Equilibria 2

Question 1

Kc

Answer 1

Ratio of product concentration to reactant concentration
Constant for a given temperature

Question 2

Total pressure

Answer 2

Sum of all the partial pressures of the individual gases
The greater the number of moles of a gas, the greater it’s partial pressure

Question 3

Partial pressure equation

Answer 3

Mole fraction x pressure

Question 4

Heterogenous equilibria

Answer 4

Kc- dont include solids or pure liquids as these concentrations stay constant
Kp- only include gases

Question 5

Effect of increasing temperature on the equilibrium constant

Answer 5

Exothermic reaction- causes k to decrease because increasing temperature favours endothermic reaction, in this case this would be the backwards reaction and therefore produces more reactants
Endothermic reaction- k increases (same reasoning)

Question 6

Effect of decreasing temperature on equilibrium constant

Answer 6

Exothermic- k increases
Endothermic- k decreases

Question 7

Rules for changing temperature

Answer 7

If it causes less product to form, equilibria has moved to the left and k decreases
Vide verse

Question 8

Effect of concentration on equilibrium constant

Answer 8

Equilibrium constant is fixed at a constant temperature
If the concentration of one thing changes then the concentrations of the others must change to keep the values of kc the same
When a concentration changes, Qc no longer equal to Kc and the composition of equilibrium changes until they’re equal again

Question 9

Effect of pressure on equilibrium constant

Answer 9

Same as in concentration

Question 10

Kp

Answer 10

Describes the state of equilibrium with respect to the partial pressures exerted by the reactants and products