ap chemistry chapter 14 jeopardy
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AP Chemistry Chapter 14 Jeopardy. Jennie L. Borders. Round 1 – Chapter 14. Rate Laws 100. The reaction 2ClO 2 + 2OH - ClO 3 - + ClO 2 - + H 2 O was studied with the following results: Determine the rate law for the reaction. Rate = k[ClO 2 ] 2 [OH - ]. Rate Laws 200. - PowerPoint PPT PresentationTRANSCRIPT
AP ChemistryAP ChemistryChapter 14 JeopardyChapter 14 Jeopardy
Jennie L. BordersJennie L. Borders
Round 1 – Chapter 14 Round 1 – Chapter 14
Rate LawsRate Laws Half-LifeHalf-Life GraphingGraphing MechanismsMechanismsActivation Activation
EnergyEnergy SurpriseSurprise
100 100 100 100 100 100
200 200 200 200 200 200
300 300 300 300 300 300
400 400 400 400 400 400
500 500 500 500 500 500
Rate Laws 100Rate Laws 100The reaction 2ClOThe reaction 2ClO22 + 2OH + 2OH-- ClO ClO33
-- + +
ClOClO22-- + H+ H22O was studied with the O was studied with the
following results:following results:
Determine the rate law for the reaction.Determine the rate law for the reaction.
Rate = k[ClORate = k[ClO22]]22[OH[OH--]]
ExperimentExperiment [ClO[ClO22] (M)] (M) [OH[OH--] (M)] (M) Rate (M/s)Rate (M/s)
11 0.0600.060 0.0300.030 0.02480.0248
22 0.0200.020 0.0300.030 0.002760.00276
33 0.0200.020 0.0900.090 0.008280.00828
Rate Laws 200Rate Laws 200The reaction 2ClOThe reaction 2ClO22 + 2OH + 2OH-- ClO ClO33
--
+ ClO+ ClO22-- + H+ H22O was studied with the O was studied with the
following results:following results:
Calculate the rate constant.Calculate the rate constant.
229.63 M229.63 M-2-2ss-1-1
ExperimentExperiment [ClO[ClO22] (M)] (M) [OH[OH--] (M)] (M) Rate (M/s)Rate (M/s)
11 0.0600.060 0.0300.030 0.02480.0248
22 0.0200.020 0.0300.030 0.002760.00276
33 0.0200.020 0.0900.090 0.008280.00828
Rate Laws 300Rate Laws 300The reaction 2ClOThe reaction 2ClO22 + 2OH + 2OH-- ClO ClO33
-- + +
ClOClO22-- + H+ H22O was studied with the following O was studied with the following
results:results:
Calculate the rate when [ClOCalculate the rate when [ClO22] = 0.1M and ] = 0.1M and
[OH[OH--] = 0.05M.] = 0.05M.
0.115 M/s0.115 M/s
ExperimentExperiment [ClO[ClO22] (M)] (M) [OH[OH--] (M)] (M) Rate (M/s)Rate (M/s)
11 0.0600.060 0.0300.030 0.02480.0248
22 0.0200.020 0.0300.030 0.002760.00276
33 0.0200.020 0.0900.090 0.008280.00828
Rate Laws 400Rate Laws 400The following data was measured for the reaction The following data was measured for the reaction
BFBF33 + NH + NH33 F F33BNHBNH33
What is the rate law for the reaction?What is the rate law for the reaction?
Rate = k[BFRate = k[BF33][NH][NH33]]
ExperimentExperiment [BF[BF33] (M)] (M) [NH[NH33] (M)] (M) Initial Rate Initial Rate (M/s)(M/s)
11 0.2500.250 0.2500.250 0.21300.2130
22 0.2500.250 0.1250.125 0.10650.1065
33 0.2000.200 0.1000.100 0.06820.0682
44 0.3500.350 0.1000.100 0.11930.1193
55 0.1750.175 0.1000.100 0.05960.0596
Rate Laws 500Rate Laws 500The following data was measured for the reaction BFThe following data was measured for the reaction BF33 + +
NHNH33 F F33BNHBNH33
What is the rate when [BFWhat is the rate when [BF33] = 0.100M and [NH] = 0.100M and [NH33] = 0.500M?] = 0.500M?
