Laws Of Chemical Combinations

Concept: Chemistry (Basic Concepts) - Mole Concept and Atomicity.

Step 1: Determine the number of molecules in the given moles. One mole of any substance contains Avogadro's number ( ) of molecules. For 0.1 mole of : Number of molecules molecules.

Step 2: Identify the atomicity of the molecule. The formula for ammonia is . One molecule of ammonia consists of 1 Nitrogen atom and 3 Hydrogen atoms. Total atoms per molecule atoms.

Step 3: Set up the calculation for total atoms. Total atoms . Total atoms .

Step 4: Perform the multiplication. . So, Total atoms .

Step 5: Convert to standard scientific notation. To express the result in standard scientific notation, move the decimal one place to the left: atoms. This matches option B. $ $

The volume of 1 mole of any pure gas at

standard and pressure (STP) Is equal to

The combining ratios of hydrogen and oxygen in water and hydrogen peroxide are and . It is an example of law of multiple proportions. According to this law, if two elements combine together to form several compounds then weight of one of these elements, which combines with a fixed weight of the other, are in ratio of simple whole numbers.

The law of multiple proportions states that when two elements combine in more than one proportion to form different compounds, the masses of one element that combine with a fixed mass of the other element are in simple whole number ratios. H O and H O are examples of compounds formed by the combination of hydrogen and oxygen in different proportions, hence they illustrate this law.

The law of multiple proportions applies when two elements combine in different ways to form different compounds. Na S and NaF are not examples of this law because they do not differ in the proportions of the same elements.

The law of definite proportions states that a given compound always contains the same proportion of elements by mass, no matter how it is prepared.

Concept: Number of particles in one mole is given by Avogadro's number. Each molecule of glucose contains carbon atoms.

Step 1: Find the number of glucose molecules.

Step 2: Multiply by carbon atoms per molecule. Thus, the number of carbon atoms present is: