Chemical Kinetics

Decomposition of $\ce{H2O2}$ follows a first order reaction. In fifty minutes the concentration of $\ce{H2O2}$ decreases from 0.5 to 0.125 M in one such decomposition. When the concentration of $\ce{H2O2}$ reaches 0.05 M, the rate of formation of $\ce{O2}$ will be :

The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below :

$\ce{O3(g) + Cl^.(g) -> O2(g) + ClO^.(g)}$ ...... (i) $k_i=5.2\times10^9$ L mol$^{-1}$ s$^{-1}$

$\ce{ClO^.(g) + O^.(g) -> O2(g) + Cl^.(g)}$ ...... (ii) $k_{ii}=2.6\times10^{10}$ L mol$^{-1}$ s$^{-1}$

The closest rate constant for the overall reaction $\ce{O3(g) + O^.(g) -> 2O2(g)}$ is :

The rate law for the reaction below is given by the expression k [A][B]

A + B → Product

If the concentration of B is increased from 0.1 to 0.3 mole, keeping the value of A at 0.1 mole, the rate constant will be :

The %yield of ammonia as a function of time in the reaction
$$\ce{N2(g) + 3H2(g) <=> 2NH3(g)},\quad\Delta H<0$$
at $(P,T_1)$ is given below.

If this reaction is conducted at $(P,T_2)$, with $T_2>T_1$, the %yield of ammonia as a function of time is represented by

A closed vessel with rigid walls contains 1 mol of $^{238}_{92}\mathrm U$ and 1 mol of air at 298 K. Considering complete decay of $^{238}_{92}\mathrm U$ to $^{206}_{82}\mathrm{Pb}$, the ratio of the final pressure to the initial pressure of the system at 298 K is

In dilute aqueous $\ce{H2SO4}$, the complex diaquodioxalatoferrate(II) is oxidized by $\ce{MnO4-}$. For this reaction, the ratio of the rate of change of $[\ce{H+}]$ to the rate of change of $[\ce{MnO4-}]$ is

Higher order (>3) reactions are rare due to :

The reaction
$$\ce{2N2O5(g) -> 4NO2(g) + O2(g)}$$
follows first order kinetics. The pressure of a vessel containing only $\ce{N2O5}$ was found to increase from 50 mm Hg to 87.5 mm Hg in 30 min. The pressure exerted by the gases after 60 min. will be (Assume temperature remains constant) :

For the equilibrium, $\ce{A(g) <=> B(g)}$, ΔH is −40 kJ/mol. If the ratio of the activation energies of the forward ($E_f$) and reverse ($E_b$) reactions is $\dfrac23$ then :

$\ce{A + 2B -> C}$, the rate equation for this reaction is given as

Rate = k[A][B].

If the concentration of A is kept the same but that of B is doubled what will happen to the rate itself ?

For the elementary reaction $\ce{M -> N}$, the rate of disappearance of M increases by a factor of 8 upon doubling the concentration of M. The order of the reaction with respect to M is

For the non - stoichiometre reaction $\ce{2A + B -> C + D}$, the following kinetic data were obtained in three separate experiments, all at 298 K.

Initial Concentration (A)	Initial Concentration (B)	Initial rate of formation of C (mol L$^{-1}$ s$^{-1}$)
0.1 M	0.1 M	$1.2\times10^{-3}$
0.1 M	0.2 M	$1.2\times10^{-3}$
0.2 M	0.1 M	$2.4\times10^{-3}$

The rate law for the formation of C is :

The half-life period of a first order reaction is 15 minutes. The amount of substance left after one hour will be :

In the reaction of formation of sulphur trioxide by contact process $\ce{2SO2 + O2 <=> 2SO3}$ the rate of reaction was measured as $\dfrac{d[\ce{O2}]}{dt}=-2.5\times10^{-4}$ mol L$^{-1}$ s$^{-1}$. The rate of reaction in terms of $[\ce{SO2}]$ in mol L$^{-1}$s$^{-1}$ will be :

For the reaction, $\ce{2N2O5 -> 4NO2 + O2}$, the rate equation can be expressed in two ways $-\dfrac{d[\ce{N2O5}]}{dt}=k[\ce{N2O5}]$ and $+\dfrac{d[\ce{NO2}]}{dt}=k'[\ce{N2O5}]$

k and k′ are related as :

The rate coefficient (k) for a particular reactions is $1.3\times10^{-4}$ M$^{-1}$ s$^{-1}$ at 100°C, and $1.3\times10^{-3}$ M$^{-1}$ s$^{-1}$ at 150°C. What is the energy of activation ($E_A$) (in kJ) for this reaction ? (R = molar gas constant = 8.314 JK$^{-1}$ mol$^{-1}$)

For the reaction,
$$\ce{3A + 2B -> C + D},$$
the differential rate law can be written as :

In the reaction,
$$\ce{P + Q -> R + S}$$
the time taken for 75% reaction of P is twice the time taken for 50% reaction of P. The concentration of Q varies with reaction time as shown in the figure. The overall order of the reaction is

The initial rate of hydrolysis of methyl acetate (1 M) by a weak acid (HA, 1 M) is 1/100$^\text{th}$ of that of a strong acid (HX, 1 M), at 25 °C. The $K_a$ of HA is

In the nuclear transmutation
$$\ce{^9_4Be + X -> ^8_4Be + Y}$$
(X, Y) is(are)