Consider a reaction A + B + C. If the initial concentration of A was reduced from 4M to 2M in 1 hour and from 2M to 1M in 0.5 hours, the order of the reaction is

A gaseous reaction A₂(g) → B(g) + $\frac{1}{2}C$(g) shows increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of A₂ will be : 

During the formation of ammonia by Haber's process N₂+3H₂ → 2NH₃, the rate of appearance of NH₃ was measured as 2.5 x 10^-4 mol L^-1 s^-1.The rate of disappearance of H₂ will be : 

For a chemical reaction, A $\to$  products, the rate of reaction doubles when the concentration of A is increased by 4 times. The order of the reaction is 

The correct expression for $\frac{3}{4}$ th life of a first order reaction is:

$$\begin{gathered} 1. \frac{\mathrm{k}}{2.303}\log \frac{4}{3} \\ 2. \frac{2.303}{\mathrm{k}}\log \frac{3}{4} \\ 3. \frac{2.303}{\mathrm{k}}\log 4 \\ 4. \frac{2.303}{\mathrm{k}} \log 3 \end{gathered}$$

The plot of log k vs 1/T helps to calculate :

For an endothermic reaction, where ΔH represents the enthalpy of the reaction in kJ/mol, the minimum value for the energy of activation will be

In the formation or sulphur trioxide by the contact process,

2SO₂(g) + O₂(g) $\to$2SO₃(g)

The rate of reaction is expressed as $\frac{\mathrm{d}\left[{\mathrm{O}}_2\right]}{\mathrm{dt}}$= 2.5x10^-4 mol L^-1sec^-1. The rate disappearance of SO₂ will be

A first order reaction complete 40% in 20 minutes. In how much time it is completed 90% of its original amount?

The dissociation of H₂O₂ is a first order reaction. The half life for '16 V H₂O₂ is 30 min, calculate the time at which the solution is 1V H₂O₂ ?

If the activation energy is 65 kJ then the reaction at 25°C is .......times fast as compared to 0°C :-

When temperature is increased from 27$°$C to 127$°$C, rate of reaction becomes doubled, then E_a will be?

For a certain reaction, 10% of the reactant dissociates in 1 hour, 20% of the reactant dissociates in 2 hours, 30% of the reactant dissociates in 3 hours. Then the units of the rate constant is:-

For a first order reaction A $\to$ product :

Two reactions of the same order have equal Pre-exponential factors but their activation energies differ by 24.9 kJ/mol. Calculate the ratio between the rate constants (K₁/K₂) these reactions at 27°C :

The activation energy of a reaction is zero. The rate constant of the reaction is :

The rate constant of a first order reaction is 10^-3 min^-1 at 27°C. The temperature coefficient of this  reaction is 2. The rate constant at 17°C will be :

 For the pseudo first order reaction A + B $\to$ P, when studied with 0.1 M of B is given by -d[A]/dt =k[A] where K = 1.85 x 10⁴ sec^-1. Calculate the value of rate constant for second order reaction :

Time required to decompose half of the substance for (n)th order reaction is propotional to:-

What is the activation energy for reverse reaction on the basis of given data ?

N₂O₄(g) $\to$ 2NO₂(g)  ΔH = +54kJ

E_a(forward) = +57.2 kJ

For a first-order reaction, the time required for 99.9% of the reaction to take place is nearly :

The rate constant for a chemical reaction that takes place at 500 K, is expressed as K = A e^-1000. The activation energy of the reaction is-

The concentration of reactant X decreases from 0.1 M to 0.005 M in 40 minutes. If the reaction follows first order kinetics, the rate of reaction when concentration of X is 0.01 M will be

The half-life period of a first-order reaction is 10 min. The time required for the concentration of the reactant to change from 0.08 M to 0.02 M is:

Mechanism of a hypothetical reaction

${\mathrm{X}}_2 + {\mathrm{Y}}_2 \stackrel{ }{\to } 2\mathrm{XY}$ is given below

(i) ${\mathrm{X}}_2 \stackrel{ }{\rightleftharpoons } \mathrm{X} + \mathrm{X} \left(\mathrm{fast}\right)$

(ii) $\mathrm{X} + {\mathrm{Y}}_2 \stackrel{ }{\to } \mathrm{XY} + \mathrm{Y} \left(\mathrm{slowest}\right)$

(iii) $\mathrm{X} + \mathrm{Y} \stackrel{ }{\to }\mathrm{XY} \left(\mathrm{fast}\right)$

The overall order of the reaction will be

A first order reaction has a specific reaction rate of 10^-2s^-1. How much time will it take for 20 g of the reactant to reduce to 5 g?

(a) 238.6 s      (b) 138.6 s        (c) 346.5  s        (d) 693.0 s

The decomposition of phosphine (PH₃) on tungsten at low pressure is a first-order reaction. It is because the

The rate of a first-order reaction is 0.04 mol L^-1 s^-1 at 10 sec and 0.03 mol L^-1 s^-1 at 20 sec after initiation of the reaction. The half-life period of the reaction is

The activation energy of a reaction can be determined from the slope of the graph between : 

If the half-life is independent of it's initial concentration then order of reaction is: