Equilibria and Redox Reactions

Question 1

What is Dynamic Equilibrium?

Question 2

Conditions for dynamic equilibrium

Answer 2

Closed System
Constant Temperature
Constant Pressure
Forward reaction and backward reaction happening at same rate

Question 3

2HI (g) -><- H2 (g) + I2 (g)
What happens to this equilibrium if pressure is increased?

Answer 3

Shift right

Question 4

2HI (g) -><- H2 (g) + I2 (g)
What happens to this equilibrium if pressure is decreased?

Answer 4

Shift left

Question 5

2HI (g) -><- H2 (g) + I2 (g)
What happens to this equilibrium if concentration of HI is increased?

Answer 5

Shift right

Question 6

2HI (g) -><- H2 (g) + I2 (g)
What happens to this equilibrium if concentration of H2 is increased?

Answer 6

Shift left

Question 7

2SO2 (g) + O2 (g) -><- 2SO3 (g) (delta)H = -197 kJ mol-1
What happens to this equilibrium if Temperature is increased?

Answer 7

Shift left

Question 8

2SO2 (g) + O2 (g) -><- 2SO3 (g) (delta)H = -197 kJ mol-1
What happens to this equilibrium if Temperature is decreased?

Answer 8

Shift right

Question 9

Why are conditions compromised in industry?

Answer 9

They take into account cost and increasing yield of the desired product

Question 10

What factors need to be taken into account for production in industry?

Answer 10

Use of a catalyst
Temperature
Pressure

Question 11

aA + bB -><- dD + cC
What is the equilibrium constant for this reaction?

Answer 11

Kc = [D]^d [E]^e / [A]^a [B]^b

Question 12

The factors affecting Equilibrium Constant (Kc)

Answer 12

Temperature

Question 13

Definition of Oxidation

Answer 13

Loss of electrons

Question 14

Definition of Reduction

Answer 14

Gain of electrons

Question 15

What does an Oxidising agent do?

Answer 15

Accepts electrons and gets reduced

Question 16

What does a Reducing agent do?

Answer 16

Donates electrons and gets oxidised

Question 17

Definition of Oxidation state

Answer 17

Shows the total number of electrons an element has donated or accepted