The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
Experiment A/ mol L-1 B/ mol L-1 Initial rate/mol L-1 min-1 I 0.1 0.1 2.0x10-2 II - 0.2 4.0x10-2 III 0.4 0.4 - IV - 0.2 2.0x10-2
The reaction between A and B is first order with respect to A and zero order with respect to B. Fill in the blanks in the following table:
| Experiment | A/ mol L-1 | B/ mol L-1 | Initial rate/mol L-1 min-1 |
| I | 0.1 | 0.1 | 2.0x10-2 |
| II | - | 0.2 | 4.0x10-2 |
| III | 0.4 | 0.4 | - |
| IV | - | 0.2 | 2.0x10-2 |
Solution and Explanation
The given reaction is of the first order with respect to A and of zero order with respect to B.
Therefore, the rate of the reaction is given by,
Rate = k [A]1[B]0
⇒ Rate = k[A]
From experiment I, we obtain
2.0 x 10-2 mol L-1min-1= k (0.1 mol L-1)
⇒ k= 0.2 min-1
From experiment II, we obtain
4.0 x 10-2 mol L-1min-1= 0.2 min-1[A]
⇒ [A] = 0.2 mol L-1
From experiment III, we obtain
Rate = 0.2 min-1 x 0.4 mol L-1
= 0.08 mol L-1 min-1
From experiment IV, we obtain
2.0 x 10-2 mol L-1 min-1= 0.2 min-1 [A]
⇒ [A] = 0.1 mol L-1
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Concepts Used:
Order of Reaction
The Order of reaction refers to the relationship between the rate of a chemical reaction and the concentration of the species taking part in it. In order to obtain the reaction order, the rate equation of the reaction will given in the question.
Characteristics of the reaction order
- Reaction order represents the number of species whose concentration directly affects the rate of reaction.
- It can be obtained by adding all the exponents of the concentration terms in the rate expression.
- The order of reaction does not depend on the stoichiometric coefficients corresponding to each species in the balanced reaction.
- The reaction order of a chemical reaction is always defined with the help of reactant concentrations and not with product concentrations.
- Integer or a fraction form the value of the order of reaction will be there and it can be zero.