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38 Cards in this Set
- Front
- Back
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Rate of reaction
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The change in concentration of a reactant OR product over time
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Order
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The power to which the concentration of the reactant is raised in the rate equation
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Rate constant
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k. The constant that links the rate of reaction with the concentrations of the reactants raised to the power of their orders in the rate equation!
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Half-life
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The time taken for the concentration of a reactant to reduce by half
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Rate-determining step
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The slowest step in the reaction mechanism of a multi-step reaction
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The half-life of a first-order reaction is ___________ of the concentration
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independent
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Two factors about zero order conc-time graphs
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Conc decreases at a constant rate
Half-life decreases with time |
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Two factors about first order conc-time graphs
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Concentration halves in equal time intervals
Half-life is CONSTANT |
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Two factors about second order conc-time graphs
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Concetration decreases rapidly, but rate of decrease then slows down
Half-life INCREASES with time |
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Zero order
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First order
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Second order
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Zero order
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k =
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rate/[A]ⁿⁿ[B]ⁿ
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How is k affected by an increase in temperature?
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Increase in temperature = Increase in k and hence there is a faster rate of reaction
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Kc =
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[C]^c[D]^d/[A]^a[B]^b
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For an exothermic reaction, an increase on temperature _________ Kc
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decreases
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For an endothermic reaction, an increase in temperature _________ Kc
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increases
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How does concentration/pressure/a catalyst affect Kc?
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None of them do!
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What is an acid?
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A species that can DONATE a proton
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What is a base?
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A species that can ACCEPT a proton
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What is an acid-base pair?
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A pair of two species that TRANSFORM INTO EACH OTHER by gain or loss of a PROTON
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What is a conjugate acid?
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A species formed when a proton is added to a base
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What is a conjugate base?
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A species formed when a proton is added to an acid
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Strong acid
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An acid that completely dissociates in solution
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Weak acid
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An acid that partially dissociates in solution
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What does acid dissociation constant show?
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The extent of acid dissociation
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pH =
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-log[H⁺]
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[H⁺] =
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10^-pH
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Kw =
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[H⁺][OH⁻]
At 25*C - Kw = 1.00 x 10^-14 |
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Strong acid, [H⁺] =
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[HA]
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Weak acid, [H⁺] =
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sqrt(Ka * [HA])
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Strong base, [H⁺] =
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Kw/[OH⁻]
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Buffer solution
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A system that minimises pH changes on addition of small amounts of an acid or a base
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How can a buffer solution be made?
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From a weak acid and a salt of the weak acid
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Buffer, [H⁺] =
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Ka * [Acid]/[Salt]
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What is carbonic acid-hydrogencarbonate used for?
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A buffer in the control of blood pH
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Enthalpy change of neutralisation
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The energy change that accompanies the neutralisation of an aqueous acid by an aqueous base to form one mole of water under standard conditions
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