Module 1 - F325 Flashcards
Rate of reaction
Rate of reaction is the change in concentration of a reactant or product per unit time.
Initial rate of reaction
Initial rate of reaction is the change in concentration of a reactant, or product, per unit time at the start of the reaction when t=o.
Rate equation
A + B —> C is given by rate =k[A]m [B]n.
m is the order of reaction with respect to A
n s the order of reaction with respect to B
Order
The order with respect to a reactant is the power to which the concentration of the reactant is raised in the rate equation.
Overall Order
The overall order of reaction is the sum of the individual orders, m+n
Rate constant, K
The rate constant, K, is the constant that links the rate of reaction with the concentrations of the reactants raised to the powers of their orders in the rate equation.
Half-life
The half-life of a reactant is the time taken for the concentration of the reactant to reduce by half.
Reaction Mechanism
A reaction mechanism is a series of steps that, together, make up the overall reaction.
Rate-determining step
The rate-determining step is the slowest step in the reaction mechanism of a multi-step reaction.
Intermediate
An intermediate is a species fromed in one step of a multi-step reaction that is used up in a subsequent step, and is not seen as either a reactant or a product of the overall equation.
Dynamic Equilibrium
Dynamic equilibrium exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction.
Homogeneous equilibrium
A homogeneous equilibrium is an equilibrium in which all the species making up the reactants and products are in the same physical state.
Heterogeneous equilibrium
A heterogeneous equilibrium is an equilibrium in which species making up the reactants and products are in different physical states.
Bronsted- Lowry acid
A bronsted lowry acid is a proton, H+, donor.
Bronsted- Lowry base
A bronsted lowry base is a proton, H+, acceptor.
Alkali
An alkali is a base that dissolves in water forming OH- ions.
Neutralisation
Neutralisation is a chemical reaction in which an acid and a base react together to produce a salt and water.
Acid-base pair
An acid-base pair is a pair of two species that transform into each other by gain or loss of a proton.
Strong acid
A strong acid is an acid that completely dissociates in solution.
Weak acid
A weak acid is an acid that partially dissociates in solution.
Buffer Solution
A buffer solution is a mixture that minimizes pH changes on addition of small amounts of acid or base.
Equivalence point
The equivalence point is the point in a titration at which the volume of one solution has reacted exactly with the volume of the second solution.
End point
The end point is the point in a titration at which there are equal concentrations of the weak acid and conjugate base forms of the indicator.
Standard enthalpy change of neutralisation
Standard enthalpy change of neutralization is the energy change that accompanies the neutralization of an aqueous acid by an aqueous base to form one mole of water, under standard conditions.
