List of top Chemistry Questions on Collision Theory of Chemical Reactions

Following are the four molecules ``P``, ``Q``, ``R`` and ``S``. Which one among the four molecules will react with H-Br(aq) at the fastest rate? Molecules:

\[ P: \text{Cyclic compound with two O groups attached to the ring.} \] \[ Q: \text{Cyclic compound with one O group and one CH$_3$ group attached to the ring.} \] \[ R: \text{Cyclic compound with one O group attached to the ring and one CH$_3$ group attached to the ring.} \] \[ S: \text{Cyclic compound with one CH$_3$ group attached to the ring.} \]

What is another term used for the probability factor (P) in collision theory?

Among the ligands $ {NH}_3, \, {en}, \, {CN}^-, \, {CO} $, the correct order of their increasing field strength is:

The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of reaction with respect to reactant B is:

For the reaction H₂(g) + Br₂(g) → 2HBr(g), the experimental data suggest, rate = k[H₂][Br₂]¹/2. The molecularity and order of the reaction are respectively

In the reaction: P + Q longrightarrow ?R + S The time taken for 75% reaction of P is twice the time taken for 50% reaction of P. The concentration of Q varies with time as shown in the figure. The overall order of the reaction is:

Consider the reaction: Cl₂(aq) + H₂S(aq) → S(s) + 2H⁺(aq) + 2Cl⁻(aq) The rate equation for this reaction is: rate = k[Cl₂][H₂S] Which of these mechanisms is/are consistent with the rate equation? A. Cl₂ + H₂S → H⁺ + Cl⁻ + Cl⁺ + HS⁻ (slow) Cl⁺ + HS⁻ → H⁺ + Cl⁻ + S (fast) B. H₂S rightleftharpoons H⁺ + HS⁻ (fast equilibrium) Cl₂ + HS⁻ → 2Cl⁻ + H⁺ + S (slow)

The unit of rate constant for reactions of second order is

In a first order reaction with time the concentration of the reactant decreases

The rate constant of a reaction is 1.5×10⁻³ at 25°C and 2.1×10⁻² at 60°C. The activation energy is:

The accompanying figure depicts a change in concentration of species A and B of the reaction A → B, as a function of time. The point of intersection of the two curves represents:

For the reaction
$\text{H}_2(g) + \text{Br}_2(g) \to 2 \text{HBr}(g)$,

the experimental data suggest the rate law
$\text{Rate} = k[\text{H}_2][\text{Br}_2]^{1/2}$.
The molecularity and order of the reaction are respectively

The rate of reaction between two reactants A and B decreases by a factor of 4 if the concentration of reactant B is doubled. The order of this reaction with respect to reactant B is

Consider the reaction:
$ \text{Cl}_2 (aq) + \text{H}_2\text{S} (aq) \rightarrow \text{S} (s) + 2\text{H}^+ (aq) + 2\text{Cl}^- (aq) $
The rate equation is $ \text{rate} = k[\text{Cl}_2][\text{H}_2\text{S}] $.
Which of the following mechanisms is/are consistent with this rate equation?

In the reaction P+Q→ 2R+S, the time taken for 75% reaction of P is twice the time taken for 50% reaction of P. The concentration of Q varies with time as shown. The overall order of the reaction is: