Question

# A 0.24g sample of a compound of oxygen and boron was found by analysis to contain 0.096g of boron and 0.144g of oxygen. Calculate the percentage composition of the compound by weight.

Open in App
Solution

## Given that:The Mass of the sample = 0.24gMass of boron in the given sample = 0.096 gMass of oxygen in the given sample = 0.144 g% composition of compound = [% of boron] + [% of oxygen]Therefore, $%\mathrm{composition}\mathrm{of}\mathrm{boron}=\frac{\mathrm{Mass}\mathrm{of}\mathrm{boron}}{\mathrm{Mass}\mathrm{of}\mathrm{sample}\mathrm{compound}}×100$$%\mathrm{composition}\mathrm{of}\mathrm{boron}=\frac{0.096}{0.24}×100=40%$Therefore, $%\mathrm{composition}\mathrm{of}\mathrm{oxygen}=\frac{\mathrm{Mass}\mathrm{of}\mathrm{oxygen}}{\mathrm{Mass}\mathrm{of}\mathrm{sample}\mathrm{compound}}×100$$%\mathrm{composition}\mathrm{of}\mathrm{oxygen}=\frac{0.144}{0.24}×100=60%$The percentage composition of the boron and oxygen in the compound by weight is 40% and 60% respectively.

Suggest Corrections
9