Q.(i) Define order of reaction.

Showing the 12 most recent of 23 on this concept.

1. CBSE 2026Set A1 markMCQ
   Q.Which of the following represents the effect of temperature on reaction rate ?

   (a) Nernst's equation

   (b) Gibbs-Helmholtz equation

   (c) Arrhenius equation

   (d) Van't Hoff equation

   ›Reveal solutionSolution

   The Arrhenius equation, k = A e^(-Ea/RT), describes how the rate constant (and hence reaction rate) depends on temperature.

   The Arrhenius equation k = A e^(-Ea/RT) links the rate constant k to temperature T and activation energy Ea. It quantifies the effect of temperature on reaction rate. The Nernst equation relates electrod …

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2. CBSE 2026Set ANNUAL1 markMCQ
   Q.Activation energy of a chemical reaction can be determined by

   (a) rate constant at standard temperature

   (b) rate constants at two different temperatures

   (c) orientation of reactant molecules during the collision

   (d) using catalyst

   ›Reveal solutionSolution

   Activation energy is found from the Arrhenius equation by measuring the rate constant of a reaction at two (or more) different temperatures.

   The Arrhenius equation is: k = A e^(-Ea/RT)

   Taking the natural log at two temperatures T1 and T2 with rate constants k1 and k2, and subtracting, gives:

   ln(k2/k1) = -(Ea/R)(1/T2 - 1/T1)

   …

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3. CBSE 2026Set ANNUAL1 markMCQ
   Q.The correct form of Arrhenius equation is:

   (a) k = e^(-Ea/RT)

   (b) k = Ea/RT

   (c) k = log_e (Ea/R)

   (d) k = A e^(-Ea/RT)

   ›Reveal solutionSolution

   The Arrhenius equation is $k = Ae^{-E_a/RT}$, relating the rate constant to temperature and activation energy.

   The Arrhenius equation, proposed by Svante Arrhenius, expresses how the rate constant $k$ of a reaction varies with temperature:

   $k = Ae^{-E_a/RT}$ …

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4. CBSE 2026Set ANNUAL1 markMCQ
   Q.The influence of temperature on the rate of a reaction is determined by

   (a) Nernst equation

   (b) Gibbs-Helmholtz equation

   (c) van't Hoff equation

   (d) Arrhenius equation

   ›Reveal solutionSolution

   Of the four named equations, only the Arrhenius equation directly relates the rate constant of a reaction to temperature.

   Why the others are not it:

   • (a) Nernst equation: relates the EMF of an electrochemical cell to the concentrations (activities) of the species involved — an electrochemistry relationship, not a kinetics one.
   • (b) Gibbs–Helmholtz equation: relates the temperature dependence of Gibbs free energy change to enthalpy and entropy changes — a thermodynamics relationship about spontaneity, not reaction rate.
   • (c) van't Hoff equation: relates the equilibrium constant ($K_c$ or $K_p$) to temperature — about the position of equilibrium, not how fast equilibrium is reached.

   Arrhenius equation (d): …

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5. CBSE 2025Set X11 mark
   Q.Arrhenius factor is also called __________ factor.

   ›Reveal solutionSolution

   The Arrhenius factor $A$ is also called the frequency (pre-exponential) factor.

   The Arrhenius equation is $k = A\,e^{-E_a/RT}$, where $A$ is the Arrhenius constant. It represents the frequency of collisions with correct orientation and is therefore cal …

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6. CBSE 2025Set D1 markMCQ
   Q.The specific rate constant of a first order reaction depends upon

   (a) concentration of reactants

   (b) concentration of products

   (c) time

   (d) temperature

   ›Reveal solutionSolution

   The rate constant depends on temperature (via the Arrhenius equation), not on concentration or time.

