List of top Chemistry Questions on Order of Reaction

For a first-order reaction, the slope of the graph between \(\log[A]\) vs time is equal to:
A reaction is of second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is (i) doubled, (ii) reduced to half?
For a first-order reaction, the concentration of a reactant decreases from 0.8 M to 0.4 M in 20 minutes. What is the half-life of the reaction? (Use $\ln 2 = 0.693$)

The following data were obtained for the reaction: \[ 2NO(g) + O_2(g) \rightarrow 2N_2O(g) \] at different concentrations: 

 The rate law of this reaction is:

Which of the following plots gives a straight line for a zero-order reaction?
For a first-order reaction, the ratio of time required is $ \frac{t_1}{t_2} $, if $ t_1 $ is the time consumed when reactant reaches $ \frac{1}{4} $ of initial concentration and $ t_2 $ is the time when it reaches $ \frac{1}{8} $ of initial concentration.

For a first-order reaction, the concentration of reactant was reduced from 0.03 mol L\(^{-1}\) to 0.02 mol L\(^{-1}\) in 25 min. What is its rate (in mol L\(^{-1}\) s\(^{-1}\))? 

Consider the following reaction
\[A + B \rightarrow C\]
The time taken for A to become 1/4th of its initial concentration is twice the time taken to become 1/2 of the same. Also, when the change of concentration of B is plotted against time, the resulting graph gives a straight line with a negative slope and a positive intercept on the concentration axis.
The overall order of the reaction is ____.
Consider the two different first-order reactions given below: \[\text{A + B} \rightarrow \text{C (Reaction 1)} \\\text{P} \rightarrow \text{Q (Reaction 2)}\]The ratio of the half-life of Reaction 1 : Reaction 2 is $5 : 2$. If $t_1$ and $t_2$ represent the time taken to complete $\frac{2}{3}^\text{rd}$ and $\frac{4}{5}^\text{th}$ of Reaction 1 and Reaction 2, respectively, then the value of the ratio $t_1 : t_2$ is ____ $\times 10^{-1}$ (nearest integer).[Given: $\log_{10}(3) = 0.477$ and $\log_{10}(5) = 0.699$]
The rate constant of a reaction is $ K = 3.28 \times 10^{-4} \, \text{s}^{-1} $. Find the order of the reaction.
At 300 K, the half-life period of a gaseous reaction at an initial pressure of 40 kPa is 350 s. When pressure is 20 kPa, the half-life period is 175 s. What is the order of the reaction?
The correct order of the number of unpaired electrons in the given complexes is
A. \([Fe(CN)_6]^{3–}\)
B. \([FeF_6]^{3–}\)
C. \([CoF_6]^{3–}\)
D. \([Cr(oxalate)_3]^{3–}\)
E. \([Ni(CO)_4]\)
Choose the correct answer from the options given below:
The correct order of reactivity of following haloarenes towards nucleophilic substitution with aqueous NaOH is 
order of reactivity of following haloarenes
Choose the correct answer from the options given below:
A molecule undergoes two independent first order reactions whose respective half lives are 12 min and 3 min. If both the reactions are occurring then the time taken for the 50% consumption of the reactant is _____ min. (Nearest integer)
The bond dissociation energy is highest for
The magnetic behavior of Li2O, Na2O2 and KO2, respectively, are
For a first order reaction, the time required for completion of 90% reaction is ‘x’ times the half life of the reaction. The value of ‘x’ is (Given: In 10 = 2.303 and log 2 = 0.3010)
The reaction between X and Y is first order with respect to X and zero order with respect to Y.
reaction between X and Y is first order with respect to X and zero order with respect to Y.
Examine the data of table and calculate ratio of numerical values of M and L. (Nearest integer)
40% of HI undergoes decomposition to H2 and I2 at 300 K. ΔG° for this decomposition reaction at one atmosphere pressure is _____ J mol–1. [nearest integer]
(Use R = 8.31 J K–1 mol–1; log 2 = 0.3010, ln 10 = 2.3, log 3 = 0.477)
For a first order reaction \(A → B\), the rate constant, \(k = 5.5×10^{–14}s^{–1}\). The time required for 67% completion of reaction is \(x×10^{–1}\) times the half life of reaction. The value of \(x\) is _____. (Nearest integer)
Choose the correct set of reactions which follow first order kinetics:
(i) Thermal decomposition of HI on gold surface.
(ii) Thermal decomposition of $N_2O_5(g)$ at constant volume.
(iii) Hydrogenation of ethene.
(iv) Decomposition of $NH_3$ on a hot Pt surface.
(v) Thermal decomposition of $SO_2Cl_2(g)$ at constant volume.
The following graph shows how $(t_{1/2})$ a (half life) of a reactant R changes with the initial reactant concentration $a_0$. The order of the reaction will be
The ratio of the half-life time $ (t_{1/2}) $ , to the three quarter life-time, $ (t_{3/4}) $ , for a reaction that is second order
When initial concentration of the reactant is doubled, the half-life period of a zero order reaction
The correct difference between first- and second-order reactions is that