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प्रश्न
Answer the following in one or two sentences.
What is the rate-determining step?
What do you understand by rate determining step?
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उत्तर
When a chemical reaction occurs in a series of steps, one of the steps is slower than all other steps. Such a slow step in the reaction is called a rate-determining step.
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संबंधित प्रश्न
Distinguish between Order and Molecularity of reaction.
A reaction takes place in two steps:
- \[\ce{NO_{(g)} + Cl2_{(g)} -> NOCl2_{(g)}}\]
- \[\ce{NOCl2_{(g)} + NO_{(g)} -> 2NOCl_{(g)}}\]
- Write the overall reaction.
- Identify the reaction intermediate.
- What is the molecularity of each step?
Which of the following is a unimolecular reaction?
Identify molecularity of following reaction:
\[\ce{C2H5I_{(g)} -> C2H_{4(g)} + HI_{(g)}}\]
Name the slowest step that determines the rate in a complex reaction.
Define molecularity.
Why is molecularity applicable for only elementary reactions whereas order of a reaction is applicable for elementary and complex reactions? Explain with suitable examples.
For a zero-order reaction, molecularity can never be equal to zero. Explain.
Give one example of the reaction where order and molecularity are the same.
Mention any two factors that influence the rate of chemical reaction.
If for the reaction A → products, a straight line graph passing through origin is obtained between the rate of reaction against concentration of A, what would be the order of reaction? Why?
The rate determining step of a reaction is the step ____________.
For the elementary reaction, \[\ce{3H2_{(g)} + N2_{(g)} -> 2NH3_{(g)}}\] identify the correct relation among the following relations.
For the reaction \[\ce{2NO2 + F2 -> 2NO2F}\], following mechanism has been provided:
\[\ce{NO2 + F2 ->[slow] NO2F + F}\]
\[\ce{NO2 + F ->[fast] NO2F}\]
The rate expression of the above reaction can be written as:
The reaction \[\ce{2NO2Cl_{(g)} -> 2NO2_{(g)} + Cl2_{(g)}}\] takes place in two steps as
(i) \[\ce{NO2Cl_{(g)} -> NO2_{(g)} + Cl_{(g)}}\]
(ii) \[\ce{NO2Cl_{(g)} + Cl_{(g)} -> NO2_{(g)} + Cl2_{(g)}}\]
Identify the reaction intermediate.
Consider the following elementary reaction;
\[\ce{2AB_{(g)} -> A2_{(g)} + B2_{(g)}}\]
The molecularity of the reaction is ____________.
A reaction involving two different reactants can never be a ______
The reaction takes place in two steps as
(i) \[\ce{NO2Cl(g) ->[k1] NO2(g) + Cl(g)}\]
(ii) \[\ce{NO2Cl(g) + Cl(g) ->[k2] NO2(g) + Cl2(g)}\]
Identify the reaction intermediate.
What is an elementary reaction?
How does a catalyst differ from reaction intermediate?
A complex chemical reaction takes place in two steps.
Step I: NO(g) + O3(g) → NO3(g) + O(g)
Step II: NO3(g) + O(g) → NO2(g) + O2(g)
The predicted rate law is rate = k[NO][O3]
- Identify the rate determining step.
- Name the reaction intermediate/s. Why is/are it/these intermediate/s?
Define molecularity of reaction.
