Reaction Quotient and Equilibrium Concepts

The video tutorial explains a reaction system in a one-liter vessel containing carbon monoxide, hydrogen gas, and methanol. It discusses how the total pressure changes as the system approaches equilibrium at constant temperature. The reaction involves carbon monoxide and hydrogen in a 1:2 ratio to form methanol, with an equilibrium constant of 14.5. The tutorial breaks down the problem into calculating the reaction quotient Q and comparing it with the equilibrium constant K to determine if the system is at equilibrium. Since Q is less than K, the reaction shifts to produce more products, reducing the total pressure as the system reaches equilibrium.

What are the initial moles of methanol gas in the reaction vessel?

• 1.5 moles

• 3.0 moles

• 1.2 moles

• 2.0 moles

What is the equilibrium constant (K) for the reaction at the given temperature?

• 16.5

• 10.5

• 14.5

• 12.5

How is the reaction quotient (Q) calculated for this reaction?

• Product of reactant concentrations

• Difference between product and reactant concentrations

• Sum of reactant concentrations

• Product concentration divided by reactant concentrations

What is the value of the reaction quotient (Q) calculated from the initial concentrations?

• 0.54

• 0.64

• 0.74

• 0.84

If Q is less than K, in which direction will the reaction shift?

• Towards the products

• Towards the reactants

• Towards equilibrium

• No shift

What does it mean if Q is less than K in terms of reactants and products?

• More products than reactants

• No reactants present

• More reactants than products

• Equal amounts of reactants and products

How does the shift towards products affect the total pressure in the system?

• No change in total pressure

• Fluctuates total pressure

• Increases total pressure

• Decreases total pressure

Why does the total pressure decrease as the reaction approaches equilibrium?

• More gas molecules are formed

• Fewer gas molecules are formed

• Temperature decreases

• Volume increases

What is the relationship between total pressure and moles of gas in the system?

• No relationship

• Exponentially related

• Inversely proportional

• Directly proportional

What happens to the number of gas molecules as the reaction shifts to favor the products?

• Remains the same

• Decreases

• Increases

• Doubles