Atoms of different elements combine in fixed, small whole-number ratios to form compounds.

Atoms of different elements combine to form a molecule of

One of the statements of Dalton's atomic theory is given below "Compound are formed when atoms of different element combine in a fixed ratio " Which of the following laws is not related to this statement?

Formula showing simplest whole number ratio is :

A ________ is always made up of different elements combined in a fixed ratio by mass.

Atomic mass of an element is not neccessurity a whole number because

The atoms of different elements having same mass number but different atomic number are known as isobars. The sum of protons and neutrons, in the isobars is always different.

This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number. For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide. Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2 . N_(2) and O_(2) combine to form a number of compounds such as NO,N_(2)O,N_(2)O_(3),N_(2)O_(5) . Show that these follow the law of multiple proportion.

This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number. For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide. Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2 . An element forms two oxides .In one oxide ,one gram of the oxide containd 0.5g of the element. In another oxide, 4g of the oxide contains 0.8g of the element . Show that these data confirm the law of multiple proportion.

This law was proposed by Dalton in 1803 . According to this law , if two elements combune to form more than one compounds ,the masses of one element that combine with a fixed mass of the other element, are in the ratio of small whole number. For exemple, hydrogen combines with oxygen to form two compounds ,namely, water and hydrogen peroxide. Here, the masses of oxygen (i.e, 16g and 32g) which combine with a fixed mass of hydrogen (2g) bear a simple raio, i.e, 16 :32 or 1 :2 0.11 g of an oxide of nitrogen gives 56 Ml N_(2) at 273K and 1 atm. 0.15 g of another oxide of nitrogen gives 56mL N_(2) at 1 atm , 273K. Show that these data confirm the law of multiple proportion.

Assertion: Molecular formula shows the exact number of different types of atoms present in a molecule of a compound. Reason : Molecular formula can be obtained directly from empirical formula which represents the simplest whole number ratio of various atoms present in a compound.