Chemical Equilibrium and Gas Laws

The video tutorial explains a heterogeneous reaction involving a solid and a gas, aiming to find the equilibrium composition at 1.0-bar and 25°C. It covers calculating the equilibrium constant using Delta G, determining the extent of reaction, and calculating mol fractions. The tutorial also demonstrates solving a non-linear equation using PolyMath and performing final checks on mol fractions and saturation pressure.

What is the initial amount of carbon used in the reaction?

• 5 mols

• 10 mols

• 20 mols

• 15 mols

How is the equilibrium constant calculated in this reaction?

• Using the initial amounts of reactants

• Using the temperature and pressure directly

• From the Delta G of formation of reactants and products

• By measuring the final concentrations

Why are mol fractions important in this calculation?

• They determine the color of the gas

• They are used to calculate partial pressures

• They indicate the reaction speed

• They show the temperature change

What assumption is made about the gases in this reaction?

• They are liquid at room temperature

• They are non-ideal gases

• They are ideal gases

• They are solid at high pressure

What tool is used to solve the non-linear equation in this example?

• Excel

• PolyMath

• MATLAB

• Python

What is the extent of reaction calculated using PolyMath?

• 0.15

• 0.12

• 0.20

• 0.18

Why is it important to check the saturation pressure of hexane?

• To determine the color of the gas

• To verify no liquid condenses

• To measure the reaction speed

• To ensure the reaction is complete

What is the saturation pressure of hexane at 25°C?

• 0.061 bar

• 0.5 bar

• 0.1 bar

• 1.0 bar

What is the main reason for calculating the number of mols of carbon at equilibrium?

• To check if all carbon is used up

• To find the temperature change

• To determine the color of the gas

• To measure the reaction speed

What does a small equilibrium constant indicate about the reaction?

• The reaction has a small extent

• The reaction is slow

• The reaction has a large extent

• The reaction is fast