Advertisements
Advertisements
Question
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 _____________.
Options
increase in temperature
increase of concentration of NO
increase of concentration of Cl2
increase of concentrations of both Cl2 and NO
Advertisements
Solution
Rate law for the reaction, \[\ce{2NO + Cl2 -> 2NOCl}\] is rate = k[NO2]2[Cl2]. Thus of k would increase with increase in temperature.
APPEARS IN
RELATED QUESTIONS
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 _____________.
Choose the most correct option.
Slope of the graph ln[A]t versus t for first-order reaction is _________.
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 _______.
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?
Define order of reaction with suitable examples.
A reaction occurs in the following steps:
Step 1: \[\ce{NO_{2(g)} + F_2 -> NO2F_{(g)} + F_{(g)}}\] (slow)
Step 2: \[\ce{F_{(g)} + NO_{2(g)} -> NO_2F}\] (Fast)
- Write the equation of overall reaction.
- Write the rate law.
- Identify reaction intermediate.
For the reaction, \[\ce{N2(g) + 3H2(g) -> 2NH3(g); \Delta H}\] is equal to ______.
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 ____________.
For a chemical reaction rate law is, rate = k[A]2[B]. If [A] is doubled at constant [B], the rate of reaction ______.
For a hypothetical reaction \[\ce{A + B -> C}\], it is found that doubling the concentration of A increases the rate by 8 times and doubling the concentration of B increases the rate by 4 times. The overall order of the reaction is ____________.
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 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 \[\ce{A + B2 -> AB + B}\], the rate of reaction is directly proportional to the concentration of A and independent on the concentration of B2. What is the rate law expression?
The reaction \[\ce{A + B -> P}\], is second order in A and first order in B. What is the rate law for the reaction?
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 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 ______.
Write the rate law for the following reaction:
A reaction that is zero order in A and second order in B.
For a chemical reaction A → 7 products, the rate of reaction doubles when the concentration of A is increased by a factor 4. The order of the reaction is ______.
The rate constant for the reaction,
2N2O5(g) → 2N2O4(g) + O2(g) is 4.98 × 10-4 s-1.
What is the order of reaction?
