Factors Affecting Reaction Rate
Chemistry ⇒ Chemical Kinetics and Equilibrium
Factors Affecting Reaction Rate starts at 10 and continues till grade 12.
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See sample questions for grade 12
A reaction between a gas and a solid is found to proceed faster when the solid is finely powdered. Explain why.
A reaction between hydrogen and chlorine is carried out in the presence of light. What role does light play in this reaction?
A reaction has a rate constant k = 0.02 s-1 at 300 K and k = 0.08 s-1 at 320 K. What factor is responsible for the increase in k?
A reaction is carried out at 25°C and then at 35°C. The rate constant increases. What factor is responsible for this change?
Describe how the presence of a catalyst affects the rate of a reaction without being consumed.
Describe the effect of a catalyst on the activation energy of a reaction.
Describe the effect of increasing the concentration of a reactant on the rate of a reaction.
Explain how stirring affects the rate of a reaction between two liquids.
Explain how temperature affects the rate of a chemical reaction.
Explain why increasing the pressure increases the rate of reaction for gases but not for solids or liquids.
Explain why powdered zinc reacts faster with hydrochloric acid than a lump of zinc.
Explain why reactions between ions in aqueous solution are usually very fast.
Explain why reactions involving covalent bonds are generally slower than those involving ionic bonds.
A certain reaction is zero order with respect to reactant A. If the concentration of A is doubled, what happens to the rate of the reaction?
A reaction between two gases, A and B, is found to double its rate when the total pressure is doubled at constant temperature. Explain why this occurs, and under what conditions this relationship would not hold.
Consider the following reaction: 2NO(g) + O2(g) → 2NO2(g). Predict and explain the effect on the reaction rate if the volume of the reaction vessel is halved at constant temperature.
Explain why increasing the ionic strength of a solution can affect the rate of a reaction between two oppositely charged ions.
The rate constant (k) of a reaction increases from 1.5 × 10-3 s-1 to 6.0 × 10-3 s-1 when the temperature is raised from 300 K to 320 K. Using the Arrhenius equation, calculate the activation energy (Ea) for the reaction. (R = 8.314 J mol-1 K-1)
The rate of a reaction is given by rate = k[X][Y]2. If the concentration of X is halved and the concentration of Y is doubled, by what factor does the rate change?
