Use LeChatelier’s principle to describe the effect on the equilibrium mixture (shift left, shift right, no shift) when the following reaction conditions are changed. N2 (g) + 3 H2 (g) ⇌ 2 NH3(g) H = - 22 kcal/mol a) Removing some NH3 (b) Decreasing the pressure (c) Decreasing the temperature (d) Adding some N2 (e) Add a catalyst
Use LeChatelier’s principle to describe the effect on the equilibrium mixture (shift left, shift right, no shift) when the following reaction conditions are changed.
N2 (g) + 3 H2 (g) ⇌ 2 NH3(g) H = - 22 kcal/mol
a) Removing some NH3
(b) Decreasing the pressure
(c) Decreasing the temperature
(d) Adding some N2
(e) Add a catalyst
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According to Le Chateliers principle, when an equilibrium system is disturbed by changing conditions, the equilibrium position will shift in a direction that reduces or cancels the change.
The reaction given is:
(a)
Given that some ammonia is being removed.
When ammonia is removed, system will try to increase the concentration of ammonia. Therefore, equilibrium will shift towards forward reaction (right ).
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