Advertisements
Advertisements
Question
Answer the following in brief.
For the reaction 2A + B → products, find the rate law from the following data.
| [A]/M | [B]/M | rate/M s-1 |
| 0.3 | 0.05 | 0.15 |
| 0.6 | 0.05 | 0.30 |
| 0.6 | 0.2 | 1.20 |
Advertisements
Solution
From above observations (i) and (ii)
0.15 = (0.3)x (0.05)y ......(i)
0.30 = (0.6)x (0.05)y .......(ii)
Dividing (2) by (1)
`0.30/0.15 = 2 = ((0.6)^x (0.05)^y)/((0.3)^x (0.05)^y) = ((0.6)/(0.3))^x = 2^x`
Hence, x = 1
From observation (i) and (iii) separately in the rate law gives
0.15 = (0.3)x (0.05)y ....(iii)
1.20 = (0.6)x (0.2)y .......(iv)
Dividing (4) by (3)
`1.20/0.15 = 0.6/0.3 (0.2/0.05)^y` (∵ x = 1)
∴ `8 = 2(0.2/0.05)^y = 2 xx 4^"y"`
∴ 4 = 4y
Therefore, y = 1
The rate law is rate = k [A][B].
APPEARS IN
RELATED QUESTIONS
What is the half life of a first order reaction if time required to decrease concentration of reactant from 0.8 M to 0.2 M is 12 h?
Choose the most correct option.
For an endothermic reaction, X ⇌ Y. If Ef is the activation energy of the forward reaction and Er that for the reverse reaction, which of the following is correct?
Answer the following in one or two sentences.
For the reaction,
\[\ce{CH3Br_{(aq)} + OH^-_{ (aq)} -> CH3OH^-_{ (aq)} + Br^-_{ (aq)}}\], rate law is rate = k`["CH"_3"Br"]["OH"^-]`
What is the change in rate if concentrations of both reactants are doubled?
A First order reaction is 50% complete in 69.3 minutes. Time required for 90% completion for the same reaction is _______.
The rate law relates to the rate of a chemical reaction in terms of _______.
For the reaction \[\ce{2NO_{(g)} + 2H_{2(g)} -> N_{2(g)} + 2H2O_{(g)}}\],
The rate law is, rate = k[NO]2 [H2].
What is the overall order of reaction?
Write four key points about order of reaction.
Define order of reaction with suitable examples.
In a first-order reaction A → B, 60% of a given sample of a compound decomposes in 45 mins. What is the half-life of reaction? Also, write the rate law equation for the above first-order reaction.
In a hypothetical reaction,
\[\ce{2A + B -> Products}\]. Rate = k [A]2 [B]
Molar concentration of 'B' is kept constant and molar concentration of 'A' is tripled, then the rate of reaction will ____________.
The rate constant of a first order reaction whose half-life is 480 seconds, is ____________.
For the non-stoichiometric reaction
\[\ce{2A + B -> C + D}\], the following kinetic data were obtained in three separate experiments, all at 298 K.
| Initial concentration (A) |
Initial concentration (B) |
Initial rate of formation of C (mol dm−3 s−1) |
| 0.1 M | 0.1 M | 1.2 × 10−3 |
| 0.1 M | 0.2 M | 1.2 × 10−3 |
| 0.2 M | 0.1 M | 2.4 × 10−3 |
The rate law for the formation of C is:
The rate law for a reaction between the substances A and B is given by, rate = k[A]n [B]m. On halving the concentration of A and doubling the concentration of B, the ratio of the new rate to the earlier rate of the reaction will be as ____________.
Select the rate law that corresponds to the data shown for the following reaction:
\[\ce{A + B -> C}\]
| Exp. | [A] mol dm−3 |
[B] mol dm−3 |
Initial Rate mol dm−3 |
| 1. | 0.012 | 0.035 | 0.10 |
| 2. | 0.024 | 0.070 | 0.80 |
| 3. | 0.024 | 0.035 | 0.10 |
| 4. | 0.012 | 0.070 | 0.80 |
The order of the reaction occurring by following mechanism should be:
(i) \[\ce{A2 + B2 -> AB2 + A (slow)}\]
(ii) \[\ce{A + B2 -> AB2 (fast)}\]
The rate law for the reaction \[\ce{2NO_{(g)} + O2_{(g)} -> 2NO2_{(g)}}\] is rate = k[NO]2 [O2] , then which among the following statement is correct?
In the reaction \[\ce{2SO_{2_{(g)}} O_{2_{(g)}} -> 2SO_{3_{(g)}}}\], the rate of disappearance of SO2 is 1.28 × 10-5 M/s. What is the rate of appearance of SO3?
For the reaction \[\ce{4NH3 + 5O2 -> 4NO + 6H2O}\], the rate of disappearance of NH3 is 3.6 × 10-3 M/s. What is the rate of formation of water?
Which of the following unit is used to express the rate of a reaction?
Which of the following statement is not true for a reaction having rate law r = k[H2][I2]?
The correct order of raaii of F, F-, O and O2- is ______.
For the reaction A + B → P.
If [B] is doubled at constant [A], the rate of reaction doubled. If [A] is triple and [B] is doubled, the rate of reaction increases by a factor of 6. Calculate the rate law equation.
