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?

What happens to the rate constant of a chemical reaction with a rise in temperature by 10°C?

What is the term used for the expression that relates the rate of a reaction to the concentration of reactants?

What is the order of the reaction with respect to H2O2 in the given reaction mechanism?

What is the order of the reaction with respect to H2O2 in the given reaction?

What is a catalyst in a chemical reaction?

What is the term used to describe the constant specific to a particular reaction in the Arrhenius equation?

What is the relationship between the half-life of a zero order reaction and the initial concentration of reactants?

What is the unit of rate for a reaction when concentration is measured in mol L⁻¹ and time in seconds?

What is the unit of rate for a reaction where concentration is measured in mol L⁻¹ and time in seconds?

What is the activation energy (E_a) for the reaction 2 HI(g) → H2 + I2(g) at 581K?

What is the unit of the rate of a reaction when concentration is measured in mol L⁻¹ and time in seconds?

What does the rate constant (k) in a differential rate equation represent?

Which of the following statements about reaction rates and their characteristics is correct?

Which of the following statements correctly describes the relationship between stoichiometric coefficients and the rate law of a reaction?

Which of the following statements about the rate of reaction is correct?

Which of the following statements about reaction rates and stoichiometric coefficients is correct?

Which of the following statements about reaction orders and rate constants is correct?

Assertion (A): The molecularity of the slowest step in a reaction mechanism equals the overall reaction order.

Reason (R): The order of a reaction is always determined by the stoichiometric coefficients of the reactants.

Assertion (A): The rate of a chemical reaction depends on the concentration of reactants.

Reason (R): For a first-order reaction, the rate constant can be calculated using the change in concentration over time.

Assertion (A): In a bimolecular elementary reaction, the rate of the reaction depends on the concentration of the reactants involved in the slowest step.

Reason (R): The slowest step in a reaction mechanism is the rate-determining step, influencing the overall reaction rate.

Assertion (A): The rate of a reaction can be determined by the balanced chemical equation alone.

Reason (R): The rate law is expressed in terms of the molar concentration of reactants, which may or may not correspond to their stoichiometric coefficients.

Assertion (A): The rate of a chemical reaction increases with an increase in temperature.

Reason (R): The frequency factor A in the Arrhenius equation increases with temperature.

Assertion (A): The rate law for a reaction is not necessarily determined by the stoichiometric coefficients of the reactants.

Reason (R): The exponents in the rate law are determined experimentally and can differ from the stoichiometric coefficients.

Assertion (A): The rate of a reaction can be influenced by the initial pressure of reactants.

Reason (R): For a reaction A(g) → B(g) + C(g), the change in partial pressure of A over time can be used to determine the rate constant for a first-order reaction.

Assertion (A): The rate of a first-order reaction is dependent on the concentration of the reactant.

Reason (R): The plot of ln[R] vs time for a first-order reaction is a straight line with a negative slope.

Assertion (A): The instantaneous rate of a reaction can be determined by considering the average rate over an infinitesimally small time interval.

Reason (R): The average rate of a reaction is constant for the time interval over which it is calculated.

Assertion (A): The probability of a trimolecular reaction occurring is lower than that of a bimolecular reaction.

Reason (R): Trimolecular reactions involve simultaneous collision between three reacting species, making them rare and slow to proceed.

Assertion (A): For a reaction with a given activation energy, increasing the temperature will increase the rate constant.

Reason (R): The rate of a reaction is directly proportional to the concentration of reactants.

Assertion (A): The rate constant of a reaction is independent of the concentration of reactants.

Reason (R): For a first order reaction, the rate constant can be calculated using the concentration of the reactants at different times.