Question

a compound contain 69.5% oxygen and 30.5% notrogen and its molecular weight is 92. what is the formula of compound

Answer 1

Answer:

Molecular formula of the compound is N2O4.

Explanation:

Given:

Compound contain 69.5% of Oxygen

30.5% Nitrogen

Molecular weight = 92.

Solution:

Let us assume 100g of compound.

So, Mass of Oxygen = 69.5 grams and Mass of Nitrogen = 30.5 grams.

Let us first calculate the number of moles of each element.

No. of moles = Mass / Molar mass

No. of moles of oxygen = 69.5/16 = 4.34

No. of moles of nitrogen = 30.5/14 = 2.18

Ratio of moles of Nitrogen  and Oxygen = 2.18 : 4.34  = 1 : 2

So, the Empirical formula of the compound is NO2

Molecular formula is given by (NO2)n

Here,

n = Molecular mass / Empirical mass

Empirical mass = (1 * 14) + (2 * 16) = 46

n = 92/46 = 2

So,

Formula of the compound is N2O4.

Answer 2

Explanation:

Answer

Answer:

Molecular formula of the compound is N2O4.

Explanation:

Given:

Compound contain 69.5% of Oxygen

30.5% Nitrogen

Molecular weight = 92.

Solution:

Let us assume 100g of compound.

So, Mass of Oxygen = 69.5 grams and Mass of Nitrogen = 30.5 grams.

Let us first calculate the number of moles of each element.

No. of moles = Mass / Molar mass

No. of moles of oxygen = 69.5/16 = 4.34

No. of moles of nitrogen = 30.5/14 = 2.18

Ratio of moles of Nitrogen  and Oxygen = 2.18 : 4.34  = 1 : 2

So, the Empirical formula of the compound is NO2

Molecular formula is given by (NO2)n

Here,

n = Molecular mass / Empirical mass

Empirical mass = (1 * 14) + (2 * 16) = 46

n = 92/46 = 2

So,

Formula of the compound is N2O4.