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प्रश्न
Write an expression for instantaneous rate of reaction:
2N2O(g) → 4NO2(g) + O2(g).
What is the order of reaction?
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उत्तर
- Expression for instantaneous rate of reaction:
Rate of reaction = `- 1/2 ("d"["N"_2"O"])/"dt" = 1/4 ("d"["NO"_2])/("dt") = ("d"["O"_2])/"dt"` - The given reaction is of first order.
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संबंधित प्रश्न
Distinguish between Order and Molecularity of reaction.
Answer the following in one or two sentences.
What is the rate-determining step?
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?
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:
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.
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:
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.