0.1704 M/s0.1704 M/s
ExperimentExperiment [BF[BF33] (M)] (M) [NH[NH33] (M)] (M) Initial Rate Initial Rate (M/s)(M/s)
11 0.2500.250 0.2500.250 0.21300.2130
22 0.2500.250 0.1250.125 0.10650.1065
33 0.2000.200 0.1000.100 0.06820.0682
44 0.3500.350 0.1000.100 0.11930.1193
55 0.1750.175 0.1000.100 0.05960.0596
Half-Life 100Half-Life 100How do the half-lives of first-order and How do the half-lives of first-order and
second-order reactions differ?second-order reactions differ?
Since the half-lives of first-order Since the half-lives of first-order reactions are not based on initial reactions are not based on initial
concentration, then all the half-lives concentration, then all the half-lives are equal. Since the half-lives of are equal. Since the half-lives of
second-order reactions are based on second-order reactions are based on initial concentrations, then each half-initial concentrations, then each half-life is longer than the previous one.life is longer than the previous one.
Half-Life 200Half-Life 200
The gas-phase decomposition of The gas-phase decomposition of SOSO22ClCl22, SO, SO22ClCl22 SO SO22 + Cl + Cl22, is , is
first order in SOfirst order in SO22ClCl22. At 320. At 320ooC the C the
rate constant is 2.2 x 10rate constant is 2.2 x 10-5 -5 ss-1-1. . What is the half-life at this What is the half-life at this
temperature?temperature?
31,500s31,500s
Half-Life 300Half-Life 300
Molecular iodine, IMolecular iodine, I2(g)2(g), dissociates into , dissociates into
iodine atoms at 625K with a first-iodine atoms at 625K with a first-order rate constant of 0.271 sorder rate constant of 0.271 s-1-1. .
What is the half-life of the reaction?What is the half-life of the reaction?
2.56s 2.56s
Half-Life 400Half-Life 400
Molecular iodine, IMolecular iodine, I2(g)2(g), dissociates into , dissociates into
iodine atoms at 625K with a first-iodine atoms at 625K with a first-order rate constant of 0.271sorder rate constant of 0.271s-1-1. If . If you start with 0.050M Iyou start with 0.050M I22 at this at this
temperature, how much will remain temperature, how much will remain after 5.12s assuming that the iodine after 5.12s assuming that the iodine atoms do not recombine to form Iatoms do not recombine to form I22??
0.012M0.012M
Half-Life 500Half-Life 500
The first-order rate constant for the The first-order rate constant for the decomposition of Ndecomposition of N22OO55, 2N, 2N22OO55
4NO4NO22 + O + O22, at 70, at 70ooC is 6.28 x 10C is 6.28 x 10-3-3
ss-1-1. What is the half-life of N. What is the half-life of N22OO55
at 70at 70ooC?C?
110.35s110.35s
Graphing 100Graphing 100
For a second-order reaction, what For a second-order reaction, what quantity, when graphed versus quantity, when graphed versus time, will yield a straight line?time, will yield a straight line?
1/[A]1/[A]
Graphing 200Graphing 200
Consider the following data:Consider the following data:
Determine whether the reaction is first Determine whether the reaction is first order or second order.order or second order.
First OrderFirst Order
Time Time (s)(s) 00 4040 8080 120120 160160
Moles Moles of Aof A 0.1000.100 0.0670.067 0.0450.045 0.0300.030 0.0200.020
Graphing 300Graphing 300The gas-phase decomposition of NOThe gas-phase decomposition of NO22, 2NO, 2NO22
2NO + O 2NO + O22 is studied at 383 is studied at 383ooC, given C, given
the following data:the following data:
Is the reaction first order or second order Is the reaction first order or second order with respect to the concentration of NOwith respect to the concentration of NO22??
