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 11
A reaction between hydrogen and oxygen is slow at room temperature but becomes explosive at high temperatures. Explain why.
A reaction has an activation energy of 50 kJ/mol. If a catalyst lowers the activation energy to 30 kJ/mol, what is the effect on the reaction rate?
A reaction is carried out at 25°C and then at 35°C. The rate of reaction increases. This is mainly due to:
A reaction mixture is heated from 20°C to 40°C. Predict the effect on the rate of reaction.
A student adds a catalyst to a reaction mixture. What change should they expect in the reaction rate?
Describe how the presence of a catalyst affects the activation energy of a reaction.
Describe the effect of increasing pressure on the rate of a reaction involving gaseous reactants.
Explain how temperature affects the rate of a chemical reaction.
Explain why increasing the concentration of a reactant increases the rate of reaction.
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.
If the surface area of a solid reactant is doubled, what happens to the rate of reaction?
In a reaction between two gases, doubling the pressure will have what effect on the rate of reaction?
A gaseous reaction is carried out in a closed container. Predict and explain the effect on the reaction rate if the volume of the container is halved, assuming temperature remains constant.
A reaction between two aqueous solutions is found to proceed much faster when the solutions are stirred vigorously. Explain why stirring affects the rate of reaction.
A student observes that a reaction between sodium thiosulfate and hydrochloric acid proceeds faster when the concentration of hydrochloric acid is doubled. Which factor affecting reaction rate does this observation illustrate?
Consider the decomposition of hydrogen peroxide (H2O2) in the presence and absence of manganese dioxide (MnO2) as a catalyst. Describe how the presence of MnO2 changes the reaction profile diagram and explain the effect on the rate of reaction.
Explain why the rate of a reaction generally decreases as the reaction proceeds, even if temperature and other conditions are kept constant.
The rate constant (k) for a reaction increases from 0.02 s-1 to 0.08 s-1 when the temperature is raised from 300 K to 320 K. Using the Arrhenius equation, explain what this indicates about the activation energy of the reaction.
