In this post, I am sharing FSC 1st Year Chemistry Chapter 8 Solved Exercise & Numericals Notes PDF for the students of FSC Part 1. The name of 11th Chemistry Chapter 8 is Chemical Equilibrium. So the students can download Chemical Equilibrium Chapter Solved Exercise in PDF format from here. This file contains 31 pages. These Chemistry Notes are for all the boards working under Punjab Board like Gujranwala Board, Lahore Board, Faisalabad Board, Multan Board, Rawalpindi Board, Sargodha Board, DG Kahn Board, and Sahiwal Board. Here are the complete 1st Year Chemistry Notes.
11th Class Chemistry Chapter 8 “Chemical Equilibrium” Solved Exercise PDF Download
FSC Part 1 Chemistry Chapter 8 Chemical Equilibrium Solved Exercise
Fill in the blanks:
1) Law of mass action states that the Rate at which a reaction proceeds, is directly proportional to
the product of the active masses of the Reactant.
2) In an exothermic reversible reaction, Low temperature will shift the equilibrium toward the
3) In a gas phase reaction, if the number of moles of reactants are equal to the number of moles of the
products, Kc of the reactant is equal to the Kp.
4) Buffer solution is prepared by mixing together a weak base and its salt with strong acid or a weak
acid and its salt with strong base.
What is the justification for the increase of ionic product with temperature?
When temperature of water is increases, the dissociation of water molecules into its component ions is also increases. With the increasing concentration, of H+ and OH-1 ions in water the ionic product of water(Kw) also increases.
What happened to the acidic and basic properties of aqueous solutions when pH varies from zero to 14?
when pH varies from 0 to 7, acidic properties of aqueous solution increases and when it varies from 7 to 14 to basic properties of aqueous solution increases.
the solution is acidic when pH value is between zero and 7 and is basic when pH value is between 7 and 14.
“ The negative logarithm of hydrogen ion concentration in the solution is called pH”.
pH = -log[H+]
“ The negative logarithm of hydrogen of hydroxide ion concentration in the solution is called pOH”.
pOH = -log[OH–]
what should be the possible effect of change of temperature at equilibrium state?
Since reaction is exothermic in forward direction, increase of temperature will shift equilibrium towards right. Hence low temperature shifts the equilibrium towards right and yield is increase
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