Difference between revisions of "Reversible Reaction"
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: '''Reversible reactions''' use the symbol ⇌ to show that the [[Chemical Reaction|reaction]] can happen both ways. | : '''Reversible reactions''' use the symbol ⇌ to show that the [[Chemical Reaction|reaction]] can happen both ways. | ||
: A [[Reaction Mixture|reaction mixture]] which can undergo a '''reversible reaction''' will reach a state of [[Dynamic Equilibrium|dynamic equilibrium]] where there is a constant amount of the [[reactant]]s and [[product]]s as the [[Chemical Reaction|reaction]] keeps happening in both directions. | : A [[Reaction Mixture|reaction mixture]] which can undergo a '''reversible reaction''' will reach a state of [[Dynamic Equilibrium|dynamic equilibrium]] where there is a constant amount of the [[reactant]]s and [[product]]s as the [[Chemical Reaction|reaction]] keeps happening in both directions. | ||
| − | : Since some [[reaction]]s may be [[exothermic]] and others may be [[endothermic]], then one direction of [[Chemical Reaction|reaction]] will provide [[energy]] to the environment while the other direction will [[Absorb (Physics)|absorb]], that same amount of, [[energy]]. | + | : Since some [[Chemical Reaction|reaction]]s may be [[exothermic]] and others may be [[endothermic]], then one direction of [[Chemical Reaction|reaction]] will provide [[energy]] to the environment while the other direction will [[Absorb (Physics)|absorb]], that same amount of, [[energy]]. |
===Examples=== | ===Examples=== | ||
Revision as of 12:21, 5 April 2019
Key Stage 4
Meaning
Reversible Reactions are reactions in which the products of that reaction, may themselves react to form the original reactants.
About Reversible Reactions
- Reversible reactions use the symbol ⇌ to show that the reaction can happen both ways.
- A reaction mixture which can undergo a reversible reaction will reach a state of dynamic equilibrium where there is a constant amount of the reactants and products as the reaction keeps happening in both directions.
- Since some reactions may be exothermic and others may be endothermic, then one direction of reaction will provide energy to the environment while the other direction will absorb, that same amount of, energy.
Examples
Hydrogen + Nitrogen ⇌ Ammonia
<chem> 3H2(g) + N2(g) <=> 2NH3(g) </chem>
Calcium Oxide + Carbon Dioxide ⇌ Calcium Carbonate
<chem> CaO(aq) + CO2(g) <=> CaCO3(s) </chem>
Ammonium Chloride ⇌ Ammonia + Hydrochloric Acid
<chem> NH4Cl(s) <=> NH3(g) + HCl(g) </chem>