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33 Cards in this Set
- Front
- Back
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Strong Acids |
HCl, HBr, HI, HNO3, ClO4, H2SO4 |
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Strong Bases |
hydroxides of Group IA, IIA |
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Common Salts |
Strong electrocytes |
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Rate law |
- (change in concentration of reactants) / time |
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Rate law 2 |
k (A)m (B)n |
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Arrehnius Equation |
k=pZe -Ea/RT |
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Collision State Theory |
maxwell-Roltzman distribution curve |
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Transition State Theory |
Intermediate = produced then consumed Catalyst = consumed then produced |
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Zero Order Rate law |
Ax = -kt + A0 |
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Zero Order shape |
Ax = -kt + A0 |
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Zero Order half life |
A0/ 2k |
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1st Order Rate law |
Ln Ax = -kt + ln A0 |
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1st Order graphical representation |
Ln Ax = -kt + ln A0 |
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2nd Order rate law |
1/A0 - 1/Ax = -Kt 1/Ax = Kt + 1/A0 |
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2nd Order graphical representation |
1/A0 - 1/Ax = -Kt 1/Ax = Kt + 1/A0 |
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half life for 1st Order |
ln2/K |
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half life for 2nd Order |
1 / Ao K |
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1st Order simplified to A |
A = A0 e -kt |
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mole fraction |
mole solvent / mole solvent + mol solution |
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mass percent |
g solvent / g solution |
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molality |
moles solvent / g solution |
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conditions necessary hydrogen bonding |
a H atom is covalently bonded to a small, Highly EN non metal and simultaneously attracted to another non metal of a neighboring molecule |
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Average rate vs instantaenous rate |
average is change over time and assumes that rate is constant. Initial rate is during an extremely short time before reverse reaction |
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higher lattice energy |
in more insoluble in water |
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Necessary conditions for Eq reaction |
1. reversible 2. rate of forward rxn and reversible rxn is same |
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What is System? |
an isolated setting |
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K equilibrium Constant |
Kf/Kr = reactants / products = K |
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Rxn quotient Q > K |
reverse |
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Rxn quotient Q < K |
forward |
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Q = K |
Equilibruim |
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Solution of salts : strong base and weak acid |
pH > 7 |
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solution of salts : strong acid and weak base |
pH < 7 |
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sd |
