For the exothermic reaction 3H2(g) + N2(g) 2NH3(g) which of the following changes could be carried?
raising the temperature and removing NH3
lowering the temperature and adding NH3
both (a) and (b)
neither (a) nor (b)
Answer:
Any of the answers could be correct, depending on exactly how much of each is done.
For example, with the first option:
exothermic, heat in, reaction moves to the left
remove product, reaction moves to the right
appropriate balance - no net movement - could be found.
Same corollary for (b)
However, what do you really mean by "cause the reaction to shift to the left or to the right?"
As an equilibrium, both the forward and reverse reactions are occuring at equal rates.
Higher temperature favors the more disordered side of a reaction. That's the side with more moles of gas (the left).
Removing NH3 shifts the reaction toward the right.
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