Chemistry 10.4.3 Flashcards
A Higher Temperature of the Surroundings would Favour the ___ Reaction, as it is ___. So a ___ Yield of Reactants would be Made, as Energy is Being ___. Subsequently, the ROR ___.
Reverse, Endothermic, Higher, Gained, Increases.
A Lower Temperature of the Surroundings would Favour the ___ Reaction, as it is ___. So a ___ Yield of Reactant would be Made, as Energy is Being ___. Subsequently, the ROR ___.
Forward, Exothermic, Lower, Lost, Decreases.
Why is 450’C Used in the Haber Process?
It is a Cheap Compromise so that there is a Good Yield of Ammonia & a Good Rate of Reaction.
A Lower Pressure would Favour the ___ Reaction, as the System will Try to ___ the Pressure by Creating ___ Molecules. So a Higher Yield of ___ will be Made.
Reverse, Increase, More, Reactants.
A Higher Pressure would Favour the ___ Reaction, as the System will Try to ___ the Pressure by Creating ___ Molecules. So a Higher Yield of ___ will be Made.
Forward, Decrease, Fewer, Products.
Why is 200atm Used in the Haber Process?
It is a Compromise for a Good Yield, & Safety.
What is the Problem with Using too High Pressure in the Haber Process?
It will Explode.
What is the Problem with Using too High Temperature in the Haber Process?
It is too Expensive.
What is the Problem with Using too Little Pressure in the Haber Process?
Reaction will not Favour Forward Reaction, which Produces Ammonia, which is the Desired Product here.
What is the Problem with Using too Little Temperature in the Haber Process?
ROR will be too Low.
The Presence of a Catalyst ___ Affect the Position of Equilibrium, but it does ___ the Rate at which Equilibrium is Reached.
Doesn’t, Increase.
