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
Answer the following in brief.
What is a zeroth-order reaction?
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.
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?
The rate constant of a reaction is 5.8 × 10−2 s−1. The order of the reaction is ____________.
If 75% of a first order reaction was completed in 60 minutes, 50% of the same reaction under the same conditions would be completed in ____________.
Write the rate law for the following reaction.
A reaction that is second order in NO and first order in Br2.
Give two examples for zero order reaction.
A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?
What is the value of rate constant of first order reaction, if it takes 15 minutes for consumption of 20% of reactants?
How long would it take to electroplate a spoon with 0.1 mol of silver (108 g/mol) at a constant current of 2.0 A using AgNO3?
A first order reaction is 25% completed in 40 minutes. What is the rate constant k tor the reaction?
A reaction that is of the first order with respect to reactant A has a rate constant 6 min−1. If we start with [A]0 = 0.5 mol dm−3, when would [A] reach the value 0.05 mol dm−3?
What is the order of reaction if the unit of rate constant (k) is mol dm−3 s−1?
The integrated rate equation for first-order reaction, A → product, is ______.
For first order reaction the slope of the graph of log10 [A]t Vs. time is equal to ____________.
A first order reaction is 75% completed in 60 minutes, the time required for it's 50% completion is ____________.
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N2(g) is 2.6 × 10−4 M/s, the rate of disappearance of H2(g) in M/s is ____________.
A first order reaction is 50% completed in 16 minutes. The percentage of reactant that will react in 32 minutes is ____________.
The time required to decompose SO2Cl2 to half of it's initial amount is 60 minutes. Calculate rate constant for this first order reaction.
Half-life of first-order reaction \[\ce{X -> Y + Z}\] is 3 minutes. What is the time required to reduce the concentration of 'X' by 90 % of it's initial concentration?
The integrated rate equation is Rt = log C0 – log Ct, then the straight-line graph is obtained by plotting.
The expression to calculate time required for completion of zero order reaction is ______.
The integrated rate law is a direct relationship between time and ______
Which one of the following reactions is a true first-order reaction?
Half-life of a first order reaction is 30 minutes and initial concentration of reactant is 0.1 M.
What is half-life of the reaction if initial concentration of reactant is doubled?
Which of the following correctly represents integrated rate law equation for a first order reaction in a gas phase?
