Rate of Chemical Reactions
Chemistry ⇒ Chemical Kinetics and Equilibrium
Rate of Chemical Reactions starts at 10 and continues till grade 12.
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See sample questions for grade 11
Describe how temperature affects the rate constant (k) according to the Arrhenius equation.
Describe the difference between average rate and instantaneous rate of a reaction.
Explain how a catalyst affects the rate of a chemical reaction.
Explain why increasing the concentration of reactants generally increases the rate of reaction.
Explain why powdered zinc reacts faster with hydrochloric acid than a lump of zinc.
For a reaction: 2A → B, if the rate of formation of B is 0.05 mol L-1 s-1, what is the rate of disappearance of A?
For the reaction: 2NO2 → 2NO + O2, if the rate of disappearance of NO2 is 0.02 mol L-1 s-1, what is the rate of appearance of O2?
For the reaction: A + 2B → C, if the rate of disappearance of B is 0.04 mol L-1 s-1, what is the rate of disappearance of A?
If a reaction has a rate law Rate = k[A][B], what will happen to the rate if the concentration of A is doubled and B is kept constant?
If the concentration of a reactant is doubled and the rate of reaction increases four times, what is the order of the reaction with respect to that reactant?
State one reason why not all collisions between reactant molecules lead to a chemical reaction.
State the collision theory of chemical reactions.
The rate law for a reaction is Rate = k[A][B]2. What is the overall order of the reaction?
The rate law for a reaction is Rate = k[A]0. What does this indicate about the reaction?
The rate law for a reaction is Rate = k[A]1[B]0. If the concentration of B is doubled, what happens to the rate?
The rate of a reaction is 0.02 mol L-1 s-1 when the concentration of A is 0.1 mol L-1. If the reaction is first order in A, what will be the rate when [A] = 0.3 mol L-1?
A certain reaction is second order overall, first order in A and first order in B. If the concentration of both A and B are doubled, by what factor does the rate increase?
A reaction between X and Y is found to be first order with respect to X and zero order with respect to Y. If the initial concentration of X is 0.2 mol L-1 and that of Y is 0.5 mol L-1, write the rate law for the reaction and explain the significance of the order with respect to Y.
A reaction has a rate law Rate = k[A]1[B]2. If the concentration of A is halved and B is tripled, by what factor does the rate change?
Explain why the rate of a reaction generally decreases as the reaction proceeds.
