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What will be the effect of addition of a catalyst at constant temperature?
  • a)
    The equilibrium constant will remain constant.
  • b)
    ΔH of the reaction will remain constant.
  • c)
    Kf and Kb will increase upto the same extent.
  • d)
    Equilibrium composition will change.
Correct answer is option 'A,B,C'. Can you explain this answer?
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Most Upvoted Answer
What will be the effect of addition of a catalyst at constant tempera...
, Kf and Kb are affected equally and Keq is not affected by the presence of a catalyst.
ΔHreaction remains constant. There is no effect of catalyst since,
Both will change up to the same extent.
Community Answer
What will be the effect of addition of a catalyst at constant tempera...

Effect of Addition of a Catalyst at Constant Temperature:

The addition of a catalyst at constant temperature has several effects on a chemical reaction:

Equilibrium Constant Will Remain Constant:
- The presence of a catalyst does not affect the position of equilibrium in a reversible reaction.
- Therefore, the equilibrium constant (Kc) will remain constant even after the addition of a catalyst.

ΔH of the Reaction Will Remain Constant:
- The enthalpy change (ΔH) of a reaction is not altered by the presence of a catalyst.
- The catalyst provides an alternative pathway for the reaction to proceed, but it does not change the overall energy change of the reaction.

Kf and Kb Will Increase up to the Same Extent:
- The rate of both forward (Kf) and reverse (Kb) reactions will increase upon addition of a catalyst.
- The catalyst lowers the activation energy barrier for both the forward and reverse reactions, leading to an increase in reaction rates.

Equilibrium Composition Will Change:
- Although the position of equilibrium is not affected by the catalyst, the rates of the forward and reverse reactions will change.
- This adjustment in reaction rates may result in a temporary shift in the equilibrium composition until a new equilibrium is established.

In conclusion, the addition of a catalyst at constant temperature does not alter the equilibrium constant, enthalpy change, or overall equilibrium position of a reaction. Instead, it enhances the rates of both forward and reverse reactions, ultimately leading to a new equilibrium composition.
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There are many reactions which obey a first order rate equation although it reality they are bi- or ter-molecular. As an example of these may be taken the decomposition of Carbonyl sulfide in water, namely, COS + H20 002 + H2SAccording to the law of mass action this reaction should be second order with the rate dependent on the concentration of both the carbonyl sulfide and the water. Actually however, the rate is found to be first order with respect to the carbonyl sulfide and independent of the water Reactions exhibiting such behaviour are said to be pseudo-molecular.The pseudo-unimoecuar nature of this reaction is explainable by the fact that water is present in such excess that its concentration remains practically constant during the course of the reaction. Under these condition b x = b, and the rate equation becomesOn integration this leads towhich is the equation for a first order reaction. It is evident, however, that the now constant k is not independent of the concentration, as is the case with true first order constants, but may vary with b if the latter is changed appreciably, When such is the case, the true constant k2 can be obtained from k by dividing the latter by b. pseudo-molecular reactions are encountered whenever one or more of the reactants remain constants during the course of an experiment. This is the case with reactions conducted in solvents which are themselves one of the reactants, as in the decomposition of carbonyl sulfide in water, or in the esterification of acetic anhydride in alcohol(CH3C0)20 + 2C2H5OH 2CH3C00C2H5 + H20Again, this is also true of reactions subject to catalysis, in which case the concentration of the catalyst does not change. The decomposition of diacetone alcohol to acetone in aqueous solution is catalysed by hydroxyl ions, with the rate proportional to the concentration of the alcohol and that of the base. Since the concentration of the base does not change within any one experiment, however, the rate equation reduces to one of first order with respect to the alcohol. But the rateconstant k obtained for various concentrations of base are not identical, as may be seen from table. To obtain from these the true second order velocity constant, the ks must be divided by the hydroxyl ion concentration. When this is done excellent k2 values result, as column 3 indicatesTable : Decomposition of diacetone alcohol in water at 25C (Catalyst : NaOH)Q.By what factor does the rate of reaction of diacetone alcohol in water solution change if p0H is increased by 2 units other things remaining same ?

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What will be the effect of addition of a catalyst at constant temperature?a)The equilibrium constant will remain constant.b)ΔH of the reaction will remain constant.c)Kf and Kb will increase upto the same extent.d)Equilibrium composition will change.Correct answer is option 'A,B,C'. Can you explain this answer?
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