Unit 3 AOS 2 - Reaction Rates Quiz (1)

What are the four main factors that can affect the rate of a chemical reaction?

• Amount of light, type of reactants, type of catalyst, and type of gas produced

• Color of the reactants, pressure, time of day, and volume of the container

• Type of container, smell of the reactants, pH level, and type of solvent

• Temperature, concentration of reactants, surface area, and presence of a catalyst

How does surface area affect the rate of a chemical reaction?

• Increasing surface area decreases the rate of a chemical reaction

• Surface area only affects the color of the reactants

• Surface area has no effect on the rate of a chemical reaction

• Surface area affects the rate of a chemical reaction by providing more area for the reactant molecules to come into contact with each other.

According to collision theory, what is necessary for a successful collision to occur between reactant particles?

• Random orientation and low energy

• High pressure and low temperature

• Proper orientation and enough energy

• Low pressure and high temperature

Explain how the activation energy relates to the collision theory of reaction rates.

• The activation energy is the maximum amount of energy required for a reaction to occur, according to collision theory.

• The activation energy has no relation to the collision theory of reaction rates.

• The activation energy is the minimum amount of energy required for a reaction to occur, according to collision theory.

• The activation energy is the average amount of energy required for a reaction to occur, according to collision theory.

How does an increase in temperature affect the rate of a chemical reaction?

• Becomes solid

• Stays the same

• Decreases

• Increases

What is the effect of a catalyst on the reaction rate at a molecular level?

• Decreases the reaction rate by increasing the activation energy

• Has no effect on the reaction rate

• Increases the reaction rate by providing an alternative pathway with lower activation energy.

• Stops the reaction from occurring

How does the transition state theory explain the formation of products in a chemical reaction?

• The transition state theory states that the reactant molecules must overcome an energy barrier to form products, and this barrier is the transition state.

• The transition state theory states that the energy barrier for forming products is lower than the energy barrier for the reactants.

• The transition state theory states that the reactant molecules do not need to overcome any energy barrier to form products.

• The transition state theory states that the formation of products is not influenced by the energy barrier.

Explain the concept of activation energy and its role in determining the reaction rate.

• Activation energy is the maximum amount of energy required for a chemical reaction to occur and it slows down the reaction rate.

• Activation energy is the average amount of energy required for a chemical reaction to occur and it has no effect on the reaction rate.

• Activation energy is the energy released during a chemical reaction and it has no impact on the reaction rate.

• Activation energy is the minimum amount of energy required for a chemical reaction to occur and it influences the likelihood of successful collisions between reactant molecules.

How can the reaction rate be calculated using the change in concentration of reactants over time?

• By counting the number of products formed

• By determining the change in concentration of reactants over time.

• By analyzing the color of the reactants

• By measuring the temperature of the reaction

What is the formula for calculating the reaction rate using the initial and final concentrations of reactants?

• Rate = (Final concentration of reactants) / (Time)

• Rate = (Change in concentration of products) / (Time)

• Rate = (Change in concentration of reactants) / (Time)

• Rate = (Initial concentration of reactants) / (Time)