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प्रश्न
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?
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.
उत्तर
- Overall reaction: \[\ce{2NO_{(g)} + Cl_{2(g)} -> 2NOCl_{(g)}}\]
- Since NOCl2 is formed in the first step and consumed in the second step, it is the reaction intermediate.
- The molecularity of each step is 2 because two reactants are involved in each of the steps.
Notes
Students should refer to the answer according to their questions.
संबंधित प्रश्न
Distinguish between Order and Molecularity of reaction.
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?
Answer the following in one or two sentences.
What is the rate-determining step?
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.
Write an expression for instantaneous rate of reaction:
2N2O(g) → 4NO2(g) + O2(g).
What is the order of reaction?
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?
For the elementary reaction
\[\ce{2SO2(g) + O2(g) -> 2SO3(g)}\], identify the correct among the following relations.
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.
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.
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?
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.
