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Created page with "==Key Stage 4 Higher== ===Meaning=== '''Equilibrium position''' is the the ratio of reactants to products when a reversible reaction is in..."
==Key Stage 4 Higher==
===Meaning===
'''Equilibrium position''' is the the [[ratio]] of [[reactant]]s to [[product]]s when a [[Reversible Reaction|reversible reaction]] is in a state of [[Dynamic Equilibrium|dynamic equilibrium]].
===About the Equilibrium Position===
: The '''equilibrium position''' can be affected by the [[temperature]] and by the [[Gas Pressure|pressure]].
=====Temperature and Equilibrium Position=====
: An increase in [[temperature]] will increase the [[Rate of Reaction|rate]] of an [[endothermic]] [[Chemical Reaction|reaction]] it requires [[energy]] from the environment to take place.
: This means for an [[endothermic]] forward [[Chemical Reaction|reaction]] a higher [[temperature]] will result in more [[product]] being formed. However, for an [[exothermic]] forward [[Chemical Reaction|reaction]] less product will be formed as the back [[Chemical Reaction|reaction]] will be [[endothermic]] and would increase its [[Rate of Reaction|rate]] with higher [[temperature]].
=====Pressure and Equilibrium Position=====
: For [[reaction]]s involving a [[gas]] as either one of the [[reactant]]s or [[product]]s changing the pressure will affect the position of '''dynamic equilibrium'''.
: The number of [[mole]]s of [[gas]] in the [[reactant]]s and [[product]]s will determine which direction of [[Chemical Reaction|reaction]] is favoured by higher [[Gas Pressure|pressure]].
: If the forward [[Chemical Reaction|reaction]] [[product|produces]] more [[mole]]s of [[gas]] than the back [[Chemical Reaction|reaction]] then high [[Gas Pressure|pressure]] will reduce the amount of [[product]]s formed.
: If the forward [[Chemical Reaction|reaction]] [[product|produces]] less [[mole]]s of [[gas]] than the back [[Chemical Reaction|reaction]] then high [[Gas Pressure|pressure]] will increase the amount of [[product]]s formed.
===Examples===
Hydrogen + Nitrogen ⇌ Ammonia
<chem> 3H2(g) + N2(g) <=> 2NH3(g) </chem>
: In this [[Reversible Reaction|reversible reaction]] there are more [[mole]]s of [[gas]] in the [[reactant]]s than the [[product]]s so higher [[Gas Pressure|pressure]] will favour the forward [[Chemical Reaction|reaction]] and the [[Equilibrium Position|equilibrium position]] will have a greater [[concentration]] of [[product]]s than [[reactant]]s.
Ammonium Chloride ⇌ Ammonia + Hydrochloric Acid
<chem> NH4Cl(s) <=> NH3(g) + HCl(g) </chem>
: In this [[Reversible Reaction|reversible reaction]] there are more [[mole]]s of [[gas]] in the [[product]]s than the [[reactant]] so higher [[Gas Pressure|pressure]] will favour the back [[Chemical Reaction|reaction]] and the [[Equilibrium Position|equilibrium position]] will have a greater [[concentration]] of [[reactant]] than [[reactant]]s.
===Meaning===
'''Equilibrium position''' is the the [[ratio]] of [[reactant]]s to [[product]]s when a [[Reversible Reaction|reversible reaction]] is in a state of [[Dynamic Equilibrium|dynamic equilibrium]].
===About the Equilibrium Position===
: The '''equilibrium position''' can be affected by the [[temperature]] and by the [[Gas Pressure|pressure]].
=====Temperature and Equilibrium Position=====
: An increase in [[temperature]] will increase the [[Rate of Reaction|rate]] of an [[endothermic]] [[Chemical Reaction|reaction]] it requires [[energy]] from the environment to take place.
: This means for an [[endothermic]] forward [[Chemical Reaction|reaction]] a higher [[temperature]] will result in more [[product]] being formed. However, for an [[exothermic]] forward [[Chemical Reaction|reaction]] less product will be formed as the back [[Chemical Reaction|reaction]] will be [[endothermic]] and would increase its [[Rate of Reaction|rate]] with higher [[temperature]].
=====Pressure and Equilibrium Position=====
: For [[reaction]]s involving a [[gas]] as either one of the [[reactant]]s or [[product]]s changing the pressure will affect the position of '''dynamic equilibrium'''.
: The number of [[mole]]s of [[gas]] in the [[reactant]]s and [[product]]s will determine which direction of [[Chemical Reaction|reaction]] is favoured by higher [[Gas Pressure|pressure]].
: If the forward [[Chemical Reaction|reaction]] [[product|produces]] more [[mole]]s of [[gas]] than the back [[Chemical Reaction|reaction]] then high [[Gas Pressure|pressure]] will reduce the amount of [[product]]s formed.
: If the forward [[Chemical Reaction|reaction]] [[product|produces]] less [[mole]]s of [[gas]] than the back [[Chemical Reaction|reaction]] then high [[Gas Pressure|pressure]] will increase the amount of [[product]]s formed.
===Examples===
Hydrogen + Nitrogen ⇌ Ammonia
<chem> 3H2(g) + N2(g) <=> 2NH3(g) </chem>
: In this [[Reversible Reaction|reversible reaction]] there are more [[mole]]s of [[gas]] in the [[reactant]]s than the [[product]]s so higher [[Gas Pressure|pressure]] will favour the forward [[Chemical Reaction|reaction]] and the [[Equilibrium Position|equilibrium position]] will have a greater [[concentration]] of [[product]]s than [[reactant]]s.
Ammonium Chloride ⇌ Ammonia + Hydrochloric Acid
<chem> NH4Cl(s) <=> NH3(g) + HCl(g) </chem>
: In this [[Reversible Reaction|reversible reaction]] there are more [[mole]]s of [[gas]] in the [[product]]s than the [[reactant]] so higher [[Gas Pressure|pressure]] will favour the back [[Chemical Reaction|reaction]] and the [[Equilibrium Position|equilibrium position]] will have a greater [[concentration]] of [[reactant]] than [[reactant]]s.