Advertisements
Advertisements
Question
For the reaction 2NOBr → 2NO2 + Br2, the rate law is rate = k[NOBr]2. If the rate of a reaction is 6.5 × 10–6 mol L–1 s–1, when the concentration of NOBr is 2 × 10–3 mol L–1. What would be the rate constant of the reaction?
Advertisements
Solution
Given: Rate = k[NOBr]2 = 6.5 × 10–6 mol L–1 s–1
[NOBr] is 2 × 10–3 mol L–1
To find: Rate constant (k)
Calculation: rate = k[NOBr]2
k = `"rate"/["NOBr"]^2`
`= (6.5 xx 10^-6 "mol L"^-1"s"^-1)/((2 xx 10^-3 "mol L"^-1)^2)`
= 1.625 mol-1 L s–1
APPEARS IN
RELATED QUESTIONS
How will you represent first order reactions graphically.
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
Answer the following in brief.
Give one example and explain why it is pseudo-first-order.
For first order reaction, the rate constant for the decomposition of N2O5 is 6 × 10–4 s –1. The half-life period for decomposition in seconds is ______.
Give one example of a pseudo first-order reaction.
What is half life of first order reaction if time required to decrease concentration of reactants from 0.8 M to 0.2 M is 12 hours?
Explain pseudo first order reaction with a suitable example.
The decomposition of phosphine (PH3) on tungsten at low pressure is a first-order reaction. It is because the
Assertion: rate of reaction doubles when the concentration of the reactant is doubles if it is a first-order reaction.
Reason: rate constant also doubles.
Write the rate law for the following reaction.
A reaction that is `3/2` order in x and zero order in y.
From the following data, show that the decomposition of hydrogen peroxide is a reaction of the first order:
| t (min) | 0 | 10 | 20 |
| V (ml) | 46.1 | 29.8 | 19.3 |
Where t is the time in minutes and V is the volume of standard KMnO4 solution required for titrating the same volume of the reaction mixture.
A first order reaction has rate constant 1 × 10−2 s−1. What time will, it take for 20 g or reactant to reduce to 5 g?
The time of completion of 90% of a first order reaction is approximately ____________.
A first order reaction completes its 10% in 20 minutes, then the time required to complete its 19% is ____________.
If [A]0 is the initial concentration, then the half life of zero order reaction is ____________.
The activation energy of a reaction is zero. Its rate constant at 280 K is 1.6 × 10-6 s-1, the rate constant at 300 K is ______.
For the first order reaction, plot of log10 [A]t against time 't' is a straight line with a negative slope equal to ____________.
The order of the reaction for which the unit of rate constant is s−1 is ____________.
For a zero order reaction, the plot of [A]t vs t is linear. The slope of the line is equal to ____________.
The half-life of a first order reaction is 6.0 hour. How long will it take for the concentration of reactant to decrease from 0.4 M to 0.12 M?
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
Which is the unit of rate constant for the first-order reaction if time is expressed in seconds?
Rate constant for zero order reaction is 2 × 10-2 mol L-1 s-1. If the concentration of the reactant after 25 sec. is 0.5 M, what is the initial concentration of reactant?
Obtain the expression for half-life and rate constant of the first-order reaction.
If the rate constant for a first-order reaction is k, the time (t) required for the completion of 99% of the reaction is given by:
What are integrated rate laws?
The half-life period for the first order reaction is 1.7 hrs. How long will it take for 20% of the reactant to disappear?
