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Chemical Equilibrium: Part-1 : Crash Course (in Hindi)
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This video explains the concept of equilibrium , Law of mass action & law of Chemical Equilibrium. The lesson is important for Preparations of NEET , JEE & AIIMS examination.

Pradeep Sharma
Educator | Chemistry | NEET | JEE Teaching students for Cracking NEET , IIT-JEE , AIIMS , XII & XI since 1998.

U
Unacademy user
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Sir atomic structure ki videos upload kar dijiye please
thanks for videos.. sir ionic equilibrium bhi daal do plz
Pradeep Sharma
2 years ago
Nice to know ..your request will be completed soon
Swati Singh
2 years ago
again thanks...sir for such a concern for the viewer's.
  1. Chemical equilibrium Part-1


  2. Chemical equilibrium Part-1


  3. Chemical equilibrium Part-1


  4. EQUILIBRIUM It may be defined as a condition at which rate of forward reaction becomes equal to rate of backward reaction. Rate of forward reaction Rate of backward H2O(s)H2O (I) CH3COOH + CH3OH CH3COOCH3 + H2O


  5. EQUILIBRIUM It may be defined as a condition at which rate of forward reaction becomes equal to rate of backward reaction. TYPES OF EQUILIBRIUM 1. PHYSICAL EQUILIBRIUM 2. CHEMICAL EQUILIBRIUM H20(s)H2O () HOs)CHCOOH CH,OHCH.COOCH + H2O CH3COOCH3 H20


  6. Law of mass Action Given by Guldberg & Waage The rate of reaction is directly proportional to the product of active masses of reactants ,each raised to the power equal to its coefficient as represented by balanced chemical Rate o [ Conc. of reactant ] "


  7. Law of mass Action Given by Guldberg & Waage The rate of reaction is directly proportional to the product of active masses of reactants ,each raised to the power equal to its coefficient as represented by balanced chemical Rate o [ Conc. of reactant ] " Rate a [A] [B]b


  8. Law of mass Action Given by Guldberg & Waage The rate of reaction is directly proportional to the product of active masses of reactants ,each raised to the power equal to its coefficient as represented by balanced chemical Rate oc [ Conc. of reactant ]n 2H1 H2 +12 Rate a [HI]


  9. Law of Chemical Equilibrium forward A + B CD Backward The rate of forward ward reaction [A] [B ]


  10. Law of Chemical Equilibrium forward A + B CD Backward The rate of forward ward reaction [A] [B ] The rate of forward reaction Kf [A] [B] = = constant for forward reaction


  11. Law of Chemical Equilibrium forward A + B CD Backward The rate of forward ward reaction [A] [B ] (1) The rate of forward reactionKf[A] [B] Kr = constant for forward reaction The rate of back ward reaction [ C] [D ] ine (1) back ward react on [C] [D] Kp constant for back ward reaction at R


  12. equilibrium Rate of fwd. reaction Rate of bwd reaction Kf [CJID] Kb [A][B] Equilibrium constant Kc Kf Kb Put the value of Kf / Kb in eqn (3) ICJTD] Kc IA 1IB]


  13. [C]eIDld Kc [A][B]b EQUILIBRIUM CONSTANT may be defined as: The ratio of molar concentration of product and reactant each raised to the power equal to its coefficient at eqm LAW OF CHEMICAL EQUILIBRIUM: It states that - The ratio of molar concentration of product , each raised to the power equal to its coefficient, and molar concentration of reactant , each raised to the power equal to its coefficient, is constant at constant temperature at eqm Chemistry


  14. [C]c[D]d Kc [A] [B]b EQUILIBRIUM CONSTANT may be defined as: The ratio of molar concentration of product and reactant each raised to the power equal to its coefficient at eqm LAW OF CHEMICAL Equilibrium: It states that - The ratio of molar concentration of product, each raised to the power equal to its coefficient , and molar concentration of reactant , each raised to the power equal to its coefficient, is constant at constant temperature at eqm. EQUILIBRIUM CONSTANT is fixed for any reaction , & is affected by temperature. Its value is independent of Pressure , concentration & presence of other impurities.


  15. For gaseous reaction KD Partial pressure of Product ...at Equilibrium Partial pressure of Reactant Conc. of gases are expressed in term of partial pressure Pc Partial pressure of C Po Partial pressure of D PA Partial pressure of A


  16. Write the relation b/n K, & Kc for following CaCO3 (e) H2)2 HO 2(g) Kp Kc [RT]-112 2 H4o 2020)CO20)2H20 CsHo 15/2 02(9) 6160) 2) 3H2O


  17. Write the relation b/n K, & Kc for following 3 (9) Cao'sCO2 1 H2)20) CH4tg)+ 2029 CsHo 15/2 02(9) 2(g)H2O CO20)+2H2) 2(g)


  18. CHARACTERISTICS OF CHEMICAL EQM At equilibrium concentration of reactant and product become constant quilibrium dynamic in nature. Equilibrium can be established if none of the product or reactant is allow to escape Equilibrium can be obtained from either direction Iter or change the stat up the reaction For eqmG 0 and AH O


  19. CONCENTRATION QUOTIENT or REACTION QUOTIENT Q [concentration Product ....at any time Lconcen tration Reactant [C]c[D]d ....at any time [A] [B]b Chemistry