Chemistry Notes Reaction Rates - calhoun.k12.al.us Notes... · Method of Initial Rates Determines...
Transcript of Chemistry Notes Reaction Rates - calhoun.k12.al.us Notes... · Method of Initial Rates Determines...
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2H+ + O-2 →→→→ H2O
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4K+ + C4- →→→→ K4C
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H2O →→→→ 2H+ + O-2
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4Cs+ + Pb4-Cs4Pb →→→→
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2Al3+ + 3Ag2S →→→→
Al2S3 + 6Ag2+
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2Al 3+ + 3Ra2S →→→→
Al2S3 + 6Ra 2+
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HCl + NaOH→→→→ NaCl + H2O
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3BaCl2 + 2H3PO4 →→→→
Ba3(PO4)2 + 6HCl
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C3H8 + 5O2→→→→ 3CO2 + 4H2O
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C6H12O6 + 6O2 →→→→
6CO2 + 6H2O
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CuO + H2 →→→→ Cu + H2O
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Rate Law
The mathematical
relationship between the rate
of a chemical reaction at a
given temperature and the
concentration of reactants.
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moles/L =M
Molarity
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Reaction Rate
The change in concentration of a reactant or product per unit time, generally calculated and expressed in moles per liter per second. (mol/sL) or
(M/s)
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Average rate = ∆quantity/∆t
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CO + NO2 → CO2 + NO
NO at t1 = 0.000 M and 0.00s
NO at t2 = 0.010 M and 2.00s
[0.010M – 0.000M] ÷ [2.00s –
0.00s] = 0.0050 M/s
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CO + NO2 → CO2 + NO
CO2 at t1 = 0.000 M and 0.00s
CO2 at t2 = 0.030 M and 4.00s
[0.030M – 0.000M] ÷ [4.00s –
0.00s] = 0.0075 M/s
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Factors which influence
reaction rate• Concentration
• Surface Area
• Temperature
• Catalyst
• Inhibitor
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Catalyst
A substance that increases
the rate of a chemical
reaction by lowering
activation energies but is not
itself consumed in the
reaction.
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Heterogeneous Catalyst
A catalyst that exists in
a different physical
state than the reaction
it catalyzes.
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Homogeneous
Catalyst
A catalyst that exists in
the same physical
state as the reaction it
catalyzes.
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InhibitorA substance that
slows down the
reaction rate of a
chemical reaction or
prevents a reaction
from happening.
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Specific Rate Constant
A numerical value that
relates reaction rate
and concentration of
reactant at a specific
temperature.
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Rate = k[A]
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Reaction Order
For a reactant, describes how the rate is affected by the
concentration of that reactant.
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Rate=k[A]m[B]n
aA +bB → products
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Method of Initial Rates
Determines the reaction
order by comparing the initial
rates of a reaction carried
out with varying reactant
concentrations.
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2NO + 2H2 → N2 + 2H2O
16.0 X 10-30.2000.2003
4.00 X 10-30.1000.2002
2.00 X 10-30.1000.1001
Initial Rate (M/s)Initial [B] (M)Initial [A] (M)Trial
aA + bB → products
Experimental Initial Rates for
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2NO + 2H2 → N2 + 2H2O
According to the table, from
trial 1 to trial 2, as [A] doubles,
so did the final. This causes
the order to become 1.
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According to the table, from
trial 2 to trial 3, as [B]
doubles, the final increased
by a multiple of four. This
causes the order to become
2.
2NO + 2H2 → N2 + 2H2O
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Rate = k[A]1[B]2
Rate = k[NO]1[H2]2
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4.0 X 10-30.2000.2003
2.00 X 10-30.1000.2002
2.00 X 10-30.1000.1001
Initial Rate (M/s)Initial [B] (M)Initial [A] (M)Trial
aA + bB→ products
Experimental Initial Rates for
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According to the table,
from trial 1 to trial 2, as [A]
doubled, the final did not
change. This gave an
order of 0.
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According to the table,
from trial 2 to 3, as [B]
doubled, so did the final.
This gave an order of 1.
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Rate = k[A]0[B]1
Rate = k[B]
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2ClO2 + 2OH- → ClO3- +
ClO2- + H2O
13.80.1000.1003
27.60.2000.1002
6.90.2000.0501
Initial Rate (M/s)Initial [B] (M)Initial [A] (M)Trial
aA + bB→ products
Experimental Initial Rates for
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2ClO2 + 2OH- → ClO3- +
ClO2- + H2O
According to the table, from
trial 1 to trial 2, as [A]
doubled, the final increased
by a multiple of four. This
gave an order of 2.
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2ClO2 + 2OH- → ClO3- +
ClO2- + H2O
According to the table,
from trial 2 to 3, as [B]
halved, so did the
final. This gave an
order of 1.
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Rate = k[A]2[B]1
Rate = k[ClO2]2[OH-]1
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Instantaneous Rate
The rate of decomposition at a specific time, calculated
from the rate law, the specific rate constant, and the concentrations of all the
reactants.
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You can find the
instantaneous rate by
multiplying k (which is
given to you) by the
concentration of each
reactant after you find
each reactant’s order.
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2NO + 2H2 → N2 + 2H2O
k=1.0 X10-5 s-1
Rate = k[NO]1[H2]2
Rate = k[0.030M]1[0.04M]2
Rate=1.0X10-5s-1 (0.03M)
(0.04M)2
Rate=4.8X10-10 M/s
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Complex Reaction
A chemical reaction
that consists of two or
more elementary
steps.
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Reaction Mechanism
The complete sequence of
elementary steps that make up a complex
reaction.
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Intermediate
A substance produced in one elementary step of a complex reaction and
consumed in a subsequent elementary step. It does not appear in the final equation.
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Rate-determining Step
The slowest elementary step in a complex reaction;
limits the instantaneous rate of the overall reaction