Question

( HELP) The following system is at equilibrium. In which direction (right or left) will the equilibrium position shift with the following changes?
3NO(g) <--> N2O(g) + NO2(g) + 154.9 kJ
(right, left, or no effect)

a) Lowering the temperature?

b) Raising the temperature?

c) Adding more N2O?

d) Adding more NO?

e) Removing some N2O?

f) Adding a catalyst?

g) Increasing the volume

Answer 1

a) right

b) left

c) left

d) right

e) right

f) no effect

d) left

Explanation:

We have the following chemical reaction:

3 NO (g) ⇔ N₂O (g) + NO₂ (g) + 154.9 kJ

a) right, because by lowering the temperature you remove the heat generated by the reaction, and the reaction is able to generate more heat with the reaction proceeding from left to right.

b) left, because by increasing the temperature you add heat to the reaction and by doing so the reaction from right to left will be promoted.

c) left, increasing the concentration of N₂O the equilibrium will shift to left in order to consume the N₂O added.

d) right, increasing the concentration of NO the equilibrium will shift to right in order to consume the NO added.

e) right, decreasing the concentration of N₂O the equilibrium will shift to right in order to produce the removed N₂O.

f) no effect, adding a catalyst will not shift the equilibrium position, it will only modify the time in which the equilibrium is achieved and the energy required to achieve the equilibrium state.

g) left, by increasing the volume the equilibrium will shift to the part where more moles are produced (there are 3 moles on left side while in the right side there are 2 moles).

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Le Chatelier Principle

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