List of top Chemistry Questions on Order of 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 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)
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)
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)
The order of reaction for which the units of rate constant are mol dm$^{-3}$ s$^{-1}$ is
The rate law equation for a reaction between A, B and C is $r = k [A] [B] [C]^2$, what will be the rate of reaction if concentration of both A and B are doubled?
Which of the following represents integrated rate law equation for gas phase first order reaction, $\text{A}_{(\text{g})} \rightarrow \text{B}_{(\text{g})} + \text{C}_{(\text{g})}$ if $P_i =$ initial pressure of A and $P =$ total pressure of reaction mixture at time $t$?
Which of the following equations represents integrated rate law for zero order reaction?
A reaction is first order with respective to $\mathrm{A}$ and second order with respective to $\mathrm{B}$. What is the effect on reaction rate if concentration of $\mathrm{B}$ is increased 3 times?
If decomposition of hydrogen peroxide is a first order reaction, it's rate law equation can be represented as
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
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
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
For the reaction $H _{2}( g )+ Br _{2}( g ) \rightarrow 2 HBr ( g )$, the experiment data suggested that $r = k \left[ H _{2}\right]\left[ Br _{2}\right]^{1 / 2} .$ The molecularity and order of the reaction are respectively:
For a first order reaction $A \to P,$ the temperature (T) dependent rate constant (k) was found to followthe equation log k=- (2000) $\frac{1}{T}+6.0.$ The pre-exponential factor A and the activation energy $E_{a,}$ respectively, are
For the reaction $2SO_2 + O_2$ (excess) $\rightarrow\, 2SO_3$ the order of reaction with respect to $O_2$ is
The conversion of $A \rightarrow B$ follows second order kinetics. If $[A]$ is increased 3 times then rate of formation of $[B]$ is
Which of the following equation exhibits integrated rate law equation for first order reaction?
The order of basicity of amines in gaseous state is:
The order of basicity of the compounds is
The half life of a radioactive nucleus is $50$ days. The time interval (t$_2-t_1$) between the time t$_2$ when $\frac{2}{3}$ ot it has decayed and the time $t_1$, when $\frac{1}{3}$ of it had decayed is
The unit of rate constant for a zero order reaction is -