Second OrderSecond Order
Time Time (s)(s) 0.00.0 5.05.0 10.010.0 15.015.0 20.020.0
[NO[NO22] ]
(M)(M)0.1000.100 0.0170.017 0.0090.009 0.00620.0062 0.00470.0047
Graphing 400Graphing 400At 23At 23ooC and in 0.5M HCl, the following C and in 0.5M HCl, the following
data was obtained for the data was obtained for the disappearance of sucrose:disappearance of sucrose:
Is the reaction first order or second order Is the reaction first order or second order with respect to [Cwith respect to [C1212HH2222OO1111]?]?
First OrderFirst Order
Time Time (min)(min) 00 3939 8080 140140 210210
[C[C1212HH2222OO1111] ]
(M)(M)0.3160.316 0.2740.274 0.2380.238 0.1900.190 0.1460.146
Graphing 500Graphing 500
Is the following reaction first or Is the following reaction first or second order?second order?
Second OrderSecond Order
Mechanisms 100Mechanisms 100The decomposition of hydrogen peroxide is The decomposition of hydrogen peroxide is
catalyzed by iodide ion. The catalyzed catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step reaction is thought to proceed by a two-step
mechanism:mechanism:
HH22OO22 + I + I-- H H22O + IOO + IO-- (slow) (slow)
IOIO-- + H + H22OO22 H H22O + OO + O22 + I + I-- (fast) (fast)
Write the chemical equation for the overall Write the chemical equation for the overall process.process.
2H2H22OO22 2H 2H22O + OO + O22
Mechanisms 200Mechanisms 200The decomposition of hydrogen peroxide is The decomposition of hydrogen peroxide is
catalyzed by iodide ion. The catalyzed catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-reaction is thought to proceed by a two-
step mechanism:step mechanism:
HH22OO22 + I + I-- H H22O + IOO + IO-- (slow) (slow)
IOIO-- + H + H22OO22 H H22O + OO + O22 + I + I-- (fast) (fast)
Predict the rate law for the overall process.Predict the rate law for the overall process.
Rate = k[HRate = k[H22OO22]]
Mechanisms 300Mechanisms 300You find the reaction 4HBr + OYou find the reaction 4HBr + O22 2H 2H22O + 2BrO + 2Br22 to to
be first order with respect to HBr and first order be first order with respect to HBr and first order with respect to Owith respect to O22. You propose the following . You propose the following
mechanism:mechanism:
HBr + OHBr + O22 HOOBr HOOBr
HOOBr + HBr HOOBr + HBr 2HOBr 2HOBr
HOBr + HBr HOBr + HBr H H22O + BrO + Br22
Based of the rate law which step is rate Based of the rate law which step is rate determining?determining?
Rate = k[HBr][ORate = k[HBr][O22] ]
The first step is rate determining.The first step is rate determining.
Mechanisms 400Mechanisms 400The following mechanism has been The following mechanism has been
proposed for the reaction of NO with Hproposed for the reaction of NO with H22 to to form Nform N22O and HO and H22O:O:
NO + NO NO + NO N N22OO22
NN22OO22 +H +H22 N N22O + HO + H22OO
The observed rate law is rate = k[NO]The observed rate law is rate = k[NO]22[H[H22]. ]. What can we conclude about the relative What can we conclude about the relative speeds of the first and second reactions?speeds of the first and second reactions?
The second step is slow (rate The second step is slow (rate determining) and the first step is fast.determining) and the first step is fast.
Mechanisms 500Mechanisms 500Ozone in the upper atmosphere can be Ozone in the upper atmosphere can be
destroyed by the following two-step destroyed by the following two-step mechanism:mechanism:
Cl + OCl + O33 ClO + O ClO + O22
ClO + O ClO + O Cl + O Cl + O22
What is the overall reaction and list any What is the overall reaction and list any catalysts or intermediates?catalysts or intermediates?
OO33 + O + O 2O 2O22
Catalyst – ClCatalyst – ClIntermediate - ClOIntermediate - ClO
Activation Energy 100Activation Energy 100
What is the activation energy?What is the activation energy?
The difference in energy between The difference in energy between the energy to the transition state the energy to the transition state and the energy of the reactants.and the energy of the reactants.
