Question

tin forms two oxides the percent of tin in the two oxides is 78.77% and 88.12% show that these data confirms the law of multiple proportion

Answer 1

Given,

Percentage of tin in oxide 1 = 78.77%

Percentage of tin in oxide 2 = 88.12%

To Prove,

Show this data confirms the law of multiple proportions.

Solution,

In the first compound,

Mass of tin = 78.77g

Mass of oxygen = 100g - 78.77g = 21.23g

Mass of tin combined with 1g of oxygen = $\frac{78.77}{21.23} =3.71g$

In the second compound,

Mass of tin = 88.12g

Mass of tin = 100g - 88.12g = 11.88g

Mass of tin combined with 1g of oxygen = $\frac{88.12}{11.88} = 7.42g$

Ratio of tin combining with fixed 1g of oxygen = 3.71 : 7.42

                                                                                = 1:2

Hence this is a simple ratio, therefore this data proves the law of multiple proportions.

Answer 2

Law of Multiple Proportions definition:

• The law of multiple proportions state that if 2 elements can combine to form 2 different compounds, then the masses of one element that combines with a fixed mass of the other element, will always be ratios of whole numbers.
• For example, if we consider two elements A and B forming two separate compounds with one another, then:
• $\frac{ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 1st \hspace{1 mm}compound}{ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 2nd\hspace{1 mm}compound} = a\hspace{1 mm}small\hspace{1 mm} whole \hspace{1 mm}number$
• so, this law gives a relation between the compounds formed by 2 elements formed with one another.

In this question we can observe:

Given:

• % of tin in 1st compound= 78.77 %
• % of oxygen in 2nd compound= (100-78.77)%= 21.23 %
• % of tin in 1st compound= 88.12 %
• % of oxygen in 2nd compound= (100-88.12)%= 11.88 %

Now,

$ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 1st \hspace{1 mm}compound = \frac{78.77}{21.23} = 3.7103$

$ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 2nd \hspace{1 mm}compound = \frac{88.12}{11.88} = 7.4175$

Therefore we can see, the ratio turns out to be:

$\frac{ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 1st \hspace{1 mm}compound}{ratio\hspace{1 mm} of \hspace{1 mm}A \hspace{1 mm}and\hspace{1 mm} B\hspace{1 mm} in\hspace{1 mm} 2nd\hspace{1 mm}compound} = \frac{7.4175}{3.7103} = 1.999 = 2$

Since 2 is a small whole number, we can say that these data confirms the law of multiple proportions.