(B) The mass ratio of $C : H : N$ is $9 : 1 : 3.5$.To find the molar ratio,divide the mass of each element by its atomic mass $(C = 12, H = 1, N = 14)

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(B) The mass ratio of $C : H : N$ is $9 : 1 : 3.5$.To find the molar ratio,divide the mass of each element by its atomic mass $(C = 12, H = 1, N = 14)$:Molar ratio of $C : H : N = \frac{9}{12} : \frac{1}{1} : \frac{3.5}{14} = 0.75 : 1 : 0.25$.To simplify the ratio,divide each value by the smallest value $(0.25)$:$\frac{0.75}{0.25} : \frac{1}{0.25} : \frac{0.25}{0.25} = 3 : 4 : 1$.Therefore,the empirical formula is $C_3H_4N$.

Class 11 Chemistry Some Basic Concepts of Chemistry Percentage composition and Molecular formula

Difficult

$A$ compound of carbon,hydrogen,and nitrogen contains three elements in the respective ratio of $9 : 1 : 3.5$ grams. The empirical formula for the compound is

A
$C_2H_4N$
B
$C_3H_4N$
C
$C_3H_6N$
D
$C_2H_6N$

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Some Basic Concepts of Chemistry

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Percentage composition and Molecular formula

An organic compound contains $C = 74.0\%$,$H = 8.65\%$ and $N = 17.3\%$. Its empirical formula is:

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Which one has the highest percentage of nitrogen?

MediumAIPMT 1993

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In an analysis,the ratio of iodine to oxygen in a certain substance is $254:80$. What will be the formula of this substance? (Atomic mass $I = 127$,$O = 16$)

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$A$ gaseous compound of nitrogen and hydrogen contains $12.5\%$ (by mass) of hydrogen. The density of the compound relative to hydrogen is $16$. The molecular formula of the compound is

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$A$ compound containing $Xe$ and $F$ has $63.8\%$ of $Xe$ by mass. Calculate the oxidation number of $Xe$ in this compound.

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$A$ compound of carbon,hydrogen,and nitrogen contains three elements in the respective ratio of $9 : 1 : 3.5$ grams. The empirical formula for the compound is

Similar Questions

An organic compound contains $C = 74.0\%$,$H = 8.65\%$ and $N = 17.3\%$. Its empirical formula is:

Which one has the highest percentage of nitrogen?

In an analysis,the ratio of iodine to oxygen in a certain substance is $254:80$. What will be the formula of this substance? (Atomic mass $I = 127$,$O = 16$)

$A$ gaseous compound of nitrogen and hydrogen contains $12.5\%$ (by mass) of hydrogen. The density of the compound relative to hydrogen is $16$. The molecular formula of the compound is

$A$ compound containing $Xe$ and $F$ has $63.8\%$ of $Xe$ by mass. Calculate the oxidation number of $Xe$ in this compound.

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