   For a first order reaction rate = k[A]. The rate constant k is a proportionality constant characteristic of the reaction at a given temperature. According to the Arrhenius equation:

   k = A e^(-Ea/RT) …

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7. CBSE 2025Set D1 markMCQ
   Q.The temperature coefficient of most of the reactions lies between

   (a) 1 and 3

   (b) 2 and 3

   (c) 1 and 4

   (d) 2 and 4

   ›Reveal solutionSolution

   Temperature coefficient of most reactions is between 2 and 3.

   The temperature coefficient is the ratio of the rate constant at (T + 10) K to that at T K:

   temperature coefficient = k(T+10)/k(T)

   …

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8. CBSE 2025Set ANNUAL1 markMCQ
   Q.Which of the following represents Arrhenius equation?

   (a) k = Ae^(Ea/RT)

   (b) k = Ae^(-Ea/RT)

   (c) k = Ae^(Ea/R)

   (d) dk = Ae^(Ea/T)

   ›Reveal solutionSolution

   The Arrhenius equation relates the rate constant to temperature through an exponential term with a NEGATIVE activation-energy exponent.

   The Arrhenius equation is:

   $k = A\,e^{-E_a/RT}$ …

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9. CBSE 2025Set ANNUAL1 mark
   Q.Define : Activation energy.

   ›Reveal solutionSolution

   Activation energy is the energy barrier reactant molecules must cross to be converted into products.

   According to collision theory, not every collision between reactant molecules leads to product formation — only those collisions in which molecules possess sufficient energy (and correct orientation) are effective. The activation energy, $E_a$, is defined as the minimum extra energy that reactant molecules, over and above their average energy, must acquire before they can react to form products. Equivalently, it is the difference between the threshold energy (the minimum energy needed …

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10. CBSE 2024Set ANNUAL1 mark
    Q.The kinetic energy of maximum fraction of reactant molecules is called ______.

    ›Reveal solutionSolution

    On a Maxwell-Boltzmann distribution-of-energy curve, the energy value at the peak (where the curve is highest) is possessed by the largest fraction of molecules - this is called the most probable kinetic energy.

    In any collection of gas/reactant molecules at a given temperature, molecules do not all have the same kinetic energy; their energies are spread out according to the Maxwell-Boltzmann distribution.

    When the fraction of molecules (y-axis) is plotted against kinetic energy (x-axis), the curve rises, reaches a maximum, then falls - the energy value at this peak is the one possessed by the largest fraction of molecules, called the most probable kinetic energy. …

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11. CBSE 2024Set ANNUAL1 markMCQ
    Q.Activation energy of a chemical reaction can be determined by :

    (a) determining the rate constant at standard temperature

    (b) determining the rate constant at two temperatures

    (c) determining probability of collision

    (d) using catalyst

    ›Reveal solutionSolution

    Activation energy comes from the Arrhenius equation, which needs the rate constant measured at (at least) two temperatures to solve for $E_a$.

    The Arrhenius equation is $k = A\,e^{-E_a/RT}$, or in logarithmic form:

    $\ln k = \ln A - \frac{E_a}{RT}$

    A single rate constant at one temperature carries two unknowns ($A$ and $E_a$) and cannot be solved alone. Measuring $k$ at two different temperatures $T_1$ and $T_2$ gives two equations, which combine to: …

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12. CBSE 2024Set ANNUAL1 markMCQ
    Q.The activation energies of the forward and backward reactions are 15 kcal/mol and 20 kcal/mol. Then the change in $\Delta H$ is –

    (a) 5 kcal/mol

    (b) – 35 kcal/mol

    (c) 15 kcal/mol

    (d) 25 kcal/mol

    ›Reveal solutionSolution

    Subtracting the backward activation energy from the forward one gives ΔH = −5 kcal/mol, meaning the reaction is exothermic by 5 kcal/mol.

    The relationship between the enthalpy change of a reaction and the activation energies of its forward and reverse directions is:

    $\Delta H = E_a(\text{forward}) - E_a(\text{backward})$

    Substituting the given values:

    $\Delta H = 15 - 20 = -5\ kcal/mol$

    …

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