Chemical Equilibrium Concepts

This lesson introduces equilibrium graphs, focusing on the initial conditions of nitrogen and hydrogen in a reaction. It explains how concentrations change as the reaction progresses, with the forward reaction initially being fast due to high reactant availability. As the reaction proceeds, the forward rate decreases while the reverse rate increases, eventually reaching equilibrium where both rates are equal. At equilibrium, concentrations remain constant, and the graph lines become parallel. The lesson concludes with a summary and a preview of the next video, which will explore how the system responds to disturbances.

What are the initial reactants in the equilibrium graph discussed in the lesson?

• Ammonia and Nitrogen

• Nitrogen and Hydrogen

• Hydrogen and Oxygen

• Nitrogen and Oxygen

As the reaction progresses, what happens to the concentration of nitrogen and hydrogen?

• It increases

• It remains constant

• It decreases

• It fluctuates

What happens to the concentration of the product as the reaction proceeds?

• It disappears

• It increases

• It remains constant

• It decreases

Why is the forward reaction initially very fast?

• Because the temperature is high

• Because there are many molecules available to collide

• Because the volume is large

• Because the pressure is low

What causes the reverse reaction to start increasing in speed?

• Decrease in temperature

• Increase in pressure

• Formation of products

• Decrease in volume

At equilibrium, what is true about the forward and reverse reactions?

• Both reactions occur at the same rate

• Both reactions stop

• The reverse reaction is faster

• The forward reaction is faster

What happens to the concentrations of reactants and products at equilibrium?

• They fluctuate

• They decrease

• They increase

• They stay constant

What is the main takeaway regarding the initial state of the reaction?

• The reaction is at equilibrium

• There is a mixture of reactants and products

• There are only reactants present

• There are only products present

What is the significance of the lines becoming parallel on the concentration graph?

• The reaction is accelerating

• The reaction is at equilibrium

• The reaction has stopped

• The reaction is reversing

What will be discussed in the next lesson?

• Introduction to new reactants

• Decreasing the reaction rate

• Disturbing the equilibrium system

• Increasing the reaction rate