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Reversible Reactions

The document discusses the principles of chemical equilibrium, focusing on the effects of concentration, temperature, pressure, and catalysts on the reaction N2 + 3H2 -> 2NH3. It explains how adding or removing reactants or products shifts the equilibrium to favor the forward or reverse reactions, and how temperature changes influence exothermic and endothermic reactions. Additionally, it highlights that while catalysts speed up the reaction rate, they do not alter the position of equilibrium or the yield of products.

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19 views3 pages

Reversible Reactions

The document discusses the principles of chemical equilibrium, focusing on the effects of concentration, temperature, pressure, and catalysts on the reaction N2 + 3H2 -> 2NH3. It explains how adding or removing reactants or products shifts the equilibrium to favor the forward or reverse reactions, and how temperature changes influence exothermic and endothermic reactions. Additionally, it highlights that while catalysts speed up the reaction rate, they do not alter the position of equilibrium or the yield of products.

Uploaded by

Swiftie
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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N2 + 3H2 -> 2NH3

Forward reverse
LHS RHS

LHS -> FAVOUR REVERSE -> MORE REACTANT


RHS -> FAVOUR FORWARD -> MORE REACTANT

Adding reactant
Wants to remove reactant
1.​ Equilibrium shifts to RHS
2.​ Favouring the forward reaction
3.​ More product formed
4.​ In order to minimise effect of increase in reactant concentration
Removing reactant
1.​ Equilibrium shifts to LHS
2.​ Favouring the reverse reaction
3.​ More reactants formed
4.​ In order to minimise effect of decrease in reactant concentration

Adding Product
1.​ Equilibrium shifts to LHS
2.​ Favouring reverse reaction
3.​ More reactant formed
4.​ In order to minimise effect of increasing product concentration

Removing Product
1.​ Equilibrium shifts to RHS
2.​ Favoruing forward reaction
3.​ More product formed
4.​ In order to minimise effect of decrease in product concentration

Increasing Ammonia yield


-​ Add reactant
-​ Remove NH3

Temperature
-​ LEX -> low exo
-​ HEN -> high endo
-​ Negative enthalpy -> exothermic
-​ If forward exo, reverse automatically endo

EXOTHERMIC:
Decrease Temp:
-​ Favour forward reaction
-​ To product more heat as forward is exo
-​ Equilibrium to RHS
-​ More product formed

Increase Temp:
-​ Favour reverse to reduce heat as reverse is endo
-​ Equilibrium to LHS
-​ More reactants formed

ENDOTHERMIC
Increase temp:
-​ Forward reaction favour to consume added heat as forward is endo
-​ Equilibrium to RHS
-​ More product formed

Decrease Temp:
-​ Favours reverse reaction to produce more heat, as reverse in exo
-​ Equilibrium the LHS
-​ More reactants formed

Pressure
Moles is proportional for no of particles
N x 6.02 x 10 23 -> no. of particles
As moles increase, particles increas so pressure increases

Increase in pressure
-​ Equilibrium shifts to side having less moles
-​ To minimise effect of increase in pressure

Decrease in pressure:
-​ Equilibrium shifts to side having more moles
-​ To minimise effect of pressure decrease

1.​ Equilibrium shifts to ()


2.​ Favours () reaction
3.​ Bc there are () no of moles
4.​ More () formed

Eg. decreasein pressure for N2 + 3H2 -> 2NH3


-​ Equilibrium shafts to side with more moles
-​ Equilibrium shifts to LHS
-​ Favouring reverse reaction
-​ More reactant formed
Catalyst:
Position of equilibrium is not changed but only
the rate of the reaction increases. Equilibrium
can be achieved faster. Yield doesn’t increase.

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