SC12 - Reversible Reactions and Equilibria ✓ Flashcards
SC12a - What is a reversible reaction?
A reaction where the products can react again to reform the reactants
SC12a - What symbol would show that a reaction is reversible?
⇌ : The double arrow
SC12a - In a reversible reaction how does the speed of the forward reaction and backward reaction change over time?
- The forward reaction starts fast and gets slower over time.
- The backward reaction starts slow and gets faster over time.
SC12a - Define Dynamic Equilibrium
This is when the forward and backward reactions are occuring at the same rate, therefore the percentage of products and reactants remain the same
SC12a - What happens to the amount of products and reactants produced once a reaction has reached Dynamic Equilibrium?
They stop changing (increasing or decreasing)
SC12a - What is required for Dynamic Equilibrium to be achieved, and why?
- A closed system.
- In an open system fluids can escape and equilibrium cannot be reached
SC12a - What is the name and the chemical formula of the process that creates ammonia?
- The Haber Process:
- N2(g) + 3H2(g) ⇌ 2NH3(g)
SC12a - What is the temperature, pressure and catalyst used during the Harber Process?
- T: 450°
- P: 200 Atmospheres (atm)
- C: Iron Catalyst
SC12a - What happens to the position of equilibrium if you increase/decrease temperature?
- Increase - shifts in the endothermic direction
- Decrease - shifts in the exothermic direction
SC12a - What happens to the position of equilibrium when you decrease/increase gas pressure?
Increase - shifts in the direction that formers fewer molecules (to reduce pressure)
Decrease - shifts in the direction the forms more gas molecules (to increase pressure)
SC12a - What happens to the position of equilibrium when you decrease/increase a concentration?
- Increase - shifts in the direction that uses up the substance added
- Decrease - shifts in the direction that forms more of the substance that was removed
