Advertisements
Advertisements
प्रश्न
Answer the following in one or two sentences.
What is the rate-determining step?
What do you understand by rate determining step?
Advertisements
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.
APPEARS IN
संबंधित प्रश्न
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.
Write an expression for instantaneous rate of reaction:
2N2O(g) → 4NO2(g) + O2(g).
What is the order of reaction?
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.
For the elementary reaction
\[\ce{2SO2(g) + O2(g) -> 2SO3(g)}\], identify the correct among the following relations.
The rate determining step of a reaction is the step ____________.
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.
A reaction involving two different reactants can never be a ______
Identify the molecularity of following elementary reaction:
NO(g) + O3(g) → NO3(g) + O(g)
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.
A certain reaction occurs in two steps as
(i) \[\ce{2SO2(g) + 2NO2(g) -> 2SO3(g) + 2NO(g)}\]
(ii) \[\ce{2NO(g) + O2(g) -> 2NO2(g)}\]
In the reaction:
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.
