Chemistry Law of Definite and Multiple Proportions
Give an example of Law of Multiple Proportions.
Let's say we have the element Nitrogen monoxide. It is composed of one nitrogen atom and one oxygen atom. now in Nitrogen Dioxide you still have one atom of Nitrogen, but 2 atoms of oxygen. Nitrogen has an atomic mass of about 14. Oxygen has an atomic mass of about 16. So the ratio of mass in nitrogen monoxide is 14:16 or 7:8. In nitrogen dioxide it is 14:32 or 7:16. Then you would divide the 7/8 and get for every 1 g of oxygen there is 0.875 g of nitrogen. This can also be used to figure out nitrogen dioxide if you didn't already know it by multiplying it by 2.
Give an example of Law of Definite Proportions.
Water, written as the chemical compound H2O, is made up of atoms of hydrogen and oxygen. If one oxygen atom is combined with two hydrogen atoms, water is created. An oxygen atom has an atomic mass of 16, while a hydrogen atom has an atomic mass of 1. This means that water is made up of 11% hydrogen and 89% oxygen. The exact same proportion of hydrogen and oxygen must always be combined in order for water to be created.
State the Law of Definite Proportions
When a chemical compound is always found to be made up of the same element combined together in the same fixed proportion by mass.
State the Law of Multiple Proportions and give an example.
Whenever the same two elements form more than one compound, the different masses of one element that combines with the same mass of the other element are in the ratio of small whole numbers.
