NEET Chemistry Chemical Kinetics MCQs

For a reaction A + B → C, the rate law is found to be Rate = k[A]²[B]⁻¹. If the concentration of A is tripled while keeping the concentration of B constant, the factor by which the reaction rate changes is:

A reaction follows the rate law: Rate = k[A][B]². If the initial concentrations of both A and B are doubled, and the temperature remains constant, the initial rate of the reaction will increase by a factor of:

For a zero-order reaction, the plot of concentration of reactant versus time is:

The half-life of a first-order reaction is 20 minutes. What fraction of the reactant remains after 80 minutes?

A reaction has a rate constant 'k' at temperature T₁ and k' at T₂ (T₂ > T₁). If the activation energy is Ea, which expression correctly relates k, k', T₁, and T₂ according to the Arrhenius equation?

For a reaction with the rate law: Rate = k[A]^[1/2][B], if the concentration of B is doubled while keeping [A] constant, how does the half-life change?

A reaction between gases X and Y follows the rate law: Rate = k[X]²[Y]. If the concentration of X is tripled and the concentration of Y is halved, the new rate will be:

Two molecules A and B collide, but no reaction occurs. Which of the following MUST be true?

For a reaction with an activation energy ($E_a$) of 50 kJ/mol, how much would a 10°C increase in temperature increase the rate constant, according to the Arrhenius equation (assuming $ext{R} = 8.314 ext{ J mol}^{-1} ext{K}^{-1}$) at room temperature (approx. 300K)?

A reaction proceeds via a two-step mechanism. The first step is a fast, reversible equilibrium with a small equilibrium constant. The second step is slow. Which of the following is MOST likely true about the overall reaction rate?