JEE Main Chemical Kinetics — practice questions
31 free MCQs with worked solutions. Tap any question for the answer + explanation, or practice them all in the app.
Practice JEE Main 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 $T_1$ Rate of reaction is defined as:Rate law: r = k [A]ᵐ [B]ⁿ. Sum m + n is called:For a first-order reaction, rate ∝:Units of rate constant k for a first-order reaction:Arrhenius equation: k = A × e^(-Ea/RT). What is A?For first-order reaction, half-life t₁/₂:For zero-order reaction A → P, rate equals:For first-order, integrated rate law:For second-order reaction (single reactant), integrated rate law:Temperature dependence: per Arrhenius, raising T from 300 K to 310 K (Ea = 50 kJ/mol) increases k by approximaCatalyst affects:Order of reaction CAN be determined from:A first-order reaction is 25% complete in 20 min. Time for 75% completion:For a reaction with Ea = 100 kJ/mol, find k₂/k₁ when T goes from 300 K to 350 K. (R = 8.314 J/mol K):For a 2nd-order reaction with [A]₀ = 0.5 M and k = 0.1 L mol⁻¹ s⁻¹, half-life:For complex reaction with rate-determining step that involves 2 molecules of A, the order in A is:For Arrhenius plot of ln k vs 1/T, slope equals:Threshold energy = Ea + average kinetic energy of reactants. If Ea = 50 kJ/mol and avg KE = 4 kJ/mol, thresholFor reaction A → B with rate constant 10⁻³ s⁻¹ (first order), concentration after 1000 s if [A]₀ = 1 M:A reaction has k = 0.05 s⁻¹. After how many seconds is 90% complete?For radioactive decay (1st order), if 1/8 of initial nuclei remain, how many half-lives elapsed?A catalyst lowers Ea from 100 kJ/mol to 75 kJ/mol at T = 300 K. Rate enhancement factor (R = 8.314 J/mol K):For elementary bimolecular reaction 2 NO → products, rate law is: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: