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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
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:
Among the following, the correct order of acidity is:
The number of electrons delivered at the cathode during electrolysis by a current of $1 \text{ ampere}$ in $60 \text{ seconds}$ is (charge on electron = $1.60 \times 10^{-19} \text{ C}$):
Buffer solutions have constant acidity and alkalinity because:
In $S_N2$ substitution reaction of the type $\text{R-Br} + \text{Cl}^- \xrightarrow{\text{DMF}} \text{R-Cl} + \text{Br}^-$, which one of the following has the highest relative rate?
$\text{CCl}_2\text{F}_2$ is one of the most common haloalkanes used in industries. The reaction through which it is manufactured from tetrachloromethane is called: