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Preface
We want:
- High yield (large % of products compared to reactants)
- Fast rate of attainment of desired product(do we say equi? good q for teacher :))
- Safety and product considerations
Rate:
- High temperature
- High pressure (for gasses)(higher concentration of reactants)
- Use suitable catalyst (as is not consumed in reaction, i.e. free money)
Yield:
- Le Chatelier
- e.g. Exo reaction favoured by low temperature - this is a contradiction, hence we need to find a compromise.
- Gasses
- $Low \ mol \rightleftharpoons High \ mol$
- Forward favoured by low pressure
- Also a contradiction
Contact process and Haber process are important for assessments.
We won't need to know like how the factory is structured, none of that non-chem stuff >:(
BUT: We must remember key details
Haber Process
$N_{2(g)}+3H_{2(g)}\rightleftharpoons 2NH_{3(g)} \ \ \Delta H= -92kJ$
(To get high x):
- Rate
- High pressure (lots of $N_{2}$ and $H_{2}$ per unit volume)
- High temperature
- Catalyst (for haber process, we use an iron oxide! ($Fe_{2}O_{3}$ OR $Fe_{3}O_{4}$))
- Yield
- High pressure (Reaction moles: 4 moles $\to$ 2 moles, so forward reaction favoured)
- Low temperature - because reaction is exothermic
- Catalyst (same as before)
Conditions:
- High pressure (Not to high, cause of safety and operation costs)
- Temperature will have to be a compromise
- $350 \degree C - 550 \degree C$
- Reasonable rate and yield
- If the temperature is too low, the rate is too small.
- If the temperature is too high, the yield is too low, i.e. we don't produce as much $NH_{3}$. Not poggies.
- We remove $NH_{3}$ as reaction proceeds
- This means $NH_{3}$ is constantly being removed as it is produced, i.e. we are preventing the system from reaching equilibrium so the forward reaction is favoured
- See Le Chat prediction when we reduce concentration of product
- Even though it never reaches equilibrium, the yield argument still holds!!
- Dunno why it wouldn't but Norrie said so so it must be true
Contact Process
A method of manufacturing sulfuric acid
Luckily, we consume $SO_{2}$, which is a stinky greenhouse gas. Good stuff.
This process is used to capture $SO_{2}$ and fix climate change!! WOo!!! (also sulfuric acid good product)
Factors increasing rate:
- High temperature
- High pressure
- Catalyst
Factors increasing yield:
- Lower temperature, because the reaction is exothermic.
- High pressure
i.e. same arguments as the Haber process!
Conditions: