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प्रश्न
The rate law relates to the rate of a chemical reaction in terms of _______.
विकल्प
concentration of catalyst
temperature
potential energy
mol/L of reactants
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उत्तर
The rate law relates to the rate of a chemical reaction in terms of mol/L of reactants.
संबंधित प्रश्न
Choose the most correct option.
The order of the reaction for which the units of the rate constant are mol dm-3 s-1 is _______.
The time required for 90% completion of a certain first-order reaction is t. The time required for 99.9% completion will be _________.
Choose the most correct option.
The reaction, \[\ce{3ClO- -> ClO^-3 + 2Cl-}\] occurs in two steps,
(i) \[\ce{2ClO- -> ClO^-2}\]
(ii) \[\ce{ClO^-2 + ClO- -> ClO^-_3 + Cl-}\]
The reaction intermediate 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 _______.
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.
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 reaction, \[\ce{N2(g) + 3H2(g) -> 2NH3(g); \Delta H}\] is equal to ______.
For a chemical reaction rate law is, rate = k[A]2[B]. If [A] is doubled at constant [B], the rate of reaction ______.
The rate law for the reaction \[\ce{A + B + C -> Product}\] is expressed as Rate = k[A]2 [B]1 [C]0. What is the overall order of the reaction?
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 ____________.
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, \[\ce{N2 + 3H2 -> 2NH3}\], the rate of disappearance of H2 is 0.02 Mis. The rate of appearance of NH3 is ______.
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?
Write the rate law for the following reaction:
A reaction that is zero order in A and second order in B.
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.
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?
`t_(1/4)` can be taken as the time taken for the concentration of a reactant to drop to `3/4` of its initial value. If the rate constant for a first order reaction is k, the `t_(1/4)` can be written as ______.
