Chemical Kinetics Questions

For reaction A → B conc. is expressed as C = C₀e⁻ᵏᵗ calculate rate of reaction at t = 1/k sec. if C₀ = 10 mol/lit. & k = 500 sec⁻¹

A reaction follows the given concentration (C) vs time graph. The rate for this reaction at 20 seconds will be –

Rate law of reaction is R = k[A]¹ [B]¹/². Reaction can be a

For consecutive reaction k₁ << k₂ << k₃. order of reaction will be

Reaction A → B takes 10 mins for 10% completion, 20 mins for 20% completion, 30 mins for 30% completion & so on. Order of reaction will be -

Figure depicts the change in conc. of species x & y for reaction 2x → y, as a function of time the point of inter section of two curves represents

For Ist order reaction 2x(g) → 3y(g) + 2z(g) Assuming ideal nature of gas, time taken for 75% completion of reaction will be

What is the order of a chemical reaction A + 2B →C, if the rate of formation of 'C' increases by a factor of 2.82 on doubling the concentration of 'A' and increases by a factor of 9 on tripling the concentration of 'B'–

At a given temperature, the energy of activation of two reaction is same if

The rate constant is numerically the same for three reaction of 1st, 2nd & 3rd order respectively. For concentration < 1M, the correct order of rate of reaction is -

For the decomposition of N₂O₅ at a particular temperature, according to the equation : 2N₂O₅ → 4NO₂ + O₂ N₂O₅ → 2NO₂ + 1/2 O₂ the activation energy are E₁ & E₂ respectively, then

In the following reaction A →B + C, rate constant is 0.001 M/sec. If we start with 1M of A the conc. of A & B after 10 min are respectively

The reaction L → M is started with 10 gm of L. After 30 & 90 min. 5gm & 1.25 gm of L are left respectively. The order of reaction is

If for two reaction Ea₁ > Ea₂ & TC₁ & TC₂ are temperature coefficient respectively, then which of the following is correct -

In the following reaction : x A→yB where −ve sign indicates rate of disappearance of the reactant. Thus, x : y is –

A reaction takes place in various steps. The rate const. for 1st, 2nd, 3rd & 5th steps are k₁,k₂, k₃ & k₅ resp. The overall rate constant is given by . If activation energy are 40, 60, 50 & 10 kj/mole resp. The overall energy of activation (kJ/mole)

The instantaneous rate of disappearance of the MnO₄- ion in the following reaction is 4.56 × 10⁻³ Ms⁻¹. 2MnO₄- + 10 I- + 16H⁺ → 2Mn²⁺ + 5I₂ + 8H₂O The rate of appearance of I₂ is -

Select the correct diagram for an endothermic reaction that proceeds through two steps, with 2nd step as rate determining step (R.D.S.)

For the first order homogeneous gaseous A → 2B + C. The initial pressure was Pᵢ while total pressure of the time 't' was Pₜ. Then write expression for the rate constant k in terms of Pᵢ, Pₜ & t

Consider the plots given below, for the type of reaction nA ⟶ B + C These plots respectively corresponds to the reaction order

A gaseous reaction A₂(g) → B(g) + 1/2 C(g) shows increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of A₂ is-

At 100°C, the gaseous reaction A → 2B + C is found to be of first order. Starting with pure A, if at the end of 10 min, the total pressure of the system is 176 mm and the end of reaction, it is 270 mm, the partial pressure of A at the end of 10 min i

The progress of the reaction A ⇌ nB, with time is represented by the graph given below- The value of n is

For the reaction 2H₂ + 2NO → N₂ + 2H₂O the following mechanism has been proposed- (i) 2NO ⇌ N₂O₂ (fast) (ii) N₂O₂ + H₂ → N₂O + H₂O (r.d.s) (iii) N₂O + H₂ → N₂ + H₂O (fast) then what will be the rate law of this reaction?

For a second order reaction, the graph plotted between [A]⁻¹ and time 't' is shown below - θ = tan⁻¹ (0.5) and OP = 2L mol⁻¹. Thus rate of the reaction at start is –

For a reaction AB₅ → AB + 4B The rate can be expressed in following ways So the correct relation between K and K₁ is-

The rate of reaction at 273 K is R₀. The rate of reaction at 313 K will be (Assuming temperature coefficient equal to 2) –

A reaction rate constant is given by : . It means –

A substance ‘A’ decomposes in solution and follows the first order kinetics. Flask I contains 1M solution of A and flask II contains 0.6M solution. After 8hrs. the concentration of A in flask I becomes 0.25M, what will be the time for concentration o

A → product, follows second order kinetics. If the half life period of the reaction at [A]=0.2 mol lit⁻¹ is 20 minutes. The value of rate constant would be –

For the chemical reaction: A → products it is found that the rate of reaction increases by a factor of 6.25 when the concentration of A is increased by a factor of 2.5. The order of this reaction with respect to A is –

A reaction takes place in three steps. The rate constants are k₁, k₂ and k₃. The over all rate constant . If (energy of activation) E₁, E₂ and E₃ are 60, 30 and 10 kJ. The overall energy of activation is –

For the reaction A → B, data of initial concentration and corresponding half life period are given in the tabular form – [A] 1M 2M 4M T1/2 300s 600s 1200s The order of the reaction is –

t1/2 = constant, confirms the order of the reaction as one. a²t1/2 = constant confirms that the reaction is of –

For a hypothetical reaction A → B, the rate constant is 0.25 sec⁻¹. If the concentration of A is reduced to half then the value of rate constant is -

For a zero order reaction -

In the first order reaction, the concentration of the reactants is reduced to 25% in one hour. The half life period of the reaction is -

The temperature coefficient of most of the reactions lies between -

Which of the following represents the expression for 3/4 th life of first order reaction

The rate constant for a reaction is 10.8 x 10⁻⁵ mol lit⁻¹ sec⁻¹. The reaction is –

For the reaction A + B → C + D doubling the concentration of both the reactants increases the reaction rate 8 times and doubling the initial concentration of only B simply doubles the reaction rate. The rate law for the reaction is -

Find the rate constant for a first order reaction whose half life is 480 sec. –

The half life period of first order is t₁/₂. The half life period will –

For the reaction ; 2HI → H₂ + I₂, the expression . represents -

If the concentration is expressed in moles per litre the unit of the rate constant for a first order reaction is-

If the rate of reaction becomes 2 times for every 10°C rise in temperature, by what factor the rate of reaction increases when temperature is increased from 30°C to 80°C

Consider a gaseous reaction, the rate of which is given by k[A] [B]. The volume of the reaction vessel containing these gases is suddenly reduced to 1/4 th of the initial volume. The rate of the reaction as compared with original rate is -

Burning of coal is represented as C(s) + O₂ (g) → CO₂ (g). The rate of this reaction is increased by -

The rate of reaction increases by the increase of temperature because -

The rate of reaction between A and B increases by a factor of 100, when the concentration of A is increased by 10 times, the order of reaction with respect to A is -