hahaha my bad sorry.
Evaluate the importance of monitoring and managing the conditions used in the Haber process. - 7 marks
Pretty decent question, but marking criteria i would assume wants top-notch detail lol
I'd expect 3-4 marks for that, they must want ridiculous detail (which I won't be giving since this isn't my actual HSC)
Marked fluctuations in the conditions under which the Haber Process takes place (450-500 degrees Celsius and 200 atmospheres pressure) is not favourable for the following reasons:
TEMPERATURE
- decrease: causes the reaction to proceed more slowly, thus renders the process less economically viable
- increase: the reaction N2 + 3H2 ----> 2NH3 is exothermic. Therefore, as temperature is increased the position of the equilibrium shifts more to the left to minimise the disturbance in accordance with Le Chatelier's Principle, thus reforming reactants instead of creating more product (ammonia). As the goal of the Haber process is to synthesise ammonia, this is not desirable
PRESSURE
- decrease: the Haber Process involves four moles of reactants combining to form two moles of products. Thus, high pressure favours the formation of products (ammonia) in order to relieve this pressure. Thus, decreasing pressure leads to a decrease in ammonia yield, which is not desirable.
- increase: sustaining a very high pressure is cost intensive, thus a marked increase in temperature can cause the process to become economically inefficient, as production cost may exceed the cost of the product to the market.
Thus it is highly important to ensure these conditions are strictly monitored in order to promote financial efficiency and high ammonia yield.