Equilibrium Position (Chemistry) - Revision history

NRJC at 22:30, 3 September 2020

2020-09-03T22:30:07Z

NRJC: NRJC moved page Equilibrium Position to Equilibrium Position (Chemistry)

2020-09-03T22:20:23Z

NRJC moved page Equilibrium Position to Equilibrium Position (Chemistry)

NRJC at 22:19, 3 September 2020

2020-09-03T22:19:42Z

Ellen References at 15:03, 6 December 2019

2019-12-06T15:03:34Z

NRJC: /* Pressure and Equilibrium Position */

2019-04-05T12:21:45Z

‎Pressure and Equilibrium Position

NRJC: /* About the Equilibrium Position */

2019-01-27T12:52:04Z

‎About the Equilibrium Position

NRJC: /* Temperature and Equilibrium Position */

2019-01-27T12:50:22Z

‎Temperature and Equilibrium Position

NRJC at 16:06, 16 January 2019

2019-01-16T16:06:47Z

NRJC: Created page with "==Key Stage 4 Higher== ===Meaning=== '''Equilibrium position''' is the the ratio of reactants to products when a reversible reaction is in..."

2019-01-16T16:06:19Z

Created page with "==Key Stage 4 Higher== ===Meaning=== '''Equilibrium position''' is the the ratio of reactants to products when a reversible reaction is in..."

New page

==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.

@@ Line 20: / Line 20: @@
 Hydrogen + Nitrogen ⇌ Ammonia
-<math> 3H2(g) + N2(g) <=> 2NH3(g) </math>
+<math> 3H_2(g) + N_2(g) ⇌ 2NH_3(g) </math>
-: 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.
+: 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''' will have a greater [[concentration]] of [[product]]s than [[reactant]]s.
 Ammonium Chloride ⇌ Ammonia + Hydrochloric Acid
-<math> NH4Cl(s) <=> NH3(g) + HCl(g) </math>
+<math> NH_4Cl(s) ⇌ NH_3(g) + HCl(g) </math>
-: 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.
+: 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''' will have a greater [[concentration]] of [[reactant]] than [[reactant]]s.
 ===References===

← Older revision		Revision as of 15:03, 6 December 2019
Line 27:		Line 27:
	<chem> NH4Cl(s) <=> NH3(g) + HCl(g) </chem>		<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.		: 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.
		+
		+	===References===
		+	====OCR====
		+
		+	:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Equilibrium position, pages 188-191, Gateway GCSE Chemistry, Oxford, OCR '']

← Older revision	Revision as of 22:20, 3 September 2020
(No difference)

@@ Line 12: / Line 12: @@
 =====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|dynamic equilibrium]].
+: For [[Chemical Reaction|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|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.

@@ Line 5: / Line 5: @@
 ===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.