NEET Chemistry Chemical Kinetics Class 12 Questions

The reaction, 2X → Y + Z would be zero order reaction when

According to Arrhenius equation rate constant k is equal to A e⁻ᴱᵃ/ᴿᵀ. Which of the following options represents the graph of ln k vs 1/T?

What will be the half-life of the first order reaction for which the value of rate constant is 200 s⁻¹?

Rate law for the reaction A + 2B ⟶ C is found to be : Rate = k[A][B] Concentration of reactant ‘B’ is doubled, keeping the concentration of ‘A’ constant, the value of rate constant will be..........

Rate law for the reaction A + 2B → C is found to be Rate = k[A][B] Concentration of reactant 'B' is doubled, keeping the concentration of 'A' constant, the value of rate constant will be..........

Compounds 'A' and 'B' react according to the following chemical equation. A(g) + 2B(g) → C(g) Concentration of either 'A' or 'B' were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

For a general reaction X → Y, the plot of conc. Of X vs time is given in the figure. What is the order of the reaction and what are the units of rate constant?

For a chemical reaction, X → Y, the rate of reaction increases by a factor of 1.837 when the concentration of X is increased by 1.5 times, the order of the reaction with respect to X is:

A first order reaction is 50% completed in 1.26 × 10¹⁴ s. How much time would it take for 100% completion?

Threshold energy is equal to

Consider the Arrhenius equation given below and mark the correct option. k = Ae⁻ᴱₐ/ᴿᵀ

A first order reaction takes 40 min for 30% decomposition. What will be t₁/₂?

For the reaction A + B → products, what will be the order of reaction with respect to A and B?

An endothermic reaction with high activation energy for the forward reaction can be shown by the figure

What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C ? (R = 8.314 J mol⁻¹ K⁻¹)

Consider the reaction: 2N₂O₅ ⇌ 4NO₂ If -d[N₂O₅]/dt = k and d[NO₂]/dt = k' then

According to Arrhenius equation, rate constant k is equal to Ae⁻ᴱᵃ/ᴿᵀ. Which of the following options represents the graph of ln k vs 1/T?

Observe the given graphs carefully. Which of the given orders are shown by the graphs respectively?

In a first order reaction, the concentration of reactant is reduced to 1/8 of the initial concentration in 75 minutes at 298 K. What is the half-life period of the reaction in minutes?

According to Arrhenius equation, rate constant k is equal to Ae⁻ᴱᵃ/ᴿᵀ. Which of the following options represents the graph of ln k vs 1/T?

For a general reaction X → Y, the plot of conc. of X vs time is given in the figure. What is the order of the reaction and what are the units of rate constant?

Match List I with List II: Choose the correct answer from the options given below:

For a certain reaction R → Product, the plot of concentration [R] vs time has a negative slope as shown. The order of reaction is:

Given below is an expression for the rate constant of a first-order reaction occurring at a certain temperature, T (K). ln k = 14.³⁴⁻ \(\frac{1.25 \times 10^4}{T}\) The energy of activation in kcal mol⁻¹ for the reaction is : (Given: k in s⁻¹, R = 1.987 cal mol⁻¹ K⁻¹)

If the half-life (t₁/₂) for a first order reaction is 1 minute, then the time required for 99.9% completion of the reaction is closest to:

If the rate constant of a reaction is 0.03 s⁻¹, how much time does it take for 7.2 mol L⁻¹ concentration of the reactant to get reduced to 0.9 mol L⁻¹? (Given: log 2 = 0.301)

Activation energy of any chemical reaction can be calculated if one knows the value of

Which plot of ln k vs 1/T is consistent with Arrhenius equation?

The rate of a reaction quadruples when temperature changes from 27°C to 57°C. Calculate the energy of activation. Given R = 8.314 J K⁻¹ mol⁻¹, log 4 = 0.6021

For a certain reaction, the rate = k[A]²[B], when the initial concentration of A is tripled keeping concentration of B constant, the initial rate would

Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R: Assertion A: A reaction can have zero activation energy. Reasons R: The minimum extra amount of energy absorbed by reactant molecules so that their energy becomes equal to threshold value, is called activation energy. In the light of the above statements, choose the correct answer from the options given below:

The given graph is a representation of kinetics of a reaction. The y and x axes for zero and first order reactions, respectively are:

For a first order reaction A → Products, initial concentration of A is 0.1 M, which becomes 0.001 M after 5 minutes. Rate constant for the reaction in min⁻¹ is

For a reaction A→B, enthalpy of reaction is −4.2 kJ mol⁻¹ and enthalpy of activation is 9.6 kJ mol⁻¹. The correct potential energy profile for the reaction is shown in option.

The slope of Arrhenius Plot (ln k v/s 1/T) of first order reaction is −5 × 10³ K. The value of Eₐ of the reaction is. Choose the correct option for your answer. [Given R = 8.314 J/K⁻¹mol⁻¹]

An increase in the concentration of the reactants of a reaction leads to change in:

The rate constant for a first order reaction is 4.606 × 10⁻³ s⁻¹. The time required to reduce 2.0 g of the reactant to 0.2 g is:

For the chemical reaction, N₂H₄ + 3H₂O₂ → N₂ + 4H₂O, the CORRECT option is

If the rate constant for a first order reaction is k, the time (t) required for the completion of 99% of the reaction is given by ______.

The CORRECT difference between first- and second-order reactions is that __________.

In the electrochemical cell, Zn | ZnSO₄(0.01 M) || CuSO₄(1.0 M) | Cu, the emf of this Daniel Cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ changed to 0.01 M, the emf changes to E₂. From the following, which one is the relationship between E₁ and E₂? (Given, RT/F = 0.059)

Mechanism of a hypothetical reaction X₂ + Y₂ ⟶ 2XY is given below: (i) X₂ ⟶ X + X ... fast (ii) X + Y₂ ⟶ XY + Y ... slow (iii) X + Y ⟶ XY ... fast The overall order of the reaction will be ______.

Which of the following statements is INCORRECT?

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

The addition of a catalyst during a chemical reaction alters which of the following quantities?

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

When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is ______.

The activation energy of a reaction can be determined from the slope of which of the following graphs?

For a reaction between A and B the order with respect to A is 2 and the order with respect to B is 3. The concentration of both A and B are doubled the rate will increase by a factor of:

A reaction is 50% complete in 2 hours and 75% complete in 4 hours. The order of reaction is: