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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:
Which plot of $\ln k$ vs $1/T$ is consistent with Arrhenius equation?
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:
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?
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 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:
Consider the reaction: $\text{CH}_3\text{CH}_2\text{CH}_2\text{Br} + \text{NaCN} \rightarrow \text{CH}_3\text{CH}_2\text{CH}_2\text{CN} + \text{NaBr}$ This reaction will be the fastest in
The efficiency of a fuel cell is given by:
Which of the following is the most preferred method for preparing pure alkyl chlorides from alcohols?
The reaction of hydrogen and iodine monochloride is given as: $H_2(g) + 2ICl(g) \rightarrow 2HCl(g) + I_2(g)$. This reaction is of first order with respect to $H_2(g)$ and $ICl(g)$, for which of the following proposed mechanisms: Mechanism A: $H_2(g) + 2ICl(g) \rightarrow 2HCl(g) + I_2(g)$ Mechanism B: $H_2(g) + ICl(g) \rightarrow HCl(g) + HI(g)$; slow $HI(g) + ICl(g) \rightarrow HCl(g) + I_2(g)$; fast
If force [F], acceleration [A] and time [T] are chosen as the fundamental physical quantities. Find the dimensions of energy.
Which of the following methods is incorrect for the synthesis of alkenes?
The reaction of $\text{C}_6\text{H}_5\text{CH=CHCH}_3$ with $\text{HBr}$ produces:
Consider the reactions: (i) $(\text{CH}_3)_2\text{CHCH}_2\text{Br} \xrightarrow{\text{C}_2\text{H}_5\text{OH}} (\text{CH}_3)_2\text{CHCH}_2\text{OC}_2\text{H}_5 + \text{HBr}$ (ii) $(\text{CH}_3)_2\text{CHCH}_2\text{Br} \xrightarrow{\text{C}_2\text{H}_5\text{O}^-} (\text{CH}_3)_2\text{CHCH}_2\text{OC}_2\text{H}_5 + \text{Br}^-$ The mechanisms of reactions (i) and (ii) are, respectively:
If $E^\circ_{\text{Fe}^{2+}/\text{Fe}} = -0.441 \text{ V}$ and $E^\circ_{\text{Fe}^{3+}/\text{Fe}^{2+}} = 0.771 \text{ V}$, the standard emf of the reaction: $\text{Fe} + 2\text{Fe}^{3+} \rightarrow 3\text{Fe}^{2+}$ will be: