Question

0.2475g of an organic compound gave on combustion 0.4950g of carbon dioxide and 0.2025 g of water. The percentage of carbon and hydrogen are

Answer 1

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Answer 2

The percentage by mass of carbon and hydrogen in organic compound is 54.5 % and 9.09 %

Explanation:

We are given:

Mass of $CO_2=0.4950g$

Mass of $H_2O=0.2025g$

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 0.4950 g of carbon dioxide, $\frac{12}{44}\times 0.4950=0.135g$ of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 0.2025 g of water, $\frac{2}{18}\times 0.2025=0.0225g$ of hydrogen will be contained.

To calculate the mass percentage of element in sample, we use the equation:

$\text{Mass percent of element}=\frac{\text{Mass of element}}{\text{Mass of sample}}\times 100$

• For carbon:

Mass of carbon = 0.135 g

Mass of sample = 0.2475 g

Putting values in above equation, we get:

$\text{Mass percent of carbon}=\frac{0.135g}{0.2475g}\times 100=54.5\%$

• For hydrogen:

Mass of hydrogen = 0.0225 g

Mass of sample = 0.2475 g

Putting values in above equation, we get:

$\text{Mass percent of hydrogen}=\frac{0.0225g}{0.2475g}\times 100=9.09\%$

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