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प्रश्न
Explain with the help of a potential energy diagram that the catalyst increases the rate of the reaction.
उत्तर
- A catalyst provides alternative pathway associated with lower activation energy.
Potential energy barriers for catalyzed and uncatalyzed reactions - The potential energy diagram compares the potential energy barriers for the catalysed and uncatalysed reactions. The barrier for uncatalysed reaction (Ea) is larger than that for the same reaction in the presence of a catalyst Ea.
- Consider the decomposition of H2O2 in aqueous solution catalysed by I− ions \[\ce{2H2O_{2(l)} ->[I-] 2H2O_{(l)} + O_{2(g)}}\]
At room temperature, the rate of reaction is slower in the absence of catalyst with its activation energy being 76 kJ mol−1. In the presence of catalyst, iodide ion (I−), the reaction is faster since the activation energy decreases to 57 kJ mol−1.
संबंधित प्रश्न
Answer the following in one or two sentences.
What are the units for rate constants for zero-order and second-order reactions if time is expressed in seconds and concentration of reactants in mol/L?
Solve
The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
What is half life of first order reaction if time required to decrease concentration of reactants from 0.8 M to 0.2 M is 12 hours?
Derive an integrated rate law expression for first order reaction: A → B + C
Derive an expression for the relation between half-life and rate constant for first-order reaction.
For a first order reaction \[\ce{A ->Product}\] with initial concentration x mol L−1, has a half life period of 2.5 hours. For the same reaction with initial concentration `("x"/2)` mol L−1 the half life is
For a first-order reaction, the rate constant is 6.909 min−1 the time taken for 75% conversion in minutes is
If 75% of a first order reaction was completed in 60 minutes, 50% of the same reaction under the same conditions would be completed in ____________.
Write the rate law for the following reaction.
A reaction that is second order in NO and first order in Br2.
The integrated rate law is a direct relationship between ____________ and ____________.
The following reactions follow zero order kinetics, EXCEPT ____________.
The rate of the reaction \[\ce{A + B -> C}\] is 3.6 × 10−2 mol dm−3 s−1 when [A] = 0.3 mol dm−3 and [B] = 0.2 mol dm−3. Calculate k if reaction is first order in A and zero order in B.
Which among the following reaction is an example of a zero order reaction?
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ____________.
If time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 hours, the half life of this first order reaction is ____________.
Half-life period of a first order reaction, \[\ce{A -> product}\] is 3.0 hours. What is the value of rate constant?
A first order reaction is 75% completed in 60 minutes, the time required for it's 50% completion is ____________.
For a zero order reaction, the plot of [A]t vs t is linear. The slope of the line is equal to ____________.
The rate of formation of B at time t for reaction \[\ce{2A -> 3B}\] is equal to ____________.
Which among the following is an example of zero order reaction?
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
Half-life of first order reaction is 20 minutes. What is the time taken to reduce the initial concentration of the reactant to `1/10`th?
The integrated rate law is a direct relationship between time and ______
The rate constant and half-life of a first order reaction are related to each other as ______.
Calculate half-life of a first order reaction in minute if the rate constant is 1 × 10-3 s-1.
Which is the relation between half life and rate constant for a zero order?
The half-life period for the first order reaction is 1.7 hrs. How long will it take for 20% of the reactant to disappear?
