gave, on reduction, 3.64 g of copper. Show with the help of calculation that these figures verify the law of constant proportions.

1.08 g of copper wire was allowed to react with nitric acid. The resulting solution was dried and ignited when 1.35 g of copper oxide was obtained. In another experiment 2.30 g of cpper oxide was heated in presence of hydrogen yielding 1.84 g of copper. Show that the above data in accordance with law of constant proporation.