Activation Energy 200Activation Energy 200The rate of the reactionThe rate of the reaction
CHCH33COOCCOOC22HH55 + OH + OH-- CH CH33COOCOO-- + C + C22HH55OHOH
Was measured at several temperatures, and the Was measured at several temperatures, and the following data was collected: following data was collected:
Temperature (Temperature (ooC) k(MC) k(M-1-1ss-1-1))1515 0.0521 0.05212525 0.101 0.1013535 0.184 0.1844545 0.332 0.332
Determine this data, determine EDetermine this data, determine Eaa. .
47,041.61 J/mol47,041.61 J/mol
Activation Energy 300Activation Energy 300The temperature dependence of the rate The temperature dependence of the rate
constant for the reaction is tabulated as constant for the reaction is tabulated as follows:follows:
Temperature (K)Temperature (K) k (Mk (M-1-1ss-1-1))600600 0.028 0.028650650 0.22 0.22700700 1.3 1.3750750 6.0 6.0800800 23 23
Calculate ECalculate Eaa.. 133,803.44 J/mol133,803.44 J/mol
Activation Energy 400Activation Energy 400
What part of the energy profile of a What part of the energy profile of a reaction is affected by a catalyst?reaction is affected by a catalyst?
Activation energyActivation energy
Activation Energy 500Activation Energy 500The oxidation of SOThe oxidation of SO22 to SO to SO33 is catalyzed by is catalyzed by
NONO22. The reaction proceeds as follows:. The reaction proceeds as follows:
NONO22 + SO + SO22 NO + SO NO + SO33
2NO + O2NO + O22 2NO 2NO22
Why do we consider NOWhy do we consider NO22 a catalyst and not an a catalyst and not an intermediate in this reaction?intermediate in this reaction?
NONO22 is present at the beginning and is present at the beginning and
end of the reaction. Intermediates end of the reaction. Intermediates are formed during the reaction and are formed during the reaction and
used during the reaction.used during the reaction.
Surprise 100Surprise 100
What are the 4 factors that affect the What are the 4 factors that affect the rate of a reaction?rate of a reaction?
1.1.Concentration of reactantsConcentration of reactants2. Catalysts2. Catalysts
3. State of reactants3. State of reactants4. Temperature4. Temperature
Surprise 200Surprise 200
The decomposition of NThe decomposition of N22OO55 in carbon in carbon
tetrachloride proceeds as follows: tetrachloride proceeds as follows: 2N2N22OO55 4NO 4NO22 + O + O22. The rate law is . The rate law is
first order in Nfirst order in N22OO55. At 64. At 64ooC the rate C the rate
constant is 4.82 x 10constant is 4.82 x 10-3-3ss-1-1. What . What happens to the rate when the happens to the rate when the
concentration of Nconcentration of N22OO55 is doubled? is doubled?
The rate doubles.The rate doubles.
Surprise 300Surprise 300
Consider the hypothetical reaction Consider the hypothetical reaction between A, B, and C that is first between A, B, and C that is first order in A, zero order in B, and order in A, zero order in B, and
second order in C.second order in C.
How does the rate change when [A] How does the rate change when [A] is doubled and the other reactant is doubled and the other reactant concentrations are held constant?concentrations are held constant?
The rate doubles.The rate doubles.
Surprise 400Surprise 400
Consider the hypothetical reaction Consider the hypothetical reaction between A, B, and C that is first between A, B, and C that is first order in A, zero order in B, and order in A, zero order in B, and
second order in C.second order in C.
How does the rate change when [B] How does the rate change when [B] is tripled and the other reactant is tripled and the other reactant
concentrations are held constant?concentrations are held constant?
The rate remains the same.The rate remains the same.
Surprise 500Surprise 500
Consider the hypothetical reaction Consider the hypothetical reaction between A, B, and C that is first between A, B, and C that is first order in A, zero order in B, and order in A, zero order in B, and
second order in C.second order in C.
By what factor does the rate change By what factor does the rate change when the concentrations of all when the concentrations of all
three reactants are tripled?three reactants are tripled?
The rate increases 27 fold.The rate increases 27 fold.