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Making ammonia (2) 3.5
Terms in this set (12)
Why do the reaction conditions of the Haber process have to be chosen carefully?
to produce a reasonable yield of ammonia quickly
What are important when determining the optimum conditions in industrial processes?
the factors that effect equilibrium
Is the forward reaction to produce ammonia exothermic or endothermic?
What does using a low temperature produce?
increased yield slowly
In the gaseous reactions, what will an increase in pressure favour?
the reactions that produces the lowest number of molecules
the right hand side- increases the yield of ammonia
What are the negatives of using high-pressure reactors?(3)
expensive to make
increase the risk of explosion
require a high energy input
Why are reaction rates important? (2)
they effect the equilibrium position
they determine the optimum conditions in industrial processes
In the Haber process, how are optimum conditions to produce a reasonable yield of ammonia quickly achieved? (3)
a catalyst to speed up the reaction
high pressure drives the equilibrium forwards, but not so high that it is expensive etc
low temp- increase the yield but make reaction too slow- chosen pressure and temperature is a compromise
What is it important to do for sustainable development and economic reasons? (2)
minimise energy requirements
minimise energy wasted
Why does the Haber process use large amounts of energy?
due to the high temperature and pressure conditions
In other industrial processes, what does using low pressure and temperature conditions (non-vigorous) result in? (2)
less energy used
less energy released to the environment
What does running processes sustainably include? (3)
recycling unused reactants back into the process
converting waste products into useful materials
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