Notes On Gaseous State This page provides you all details about the gaseous state of BSc standard. Concerned problems will be solved at the end of each concept. Continue till the end to find the easiest explanation of every concept you need in this regard . Postulates of Kinetic Theory of Gases: 1. All gas consist of a very large number of minute particles, called molecules. 2. The gas molecules are extremely small in size and are separated by large distance. The actual volume of the gas molecules is thus negligible as compared to the total volume occupied by the gas. 3. The pressure exerted by the gas is due to the bombardment of the molecules on the walls of the vessel. 4. The gas molecules collide with one another and also with the walls of the vessels. These collisions are perfectly elastic and there is no loss of energy during these collisions. 5. The distance between the gas molecules are very large. Thus, there is no effective force of attraction or r
Difference between Strength and Mole fraction Expressing the Concentration of a Solution: T he amount of solute present in a given quantity of solution or dissolved in a given amount of solvent is called the concentration of a solution . Depending on the units of the solute and solvents taken, the concentrations of a solution can be expressed in many ways. Strength (s): It is defined as the amount of solute in gram dissolved per litre of solution. S = (weight of solute in gram/ volume of solution in ml) X 1000. For example if 4gm urea is dissolved in 500 ml then strength of the solution, s = (4/500) x 1000 = 8 g/ltr Mole fraction (X): Mole fraction of a component in a solution is defined as the ratio of moles of that component to the total number of moles of all the components present in the solution. In a binary solution, if n 1 is the numbers of moles of solvent and n 2 is the numbers of moles of solute then, X solvent = n 1 / (n 1 + n 2 )