STANDARD Chemistry Chemical Kinetics Class 12 Questions

For a reaction, P + Q → 2R + S. Which of the following statements is incorrect?

For the reaction, 2N₂O₅ → 4NO₂ + O₂, the rate of reaction can be expressed in terms of time and concentration by the expression:

Consider the reaction: 2N₂O₄ ⇌ 4NO₂ If \( \frac{d[N_2O_4]}{dt} = k \) and \( \frac{d[NO_2]}{dt} = k' \) then

Consider the reaction, 2N₂O₅ → 4NO₂ + O₂ In the reaction, NO₂ is being formed at the rate of 0.0125 mol L⁻¹ s⁻¹. What is the rate of reaction at this time?

In a reaction, 2HI → H₂ + I₂, the concentration of HI decreases from 0.5 mol L⁻¹ to 0.4 mol L⁻¹ in 10 minutes. What is the rate of reaction during this interval?

Nitrogen dioxide (NO₂) dissociated into nitric oxide (NO) and oxygen (O₂) as follows: 2NO₂ → 2NO + O₂. If the rate of decrease of concentration of NO₂ is 6.0 × 10⁻¹² mol L⁻¹ s⁻¹, what will be the rate of increase of concentration of O₂?

In a reaction, 2X → Y, the concentration of X decreases from 3.0 moles/litre to 2.0 moles/litre in 5 minutes. The rate of reaction is:

The rate constant of a reaction depends upon:

The rate law for a reaction, A + B → C + D is given by the expression k[A]. The rate of reaction will be:

A reaction in which reactants (R) are converted into products (P) follows second order kinetics. If concentration of R is increased by four times, what will be the increase in the rate of formation of P?

The rate constant for the reaction, 2N₂O₃ → 4NO₂ + O₂ is 2 × 10⁻³ s⁻¹. If rate of reaction is 1.4 × 10⁻³ mol L⁻¹ s⁻¹, what will be the concentration of N₂O₃ in mol L⁻¹?

What will be the rate equation for the reaction 2X + Y → Z, if the order of the reaction is zero?

Find the values of A, B and C in the following table for the reaction X + Y → Z. The reaction is of first order w.r.t. X and zero w.r.t. Y.

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:

For a reaction X → Y, the rate of reaction becomes twenty seven times when the concentration of X is increased three times. What is the order of the reaction?

Match the rate law given in column-I with the dimensions of rate constants given in column-II and mark the appropriate choice. Column-I (A) Rate = k[NH₃]⁰ (B) Rate = k[H₂O₂][I⁻] (C) Rate = k[CH₃CHO]³/₂ (D) Rate = k[C₂H₅Cl] Column-II (i) Mol L⁻¹ s⁻¹ (ii) L mol⁻¹ s⁻¹ (iii) s⁻¹ (iv) L¹/² mol⁻¹/² s⁻¹

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

For a zero order reaction, rate = k = \( \frac{dx}{dt} \). Units of k = mol L⁻¹ s⁻¹

For a reaction, X + Y → Z, rate ∝ [X]. What are the molecularity and order of reaction?

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

A first order reaction is 20% complete in 10 minutes. What is the specific rate constant for the reaction?

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

A first order reaction has a rate constant 1.15 × 10⁻³ s⁻¹. How long will 5g of this reactant take reduce to 3g?

Which of the following describes the given graph correctly?

Match the graphs given in column-I with the order given in column-II and mark the appropriate choice.

Half-life period of a first order reaction is 10 min. What percentage of the reaction will be completed in 100 min?

The rate constant for a first order reaction is 2 × 10⁻² min⁻¹. The half-life period of reaction is:

The half-life of the reaction X → Y, following first order kinetics, when the initial concentration of X is 0.01 mol L⁻¹ and initial rate is 0.00352 mol L⁻¹ min⁻¹ will be:

The time taken for 90% of a first order reaction to complete is approximately

Which one of the following is wrongly matched?

The temperature dependence of the rate constant k is expressed as k = Ae⁻ᴱᵃ/ᴿᵀ. When a plot between log k and 1/T is plotted, we get the graph as shown. What is the value of slope in the graph?

Which of the following statements is not correct?

The increase in concentration of the reactants lead to change in:

Threshold energy is equal to:

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

Which of the following statements is correct?

Which of the following statements is not correct for the catalyst?

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 _______.

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

For a first order reaction, the time required for completion of 90% reaction is 'x' times the half-life of the reaction. The value of 'x' is: (Given: ln 10 = 2.303 and log 2 = 0.3010)

For a reaction of order n, the unit of the rate constant is:

For reaction aA → xP, when [A] = 2.2 mM, the rate was found to be 2.4 mM s⁻¹. On reducing concentration of A to half, the rate changes to 0.6 mM s⁻¹. The order of reaction with respect to A is:

The rate constant of reaction is 3.6 × 10⁻³ s⁻¹. The order of the reaction is:

75% of a zero order reaction completes in 4h, 87.5% of the same reaction completes in:

For a first order reaction, A → P, t₁/₂ (half-life) is 10 days. The time required for 1/4th conversion of A (in days) is (ln 2 = 0.693, ln 3 = 1.1)

If 50% of a reaction occurs in 100 seconds and 75% of the reaction occurs in 200 seconds, the order of this reaction is:

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