Question

1.375 gram of copper oxide was reduced by hydrogen and 1.098 gram of copper was obtained in another experiment 1.178 gram of copper was dissolved in nitric acid and resulting copper nitrate was converted into copper oxide by ignition . The weight of copper oxide form was 1.476 grams show that the result Prove the law of constant proportion composition

Answer 1

Dear Student,

$$\begin{gathered} \mathrm{Experiment}1: \\ \mathrm{Mass}\mathrm{of}\mathrm{copper}\mathrm{oxide}\mathrm{taken}=1.375\mathrm{g} \\ \mathrm{Mass}\mathrm{of}\mathrm{copper}\mathrm{obtained}=1.098\mathrm{g} \\ \mathrm{Mass}\%\mathrm{of}\mathrm{copper}=\frac{1.098}{1.375}\times 100=79.86\% \\ \mathrm{Experiment}2: \\ \mathrm{Mass}\mathrm{of}\mathrm{copper}\mathrm{oxide}\mathrm{produced}=1.476\mathrm{g} \\ \mathrm{Mass}\mathrm{of}\mathrm{copper}\mathrm{used}=1.178\mathrm{g} \\ \mathrm{Mass}\%\mathrm{of}\mathrm{copper}=\frac{1.178}{1.476}\times 100=79.81\% \\ \mathrm{Since}\mathrm{the}\mathrm{percentage}\mathrm{of}\mathrm{copper}\mathrm{in}\mathrm{the}\mathrm{two}\mathrm{samples}\mathrm{of}\mathrm{copper}\mathrm{oxide}\mathrm{is}\mathrm{same}(\mathrm{within}0.5\%),\mathrm{hence}\mathrm{the}\mathrm{law}\mathrm{of}\mathrm{definite}\mathrm{proportion}\mathrm{is}\mathrm{verified}. \end{gathered}$$