Advertisements
Advertisements
Question
Choose the most correct option.
The rate constant for the reaction \[\ce{2N2O5_{(g)} -> 2N2O4_{(g)} + O2_{(g)}}\] is `4.98 xx 10^-4 "s"^-1`. The order of reaction is _____________.
Options
2
1
0
3
Advertisements
Solution
The rate constant for the reaction \[\ce{2N2O5_{(g)} -> 2N2O4_{(g)} + O2_{(g)}}\] is `4.98 xx 10^-4 "s"^-1`. The order of reaction is 1.
APPEARS IN
RELATED QUESTIONS
The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be _________.
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?
The elementary reaction \[\ce{O3_{(g)} + O_{(g)} -> 2O2_{(g)}}\] is ______.
Choose the most correct option.
Rate law for the reaction, \[\ce{2NO + Cl2 -> 2NOCl}\] is rate = k[NO2]2[Cl2]. Thus of k would increase with _____________.
Answer the following in one or two sentences.
For the reaction, \[\ce{CH3Br_{(aq)} + OH^{-}_{(aq)} -> CH3OH^{\ominus}_{(aq)} + Br^{\ominus}_{(aq)}}\], rate law is rate = \[\ce{k[CH3Br][OH^\ominus]}\]
How does reaction rate changes if \[\ce{[OH^\ominus]}\] is decreased by a factor of 5?
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 |
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 _______.
Order of reaction for which unit of rate constant is mol dm–3 s–1 is _______.
Write four key points about order of reaction.
For the reaction 2A + B → C, rate of disappearance of A 0.076 mol s –1.
- What is the rate of formation of C?
- What is the rate of consumption of B?
- What is the rate of the overall reaction?
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 ____________.
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:
For the reaction, \[\ce{N2(g) + 3H2(g) -> 2NH3(g); \Delta H}\] is equal to ______.
A gaseous hypothetical chemical equation \[\ce{2A ⇌ 4B + C}\] is carried out in a closed vessel. The concentration of B is found to increase by 5 × 10−3 mol dm−3 in 10 second. The rate of ____________.
The order of the reaction occurring by following mechanism should be:
(i) \[\ce{A2 + B2 -> AB2 + A (slow)}\]
(ii) \[\ce{A + B2 -> AB2 (fast)}\]
Consider the reaction \[\ce{2A + 2B -> C + 2D}\], if concentration of A is doubled at constant [B], rate increases by a factor 4. If concentration B is doubled at constant [A] the rate is doubled. Rate law of the reaction is ____________.
In the reaction, \[\ce{N2 + 3H2 -> 2NH3}\], the rate of disappearance of H2 is 0.02 Mis. The rate of appearance of NH3 is ______.
For the reaction \[\ce{2A + B -> 3C + D}\], which among the following is NOT the correct rate law expression?
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]?
Write the rate law for the following reaction:
A reaction that is zero order in A and second order in B.
Write the rate law for the following reaction:
A reaction that is second order in NO and first order in Br2.
The rate constant of a reaction ______.
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.
