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The equilibrium constant is K=[KNO3]/[AgNO3][KSCN]
- The equilibrium constant is defined as the ratio of the concentration of products upon reactants.
- The species present in solid phase are taken as unity.
- Substituting the values, we get
- K=[KNO3][AgSCN]/AgNO3][KSCN]
- K=[KNO3]×1/[AgNO3][KSCN]
- k=[KNO3]/[AgNO3][KSCN]
- The ratio of reactant to product amounts that is used to predict chemical behavior is the definition of the equilibrium constant for a chemical process.
- The rate constants are constant at a certain temperature.
- The value of a chemical reaction's reaction quotient at chemical equilibrium, a condition that a dynamic chemical system approaches is the equilibrium constant for that reaction when enough time has passed and at which its composition shows no evident tendency to change further.
- The equilibrium constant is independent of the initial analytical concentrations of the species of the reactant and product in the mixture given a certain set of reaction conditions.
- As a result, the composition of a system at equilibrium may be calculated from its starting composition using known equilibrium constant values.
- However, factors affecting the reaction such as temperature, solvent, and ionic strength may all affect the equilibrium constant's value.
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