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For the reaction $A + B \rightarrow \text{products}$, it is observed that: (i) On doubling the initial concentration of A only, the rate of reaction is also doubled. (ii) On doubling the initial concentrations of both A and B, there is a change by a factor of 8 in the rate of the reaction. The rate of this reaction is given by:

Match List-I with List-II. **List-I (Compound)** A. $NH_3$ B. $BrF_5$ C. $XeF_4$ D. $SF_6$ **List-II (Shape/geometry)** I. Trigonal Pyramidal II. Square Planar III. Octahedral IV. Square Pyramidal

Identify the incorrect statement among the following:

The decomposition of phosphine ($\text{PH}_3$) on tungsten at low pressure is a first-order reaction. It is because the:

For a first-order reaction $A \rightarrow \text{Products}$, initial concentration of A is $0.1 \text{ M}$, which becomes $0.001 \text{ M}$ after $5 \text{ minutes}$. Rate constant for the reaction in $\text{min}^{-1}$ is

Which pair of the following compounds has one lone pair of electrons on the central atom?

The bromination of acetone that occurs in acid solution is represented by this equation: $\text{CH}_3\text{COCH}_3(aq) + \text{Br}_2(aq) \rightarrow \text{CH}_3\text{COCH}_2\text{Br}(aq) + \text{H}^+(aq) + \text{Br}^-(aq)$ These kinetic data were obtained for given reaction concentrations: | $[\text{CH}_3\text{COCH}_3]$ (M) | $[\text{Br}_2]$ (M) | $[\text{H}^+]$ (M) | Initial rate, disappearance of $\text{Br}_2$ ($\text{M s}^{-1}$) | | :---: | :---: | :---: | :---: | | $0.30$ | $0.05$ | $0.05$ | $5.7 \times 10^{-5}$ | | $0.30$ | $0.10$ | $0.05$ | $5.7 \times 10^{-5}$ | | $0.30$ | $0.10$ | $0.10$ | $1.2 \times 10^{-4}$ | | $0.40$ | $0.05$ | $0.20$ | $3.1 \times 10^{-4}$ | Based on these data, the rate equation is:

A first-order reaction has a rate constant of $2.303 \times 10^{-3} \text{ s}^{-1}$. The time required for $40 \text{ g}$ of this reactant to reduce to $10 \text{ g}$ will be [Given that $\log_{10} 2 = 0.3010$]

A compound that does not undergo $S_N1$ reaction with $\text{OH}^-$ is:

Which of the following species contains an equal number of $\sigma$ and $\pi$ bonds?

The given graph is a representation of the kinetics of a reaction. The $y$ and $x$ axes for zero and first-order reactions, respectively are:

What is the rate constant for a reaction if the time taken by the first-order decomposition of $\text{SO}_2\text{Cl}_2$ to decompose to $40\%$ is $560 \text{ seconds}$? [Given: $\log 2.5 = 0.3979$]

Mechanism of a hypothetical reaction $X_2 + Y_2 \rightarrow 2XY$ is given below: (i) $X_2 \rightleftharpoons X + X$ (fast) (ii) $X + Y_2 \rightarrow XY + Y$ (slow) (iii) $X + Y \rightarrow XY$ (fast) The overall order of the reaction will be:

For the reaction, $\text{N}_2\text{O}_5(g) \rightarrow 2\text{NO}_2(g) + \frac{1}{2}\text{O}_2(g)$ the value of the rate of disappearance of $\text{N}_2\text{O}_5$ is given as $6.25 \times 10^{-3} \text{ mol L}^{-1}\text{s}^{-1}$. The rate of formation of $\text{NO}_2$ and $\text{O}_2$ is given respectively as:

The unit of rate constant for a zero-order reaction is:

Which of the following expression is correct for the reaction given below? $2HI(g) \rightarrow H_2(g) + I_2(g)$

When the initial concentration of the reactant is doubled, the half-life period of a zero-order reaction:

Given below are two statements: Assertion (A): A reaction can have zero activation energy. Reason (R): The minimum amount of energy required by reactant molecules so that their energy becomes equal to threshold value, is called activation energy.

Which of the following statements about the order of reaction is incorrect?

In a reaction, $A + B \rightarrow \text{Product}$, the rate is doubled when the concentration of $B$ is doubled, and the rate increases by a factor of $8$ when the concentrations of both the reactants ($A$ and $B$) are doubled. The rate law for the reaction can be written as: