Here is an equilibrium: C (s) + CO₂ (g) $⇌$ 2 CO (g) [ΔH⁰_rxn = 65 kJ]
Predict and explain the direction that the equilibrium will shift when each of the following changes occurs:
- CO is removed at constant temperature
- the total pressure is increased by addition of N₂ (g) at constant temperature
- the volume is increased at constant temperature
- the temperature is decreased

Question

Here is an equilibrium: C (s) + CO₂ (g)

⇌

2 CO (g) [ΔH⁰_rxn = 65 kJ]

Predict and explain the direction that the equilibrium will shift when each of the following changes occurs:

- CO is removed at constant temperature

- the total pressure is increased by addition of N₂ (g) at constant temperature

- the volume is increased at constant temperature

- the temperature is decreased

| General Chemistry 3

Accepted Answer

- CO is removed at constant temperature:

direction: toward product

explanation: when product is removed, the reaction shifts to make more product (Le Chatelier’s principle)

- the total pressure is increased by addition of N₂ (g) at constant temperature

direction: no change

explanation: volume did not change à partial pressure did not change à Q did not change à no shift

- the volume is increased at constant temperature

direction: toward product

explanation: side with most moles of gas

- the temperature is decreased

direction: toward reactants

explanation: reaction is endothermic

Midterm 1 - Question 1 | General Chemistry 3