Question

Carbon forms two oxides in which the weight of oxygen combines with 1 g of carbon

are 1.33 g and 2.66 g respectively. What law is in agreement with this observation?
Give reasons.​

Answer 1

This is based on the masses of one element, that will be combined with a fixed mass of the other element.

Step-by-step explanation:

This is based on the masses of one element, that will be combined with a fixed mass of the other element. Thoses masses are in a ratio.

This state we can find in 'The Law of Multiple Proportions, which is part of Dalton's atomic theory

We see that in the 2 compounds, the masses of oxygen, that combine with a fixed mass of carbon , will be in proportion.

For the first oxide we have 1g carbon per 1.33 g Carbon

1g /1.33g = 0.752

For the second oxide we have 1g carbon per 2.66g Carbon

1g/2.66g = 0.376

Dividing the mass O per g C of the second (larger value) compound:

2.66 / 1.33 = 2 which is the same as 0.752 / 0.376

thus, it means that the masses of oxygen that combine with carbon are in a 2:1 ratio.