JEE Chemistry - MCQ Practice Questions

In the reaction 2A + B → C, if the concentration of A is doubled and B is tripled, the rate increases by 12 times. The rate law is:

For a bimolecular reaction between A and B molecules, the collision frequency (Z) depends on:

A catalyst increases the rate of reaction by:

The reaction A → B has rate constant k = 4.5 × 10⁻³ min⁻¹. This is a first-order reaction. The percentage of A remaining after 100 minutes is:

In enzyme catalysis, the Michaelis constant (Km) represents:

For a reaction with rate law Rate = k[A]⁰[B]¹, if [B] is increased 4 times while [A] remains constant, the rate increases by:

In the reaction mechanism: (1) A + B ⇌ AB (fast), (2) AB + C → ABC (slow), the order predicted from this mechanism is:

The temperature coefficient (Q₁₀) for a reaction is 2.5. If the rate at 300 K is r, then the rate at 320 K is approximately:

For the reaction A → B, experimental data shows: [A] vs time is a straight line. This indicates:

In the complex reaction: A + B → I (fast equilibrium), I + B → C (slow), the rate law derived from this mechanism is:

The pre-exponential factor (A) in the Arrhenius equation is related to:

For an elementary reaction: A + A + B → Products, the rate law is:

For the reaction 2NO + O₂ → 2NO₂, the rate law is Rate = k[NO]²[O₂]. What is the overall order of reaction?

Half-life of a first-order reaction is 30 minutes. What fraction of reactant remains after 90 minutes?

The rate constant of a reaction increases from 4 × 10⁻³ s⁻¹ to 8 × 10⁻³ s⁻¹ when temperature increases from 300K to 310K. Calculate activation energy (R = 8.314 J/mol·K)

Which of the following statements about collision theory is INCORRECT?

For a zero-order reaction, the integrated rate law is [A] = [A]₀ - kt. If [A]₀ = 0.5 M and k = 0.02 M·s⁻¹, find time when [A] = 0

Consider the mechanism: (1) A + B ⇌ C (fast equilibrium), (2) C + D → E + F (slow). Which is the rate-determining step?

The rate law for a reaction is Rate = k[A]¹[B]⁰. If [B] is doubled and [A] is halved, how does the rate change?

At 25°C, the rate constant is 3 × 10⁻² s⁻¹ and at 35°C it is 6 × 10⁻² s⁻¹. What is the temperature coefficient (Q₁₀) for this reaction?