List of top Chemistry Questions on Collision Theory of Chemical Reactions asked in BITSAT

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: 

The unit of rate constant for reactions of second order is:
In a first order reaction with time the concentration of the reactant decreases:
A gaseous reaction \(X_2(g) \rightarrow Y + \frac{1}{2}Z(g)\). There is an increase in pressure from 100 mm to 120 mm in 5 minutes. The rate of disappearance of \(X_2\) is:
The reduction of peroxodisulphate ion by I\(^{-}\) ion is expressed by \(\text{S}_2\text{O}_8^{2-} + 3\text{I}^- \rightarrow 2\text{SO}_4^{2-} + \text{I}_3^-\). If rate of disappearance of I\(^{-}\) is \(9/2 \times 10^{-3}\,\text{mol L}^{-1}\text{s}^{-1}\), what is the rate of formation of \(2\text{SO}_4^{2-}\) during same time?
Velocity constant of a reaction at 290 K was found to be \( 3.2 \times 10^{-3} \). At 300 K it will be:
\( 2N_2O_5 \to 4NO_2 + O_2 \) If rate and rate constant for above reaction are \( 2.40 \times 10^{-5} \, \text{mol L}^{-1} \text{s}^{-1} \) and \( 3 \times 10^{-5} \, \text{s}^{-1} \), respectively, then calculate the concentration of \( N_2O_5 \):
During the kinetic study of the reaction 2A + B → C + D, the following results were obtained. Based on the data, which rate law is correct?
The activation energy for a simple chemical reaction A → B is Eₐ in the forward direction. The activation energy for reverse reaction
The following data are for the decomposition of ammonium nitrite in aqueous solution: arrayc c Vol. of N₂ in cc & Time (min)
6.25 & 10
9.00 & 15
11.40 & 20
13.65 & 25
35.65 & ∞ array The order of reaction is: