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Unit 18CP6
,In the graph above the Hydrogen is decreasing along with the Nitrogen but the Ammonia is
increasing which means that overall the equilibrium is achieved as a result of this. (Gevorg, 2022)
, In the Graph above, The Nitrogen Dioxide is increasing with time as the concentration also increases.
The Dinitrogen Tetroxide decreases with time as the concentration also decreases. (Khan Academy,
2017)
P7
Calculations involving Kc:
When the concentrations of reactants and products are in equilibrium, their ratio stays constant. The
equilibrium constant, or Kc, is the name given to this constant ratio. A given reaction's equilibrium
constant, or Kc, is found under predetermined parameters like pressure and temperature. Regarding
the relative concentrations of reactants and products at equilibrium, it offers useful information.
One can learn more about the nature of the equilibrium mixture and the magnitude of the response
by figuring out or measuring the equilibrium constant. It assists in forecasting how shifting situations
may affect the equilibrium state and enables us to comprehend the balance between the forward
and reverse reactions.
Kc = (products) / (Reactants)
Equilibrium A (the synthesis of methanol):
CO(g) + 2H2(g) CH3OH(g)
1) A rise in temperature tends to encourage the reaction's endothermic direction. The equilibrium
moves to the left, favouring the side that has more reactants as a result.
2) In contrast, the exothermic direction of the reaction is favoured by a drop-in temperature. As a
result, the balance shifts to the right, favouring the side with more goods.
3) The direction with fewer gas moles is usually favoured by a rise in pressure. As a result, the side
with more products gains momentum and the equilibrium moves to the left.
4) As the equilibrium shifts to the right, favouring the side with more reactants, a drop-in pressure,
on the other hand, tends to favour the direction with more gas moles.
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