UP Board Class 12 Chemical Kinetics — practice questions
22 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice UP Board Class 12 Chemical Kinetics in the app →For a first-order reaction, the half-life period $t_{1/2}$ is related to the rate constant $k$ as:The units of the rate constant for a zero-order reaction are:Acid-catalysed hydrolysis of ethyl acetate, $\mathrm{CH_3COOC_2H_5 + H_2O \to CH_3COOH + C_2H_5OH}$, follows pAccording to the Arrhenius equation, if $k_1$ and $k_2$ are the rate constants at absolute temperatures $T_1$ For the reaction $A + B \to$ products, the rate law $r = k[A][B]^2$ has overall order:A first-order reaction has rate constant $k = 6.93\times 10^{-3}$ s$^{-1}$. Its half-life is:The Arrhenius equation $k = Ae^{-E_a/RT}$ predicts that, as temperature rises, the rate constant:A catalyst on the bench changes:The RATE of a chemical reaction is defined asThe RATE CONSTANT ($k$) of a reaction isThe units of the rate constant $k$ for a FIRST-ORDER reaction areWhich of the following best describes the difference between ORDER and MOLECULARITY of a reaction?For a FIRST-ORDER reaction with rate constant $k$, the half-life is given byFor a ZERO-ORDER reaction $A \to \text{products}$, which graph is a STRAIGHT LINE?A first-order reaction has a rate constant of $k = 6.93\times 10^{-3}\,\text{s}^{-1}$ at a certain temperatureThe Arrhenius equation $k = A\,e^{-E_a/RT}$ predicts that, at a given temperature, increasing the ACTIVATION EDoubling the absolute temperature from $T_1 = 300\,\text{K}$ to $T_2 = 600\,\text{K}$ for a reaction with actiA reaction has rate law $\text{rate} = k[A][B]^2$. If $[A]$ is DOUBLED and $[B]$ is HALVED, the new rate compaThe hydrolysis of a sugar like cane sugar (sucrose) in dilute aqueous acid is FIRST ORDER with respect to sucrAccording to collision theory, for a chemical reaction to occur, colliding molecules must possessThe half-life of a first-order reaction $\mathrm{N_2O_5(g)} \to 2\mathrm{NO_2(g)} + (1/2)\mathrm{O_2(g)}$ at $A catalyst increases the rate of a chemical reaction by