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CHEM 113:Final Review
rate of following reaction:
2O3(g)→3O2(g)
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(-1/2)(Δ[O3]/t)=(1/3)(Δ[O2]/t)
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units of k for
zero:
first:
second:
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0: mole/(L⋅s)
1st: 1/s=s-1
2nd: L/(s⋅mole)
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equation to find order of rate law
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(rate2/rate1)=([2]/[1])x
solve for x to find order
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find two _____ to find order of that compound
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experiments where concentration changes, then put into formula
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put given into order equation if rate cant change
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then solve for exponent (order)
q |
2 []'s, time and k value is what kind of problem?
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integrated rate law
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how to find overall k value given a stacked reaction
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manipulate top eqns to get overall exactly
flip equation (-1 power to k value)
multiply by constant to get rid of intermediate ([constant power] to k value)
overall k value is (now altered) k values multiplied together
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Q>K?
Q<K?
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reaction left (reactants favored)
reaction right (products favored)
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equilibrium equations involve
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pressure (atm) and molarity
unless titration involves strong base or acid (then moles)
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kp and kc
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pressure and concentration
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exothermic
endothermic
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ex: -ΔH(heat on products)
en: +ΔH(heat on reactants)
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Don't Care None
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Cl-, Br-, NO3-, ClO4-, Li↓, Ca↓
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1.10E-14
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ka⋅kb |
ΔH (kj)
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Enthalpy
(+) endothermic
(-) exothermic
ΔH=P-R
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ΔS (J)
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Entropy
(+) disorder
(-) take away disorder
ΔS=P-R
ΔSsurr=(-ΔH/Temp)
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ΔG=ΔH-TΔS
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(+) non-spon
(-) spon
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which will see changes in solubility with changes in pH?
√?
√?
x?
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√: OH-
√: weak bases
x: Cl-, Br-, I-, ClO4-
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strong acids
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HCl, HBr, HNO3, HClO4, H2SO4, HI-
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strong bases
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Li↓, Ca↓, OH-
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acid vs base rules?
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general: H=acid
internal H= base (CHOO)
metal: acid (Pb)
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heat vs. pH
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heat↑, pH↓
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how to create a buffer
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add a conjugate
add a strong acid/base
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loss of electrons
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oxidized
anode (reducing agent)
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gain of electrons
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reduced
cathode (oxidizing agent)
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what side are electrons on in:
oxidizing agent
reducing agent
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oxy agent: left
reduce agent: right
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balancing redox reactions
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1 split into half reactions. 2 balance all element ecpt H/O. 3 balance O with H20. 4 balance H with H+. 5 balance charge with e-. 6 convert to OH- then cancel water
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cell notation
/ and ,
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Anode//Cathode
/ means change state
, means same state
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voltaic (galvanic) cell:
E=
ΔG=
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Ecell=+
ΔG= -
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what does not effect rate of the reaction?
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catalyst
inert gas (noble gas)
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Ksp
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may involve more than one acid/base equation (stacked)
also involves just a solid and two ions
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pH=14
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pH=14-(-log[OH-])
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how to predict if solid will form
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Qsp>Ksp yes
Qsp<Ksp no
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if given volume and Molarity
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M1V1=M2V2
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activation energy and change H on graph
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ae=increase from the reactants. change in h is difference from products and reactants
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acid equation
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HA+H20↔A-+H3O+
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HA+H20↔A-+H3O+
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B+H2O↔HB++OH-
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