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Unit 18C - Industrial Chemical Reactions - distinction received

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  • May 6, 2022
  • 7
  • 2021/2022
  • Essay
  • Unknown
  • A+

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  • unit
  • unit 18
  • 18c
  • unit 18c
  • applied
  • science
  • applied science
  • industrial
  • chemical
  • reactions
  • unit 18c industrial chemical reactions
  • industrial chemical reactions

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  • PEARSON (PEARSON)
  • Applied Science 2016 NQF
  • Unit 18 - Industrial Chemical Reactions
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Unit 18C: Industrial Chemical Reactions – C: Investigate chemical equilibrium in
order to understand the extent to which reactions go to completion

Equilibrium refers to a situation in which the reactants can form products,
but the products can also reform the reactants. The equilibrium sign in
the equation is used to show these reactions. It is a process in which the
reactants form products, but the products can also reform the reactants,
and this is known as equilibrium. An equilibrium symbol in the equation
depicts these reactions O Chemical equilibria is a delicate process which
stabilises itself into a predetermined concentration if the concentrations of
the reactants and products do not fluctuate.

For e.9. H2(g) + 12(g) - 2HI(g)

Chemical equilibrium is a fine process that will stabilise itself into set
concentrations if the concentrations of the reactants and products do not
change.

Dynamic equilibrium

If the container is sealed, dynamic equilibrium can be achieved. This will
allow the reactants and products to stabilise and maintain the same
concentration. At this point, the forward reaction rate will equal the
backward reaction rate. The equilibrium position will be set if the
container is sealed. The equilibrium position is determined by the
reaction. It could be in the direction of reactants or products. The
equilibrium constant is the value for the position of the equilibrium.

Le Chateliers Principle

The principle states that if the conditions of a dynamic equilibrium are
changed, the position of equilibrium shifts to compensate for the change
and re-establish equilibrium. If a dynamic equilibrium is disturbed by
altering the circumstances, the position of equilibrium shifts to
compensate for the change and restore an equilibrium, according to Le
Chatelier's Principle. (“What is Le Chateliers principal class 11 chemistry
CBSE”)


What happens to equilibrium when you change temperature,
concentration, pressure and add a catalyst?

Different conditions can change the equilibrium position.
When we change the temperature, concentration, or pressure, we can
affect the equilibrium and thus the concentrations of the reactants and
products. We can change the rate at which equilibrium is reached with a
catalyst, but not the final concentrations of reactants and products. An
equilibrium reaction's enthalpy changes aids in determining how high the

, temperature can be raised. When the temperature changes, equilibrium
reactions can be either exothermic or endothermic, and they will move in
one of two directions. Raising the temperature will allow the reaction to
move to the reactants if it is exothermic (AH is negative) (left). You'll
need to lower the temperature in these reactions to make more products.
If the reaction is endothermic (AH is positive), increasing the temperature
will cause it to migrate to the right side of the products, producing more
of what you need. Raising or lowering the concentration may affect the
location of equilibrium as the reaction adjusts to clear excess
concentrations. More products are produced when the concentration of
reactants is increased to reduce the excess concentration. On the other
hand, increasing the concentration of products shifts the equilibrium back
to the reactants. When it comes to industry, clearing items as soon as
they're generated will reduce their concentration. As a result, the
equilibrium shifts to the right, resulting in the formation of more products
to replace those that have been lost. Even though gases are present in
many equilibrium reactions, pressure can be used to change
concentrations. The chemical molar rations determine how the equilibrium
shifts as pressure changes. Raising the pressure causes the equilibrium to
shift towards the products when there are more reactants than products.
The amount of pressure and volume taken up by the reactants and
products will be reduced as a result. When the pressure is increased, the
equilibrium will shift to the reactants if the moles of product are greater
than the moles of reactants. As a result of lowering the pressure, you will
be able to produce more items. An equilibrium's goal is to reduce the
amount of energy required for a reaction to occur, allowing the process to
proceed more quickly. This is true in all reactions. In an equilibrium
reaction, there are two reactions. Products reactants and reactants
products. Each of these reactions has an activation energy, and using a
catalyst lowers the activation energy for both. As a result, the time it
takes to reach equilibrium increases, but the equilibrium position remains
unchanged.

What is Kc?

Kc stands for the equilibrium constant. When a reaction reaches dynamic
equilibrium, Kc indicates how far it has progressed.
When the reactants and products are in a fine balance, equilibrium
reactions occur.

What is the relationship between equilibrium and Kc?

Kc could be greater or lesser than 1 depending on the equilibrium
position. If the equilibrium position is towards the products, Kc will be
greater than 1. If equilibrium is toward the reactants, Kc will be less than
1. The equilibrium between the reactants and products will be precise if
the value of Kc is exact. When the Kc is less than 1, the equilibrium will

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