Reaction Rates and Equilibrium Concepts

The video tutorial explains the process of a chemical reaction, focusing on how reactants decrease and products increase over time. It highlights the concept of reaction rates, showing how they are represented by the gradient of a graph. The tutorial discusses irreversible reactions, where reactants convert to products without reversing. Initially, the reaction rate is high due to abundant reactants, but it decreases as products form, leading to fewer reactant collisions. Eventually, the reaction rate becomes zero when reactants are fully converted.

What happens to the concentration of reactants as a reaction progresses?

• It remains constant.

• It increases.

• It decreases.

• It fluctuates randomly.

What does a steep gradient on a reaction graph indicate?

• A constant reaction rate.

• No change in reaction rate.

• A high reaction rate.

• A low reaction rate.

What is the relationship between reactant concentration and reaction rate at the start of a reaction?

• Higher reactant concentration leads to a lower reaction rate.

• Reactant concentration and reaction rate are inversely proportional.

• Higher reactant concentration leads to a higher reaction rate.

• Reactant concentration does not affect reaction rate.

In an irreversible reaction, what is the direction of the reaction?

• It does not proceed at all.

• It proceeds to the left.

• It proceeds to the right.

• It can proceed in both directions.

What is the focus of the section on equilibrium?

• Dynamic reactions.

• Irreversible reactions.

• Static reactions.

• Reversible reactions.

What happens to the reaction rate as more products are formed?

• It remains the same.

• It increases.

• It becomes unpredictable.

• It decreases.

Why does the reaction rate decrease over time?

• Because products are increasing.

• Because reactants are increasing.

• Because products are decreasing.

• Because reactants are decreasing.

When does the reaction rate become zero?

• When all reactants are consumed.

• When the reaction is reversible.

• When all products are consumed.

• When the reaction starts.

What happens to reactants when they collide with products?

• They stop reacting.

• They remain unchanged.

• They form new products.

• They form new reactants.

What does it mean when the amount of product doesn't change over time?

• The reaction is at its peak.

• The reaction is still proceeding.

• The reaction rate is zero.

• The reaction is reversible.