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Class 9Class 10First YearSecond Year
$EXAMPLE 3. In a reaction A+B=2 C when equilibrium was attained the concentration was [A]=[B]=4 moles / \mathrm{dm}^{3}[C]=6 \mathrm{moles} / \mathrm{dm}^{3} . Calculate the equilibrium constant K_{c} and the initial concentrations of A and B .$

Q14 In the equilibrium$\mathrm{PCl}_{5}(\mathrm{~g}) \square \mathrm{PCl}_{3}(\mathrm{~g})+\mathrm{Cl}_{2}(\mathrm{~g}) \Delta \mathrm{H}=+90 \mathrm{~kJ} \mathrm{~mol}^{-1}$What is the effect on(a) the position of equilibrium(b) equilibrium constant? ifi) temperature is increased

$(c) Write equilibrium constant expression for the following reactions(ii) \mathrm{Ag}^{+} (aq) +\mathrm{Fe}^{2+} (aq) \square \mathrm{Fe}^{3+} (aq) +\mathrm{Ag}(\mathrm{s})$

1. For the decomposition of dinitrogen oxide \left(\mathrm{N}_{2} \mathrm{O}\right) into nitrogen and oxygen reversible reaction takes place as follows$2 \mathrm{~N}_{2} \mathrm{O}_{(\mathrm{g})} \rightleftharpoons 2 \mathrm{~N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}$The concentration of \mathrm{N}_{2} \mathrm{O} \mathrm{N}_{2} and \mathrm{O}_{2} are 1.1 \mathrm{~mol} \mathrm{dm}^{-3} 3.90 \mathrm{~mol} \mathrm{dm}^{-3} and 1.95 \mathrm{~mol} \mathrm{dm}^{-3} respectively at equilibrium. Find out \mathrm{K}_{\mathrm{c}} for this reaction.

$11. Write note on :(ii) dynamic equilibrium$

$13. If reaction quotient Q_{c} of a reaction is more than K_{c} what will be the direction of the reaction?$

Q15. Synthesis of ammonia by Habers process is an exothermic reaction.$\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \square 2 \mathrm{NH}_{3}(\mathrm{~g}) \ddot{A} H=-92.46 \mathrm{~kJ}$(d) What happens to equilibrium position of this reaction if \mathrm{NH}_{3} is removed from the reaction vessel from time to time?