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The temperature dependence of the rate constant ($k$) of a chemical reaction is written in terms of the Arrhenius equation, $k = A e^{-E^*/RT}$. The activation energy ($E^*$) of the reaction can be calculated by plotting:

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

For a reaction $3A \rightarrow 2B$, the average rate of appearance of B is given by $\frac{\Delta [B]}{\Delta t}$. The correct relation between the average rate of appearance of B with the average rate of disappearance of A is:

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

The half-life of a first-order reaction is $2000 \text{ years}$. If the concentration after $8000 \text{ years}$ is $0.02 \text{ M}$, then the initial concentration was:

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:

Effective collisions are known to possess: A: Energy greater than the threshold energy. B: Breaking of old bonds in the reactant. C: Formation of a new bond in the product. D: High activation energy. E: Proper orientation. Choose the correct answer from the options given below:

Which plot of $\ln k$ vs $1/T$ is consistent with Arrhenius equation?

For the reaction, $2A + B \rightarrow 3C + D$, which of the following is an incorrect expression for the rate of reaction?

In the reaction, $BrO_3^-(aq) + 5Br^-(aq) + 6H^+ \rightarrow 3Br_2(l) + 3H_2O(l)$. The rate of appearance of bromine ($Br_2$) is related to the rate of disappearance of bromide ions ($Br^-$) as:

In a zero-order reaction for every 10 °C rise of temperature, the rate is doubled. If the temperature is increased from 10 °C to 100 °C, the rate of the reaction will become:

For a certain reaction, the rate = $k[A]^2[B]$, when the initial concentration of A is tripled keeping the concentration of B constant, the initial rate would be:

During the kinetic study of the reaction, 2A + B → C + D, following results were obtained: | Run | [A] / mol L⁻¹ | [B] / mol L⁻¹ | Initial rate of formation of D / mol L⁻¹ min⁻¹ | | :--- | :--- | :--- | :--- | | I | 0.1 | 0.1 | 6.0 × 10⁻³ | | II | 0.3 | 0.2 | 7.2 × 10⁻² | | III | 0.3 | 0.4 | 2.88 × 10⁻¹ | | IV | 0.4 | 0.1 | 2.40 × 10⁻² | Based on the above data which one of the following is correct?

The correct order of increasing C-X bond reactivity toward nucleophiles among the following is: I. [Missing] II. [Missing] III. $(\text{CH}_3)_3\text{C-X}$ IV. $(\text{CH}_3)_2\text{CH-X}$

For the chemical reaction $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$, the correct option is:

The compound that will react most readily with gaseous bromine has the formula:

The compound that will undergo $\text{S}_\text{N}1$ reaction with the fastest rate is:

The Gibb's energy for the decomposition of $Al_2O_3$ at $500^{\circ}\text{C}$ is as follows: $\frac{2}{3}Al_2O_3 \rightarrow \frac{4}{3}Al + O_2 \ ; \ \Delta_rG = + 960 \text{ kJ mol}^{-1}$ The potential difference needed for the electrolytic reduction of aluminium oxide ($Al_2O_3$) at $500^{\circ}\text{C}$ is at least: