Question

1. Please explain law of multiple proportion with example.
2. Difference between molecular formula and empirical formula with example .

Answer 1

Answer:

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Answer 2

Explanation:

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1)

The Law of Multiple Proportions states:

“When two elements combine to form two or more chemical compounds, the ratio between different weights of one of the elements which combine with a fixed weight of the other is always simple.”

Examples:

Compound of Carbon and Oxygen : C and O combine to form two compounds CO and CO2

In CO, 12 parts by wt. of C combine with 16 parts by wt. of O.

In CO2,12 parts by wt. of C combine with 32 parts by wt. of O.

If the weight of C is fixed at 12 parts of wt. then the ratio in the weights of oxgyen which combine with the fixed wt. of C (= 12) is 16 : 32 or 1:2.

Thus the weights of oxygen bear a simple ratio of 1 : 2 to each other.

2)

Molecular formula

• The molecular formula is the formula derived from molecules and is representative of the total number of individual atoms present in a molecule of a compound.

• A molecular formula uses subscript that reports the actual number of each type of atom in a molecule of the compound.

• Molecular formulas are associated with gram molecular masses that are simple whole number multiples of the corresponding empirical formula mass.

Emperical formula

• The empirical formula is the simplest formula for a compound which is defined as the ratio of subscripts of the smallest possible whole number of the elements present in the formula. It is also known as the simplest formula.

• An empirical formula for a compound is the formula of a substance written with the smallest integer subscript.

• The empirical formula gives information about the ratio of numbers of atoms in the compound. The percent composition of a compound directly leads to its empirical formula.

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