Question

. When 6.2g of phosphorus was combined with oxygen, 14.2g of an oxide compound of phosphorus was produced. What is the percentage composition of the compound?

Answer 1

Answer:

When 6.2g of phosphorus was combined with oxygen, 14.2g of an oxide compound of phosphorus was produced. The percentage composition of the compound is the percent of total mass made up by a specific element. It can be the molar mass of H20 is 18 g/mol. The oxygen makes up 16g.

Answer 2

Given:

6.2 g of phosphorous combines with oxygen.

14.2 g of phosphorous oxide is formed.

To find:

The percentage composition of the compound.

Formula to be used:

$%composition=\frac{mass-of-element}{mass-of-compound}*100$$%composition=\frac{mass-of-element}{mass-of-compound} *100$$%composition=\frac{mass-of-element}{mass-of-compound} *100$$percentage-composition=\frac{mass-of-element}{mass-of-compound} *100$

Step-by-step explanation:

Step 1 of 1

The amount of phosphorous taken is 6.2g.

The amount of oxygen that must be taken will be 14.2-6.2=8.0g.

$percentage-of-phosphorous=\frac{6.2}{14.2} *100\\\\=43.66%$

$percentage-of-oxygen=\frac{8}{14.2} *100\\\\=56.338%$

The percentage composition of phosphorous oxide is:

43.66% phosphorous and 56.33% oxygen.