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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.
Slope of the graph ln[A]t versus t for first-order reaction is _________.
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.
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 _______.
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 |
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?
Write four key points about order of reaction.
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.
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.
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) \[\ce{A + B2 -> AB2 (fast)}\]
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?
The reaction \[\ce{A + B -> P}\], is second order in A and first order in B. What is the rate law for the reaction?
What is the order of reaction for decomposition of gaseous acetaldehyde?
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?
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.
For the reaction 2A + B → A2B find the rate of decrease of [B].
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 ______.
