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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
Answer the following in one or two sentences.
What is the relationship between coefficients of reactants in a balanced equation for an overall reaction and exponents in the rate law? In what case the coefficients are the exponents?
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.
For the elementary reaction
\[\ce{2SO2(g) + O2(g) -> 2SO3(g)}\], identify the correct 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.
A chemical species that is formed in one elementary step in the mechanism of complex reaction and consumed in the subsequent step is called ____________.
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 ______
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.
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.
