Question

0.24g sample of a compound of oxygen and boron was by analysis to contain 0.144g of oxygen and 0.096 of boron. calculate the percentage composition of the compound by weight​

Answer 1

Answer:

Given:- Mass of compound = 0.24g

Mass of boron. = 0.096g

Mass of oxygen = 0.144g

$precentage \: of \: boron \: = \frac{mass \: of \: boron}{mass \: of \: compound } \times 100$

$= \frac{0.096}{0.24} \times 100 = 40\%$

$percentage \: of \: oxygen = \frac{mass \: of \: oxygen}{mass \: of \: compound} \times 100$

$= \frac{0.144}{0.24} \times 100 = 60\%$

Hence the percentage of boron is 40% and percentage of oxygen is 60% by mass

Answer 2

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