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First Year Chemistry Chemical Equilibrium


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Q16Sulphuricacidisthekingofchemicals.ItisproducedbytheburningofSO2toSO3throughanexothermicreversibleprocess.(b)Whatistheeffectofpressurechangeonthisreaction?Q16 Sulphuric acid is the king of chemicals. It is produced by the burning of \mathrm{SO}_{2} to \mathrm{SO}_{3} through an exothermic reversible process.(b) What is the effect of pressure change on this reaction?
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
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

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})
(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})

(c)Writeequilibriumconstantexpressionforthefollowingreactions(ii)Ag+(aq)+Fe2+(aq)□Fe3+(aq)+Ag(s)(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.
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.

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
11. Write note on :(ii) dynamic equilibrium

11.Writenoteon:(ii)dynamicequilibrium11. 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?
13. If reaction quotient Q_{c} of a reaction is more than K_{c} what will be the direction of the reaction?

13.IfreactionquotientQcofareactionismorethanKcwhatwillbethedirectionofthereaction?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?
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?

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?

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