Irrespective of the source,a pure sample of water always yields $88.89\%$ mass of oxygen and $11.11\%$ mass of hydrogen. This is explained by the law of

$1.0 \ g$ of an oxide of $A$ contained $0.5 \ g$ of $A$. $4.0 \ g$ of another oxide of $A$ contained $1.6 \ g$ of $A$. The data indicate the law of:

Explain the Law of Multiple Proportions.

Write about Dalton's Atomic Theory.

Hydrogen combines with oxygen to form $H_2O$ in which $16 \ g$ of oxygen combine with $2 \ g$ of hydrogen. Hydrogen also combines with carbon to form $CH_4$ in which $2 \ g$ of hydrogen combine with $6 \ g$ of carbon. If carbon and oxygen combine together then they will do so in the ratio of

Which of the following pairs of substances illustrates the Law of Multiple Proportions?