Chemical Kinetics Questions

The half life period for catalyst decomposition of AB₃ at 50 mm is found to be 4 hrs and at 100 mm it is 2.0 hrs. ? The order of reaction is -

A hypothetical reaction A₂ + B₂ → 2AB follows the mechanism as given below - A₂ ⇌ A + A (fast) A + B₂ → AB + B (slow) A + B → AB (fast) The order of the over all reaction is -

As the energy of activation increases –

The half life period for a certain first order reaction is 30 minutes. How long will it take for 1/32 of the reactant to be left behind -

The chemical reaction 2O₃ → 3O₂ proceeds as follows - O₃ ⇌ O₂ + O ............(fast) O + O₃ → 2O₂ ............(slow) The rate law expression should be -

For a zero order reaction, the plot of conc. (a – x) vs time is linear with -

The rate law for the reaction RCl + NaOH (aq.) → ROH + NaCl is given by, Rate = k₁ [RCl]. The rate of the reaction will be-

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

Collision theory is satisfactory for -

For a first order reaction A → products, the concentration of [A] is reduced from 1M to 0.125 M in one hour, the t₁/₂ of this reaction (in sec) is –

In a certain gaseous reaction between X and Y ; X + 3Y → XY₃ The initial rates are reported as follows – The rate law is -

A following mechanism has been proposed for a reaction - 2A + B → D + E A + B → C + D (slow) A + C → E (fast) The rate law expression for the reaction is -

In a first order reaction, 75% of the reactant disappeared in 1.386 hours. Calculate the rate constant of the reaction -

A 10° rise in temperature doubles the rate of reaction. This is because more molecules obtain–

The activation energy for the forward reaction X → Y is 60. KJ mol⁻¹ and ΔH is -20 KJ mol⁻¹, the activation energy for the reverse reaction is -

Consider the data given below for hypothetical reaction A → X. From the above data, the order of reaction is-

Select the rate law that corresponds to the data shown for the reaction A + B → C

For a certain decomposition, the rate is 0.30 M sec⁻¹ when the concentration of reactant is 0.20 M.If the reaction is second order, the rate (in M sec⁻¹) when concentration is increased 3-times is -

Among the following reactions, the fastest one is -

The activation energy of the reaction A + B → C + D + 38 k.cal is 20 k.cal, What would be the activation energy of the reaction, C + D → A + B

Which of the following explains the increase of reaction rate by catalyst -

The activation energy of reaction is equal to-

For a reaction in which the activation energies of forward and reverse reactions are equal -

The chemical reactions in which reactants require high amount of activation energy are generally -

Chemical reaction occurs as a result of collisions between reacting molecules. Therefore, the reaction rate is given by -

The activation energies of the forward and backward reactions in the case of a chemical reaction are 30.5 and 45.4 KJ/mol respectively. The reaction is –

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

The half-life period for a reaction at initial concentrations of 0.5 and 1.0 moles litre⁻¹ are 200 sec and 100 sec respectively. The order of the reaction is -

If a is the initial concentration of reactant, then the half life period of a reaction of nᵗʰ order is directly proportional to -

The t1/2 for the first order reaction, PCl₅(g) ⟶ PCl₃(g) + Cl₂(g) is 20 min. The time in which the conc. of PCl₅ reduces to 25% of the initial conc. is close to-

Radioactive decay follows -

A radioactive isotope decomposes according to the first order with half life period of 15 hrs. 80% of the sample will decompose in -

The rate constant for a second order reaction is 8.0 × 10⁻⁴ litre mol⁻¹ min⁻¹. How long will it take a 0.5M solution to be reduced to 0.25M –

For a second order reaction, if the conc. of a reactant decreases from 0.08M to 0.04M in ten minutes, what would be the time taken for the conc. to decrease to 0.01M –

In the presence of an acid, the initial concentration of cane sugar was reduced from 0.20 to 0.10 molar in 5 hours and from 0.2 to 0.05 molar in 10 hours. The reaction is of -

99% of a first order reaction was completed in 32 min. When will 99.9% of the reaction get completed -

For an elementary reaction X (g) → Y (g) + Z (g) the half life period is 10 min. In what period of time would the concentration of X be reduced to 10% of original concentration -

What is the half life of a radioactive substance if 75% of any given amount of the substance disintegrates in 60 minutes —

Wrong data for the first order reaction is —

Half life period of a zero order reaction is —

Which of following statement is false -

A first order reaction follows the expressions-

For a reaction, the rate constant is expressed as, k = A.e(-40000/T) The energy of the activation is -

The plot of log k vs.1/T yields a straight line. The slope of the line would be equal to -

Expression showing change of rate constant with temperature is —

If the first order reaction involves gaseous reactants and gaseous products the units of its rate are -

, this means that –

The rate of a certain reaction increase by 2.3 times when the temperature is raised from 300 K to 310K. If k is the rate constant at 300 K then the rate constant at 310 K will be equal to -

For a gaseous reaction the rate equation is v = k[A][B]. If the volume of each gaseous system is suddenly reduced to 1/3 of initial volume. The rate would become –

For a chemical reaction, 2A + 2B ⟶ C + D, the order of reaction is one with respect to A and one with respect to B. The initial rate of the reaction is 4 × 10⁻² mol L⁻¹ s⁻¹. When 50% of the reactants are converted into products, the rate of reaction