Chemical Equilibruim

Question 1

Define the term dynamic equilibrium

Answer 1

The rate of the forward reaction is equal to the rate of the reverse reaction

Question 2

Give an essential condition for an equilibrium mixture

Answer 2

Equilibrium occurs in a closed system ( where reactants and products cannot escape )

Question 3

State the Le Chatelier’s principle

Answer 3

If a system at equilibrium is disturbed the equilibrium moves in the direction that tends to reduce the the disturbance ( the side of higher moles )

Question 4

In the equation
CH4 +H2O -> CO + 3H
What effect would increasing the temperature have on the position of equilibrium?

Answer 4

The equilibrium position shifts to the right

Question 5

In this equation
CH4 + H2O -> CO + 3H2
What effect would increasing the pressure have on the position of equilibrium?

Answer 5

The equilibrium position shifts to the left ( as the yield doesn’t match the amount of reactants thus to balance it out )

Question 6

CH4 + H2O -> 3H2
Suggest and explain why an industrial chemist may use a high pressure for this production of hydrogen from the above reaction ?

Answer 6

1. The high pressure increases the collision frequency increasing the rate of reaction
2. This is a compromise pressure between an economically viable rate of reaction and a slightly lower yield of hydrogen

Question 7

What effect does a catalyst have on the position of equilibrium?

Answer 7

No effect ( as catalyst effect both forward and backward reaction equally )

Question 8

What condition affects the value of Kc ?

Answer 8

Temperature