ap chemistry chapter 15 jeopardy
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AP Chemistry Chapter 15 Jeopardy. Jennie L. Borders. Round 1 – Chapter 15. k 100. Write the equilibrium constant expression for the following reaction: 2C 2 H 4(g) + 2H 2 O (g) 2C 2 H 6(g) + O 2(g). K c = [C 2 H 6 ] 2 [O 2 ] [C 2 H 4 ] 2 [H 2 O] 2. - PowerPoint PPT PresentationTRANSCRIPT
AP ChemistryAP ChemistryChapter 15 JeopardyChapter 15 Jeopardy
Jennie L. BordersJennie L. Borders
Round 1 – Chapter 15 Round 1 – Chapter 15
KK QQCalculating Calculating Equilibrium Equilibrium ConstantsConstants
Applications Applications of kof k
Le Le Chatelier’s Chatelier’s PrinciplePrinciple
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
k 100k 100Write the equilibrium constant Write the equilibrium constant
expression for the following expression for the following reaction:reaction:
2C2C22HH4(g)4(g) + 2H + 2H22OO(g)(g) 2C 2C22HH6(g)6(g) + O + O2(g)2(g)
KKcc = = [C [C22HH66]]22[O[O22] ]
[C[C22HH44]]22[H[H22O]O]22
k 200k 200
Write the equilibrium constant Write the equilibrium constant expression for the following expression for the following
reaction:reaction:
4HCl4HCl(aq)(aq) + O + O2(g)2(g) 2H 2H22OO(l)(l) + 2Cl + 2Cl2(g)2(g)
KKcc = = [Cl [Cl22]]22__
[HCl][HCl]44[O[O22]]
k 300k 300Does the following reaction favor Does the following reaction favor
the production or reactants or the production or reactants or products?products?
2HBr2HBr(g)(g) H H2(g) 2(g) + Br+ Br2(g)2(g)
KKcc = 5.8 x 10 = 5.8 x 10-18-18
reactantsreactants
k 400k 400
Calculate KCalculate Kcc at 303K for SO at 303K for SO2(g)2(g) + +
ClCl2(g)2(g) SO SO22ClCl2(g)2(g) if K if Kpp = 34.5 at = 34.5 at
the temperature.the temperature.
858.23858.23
k 500k 500Consider the equilibriumConsider the equilibrium
NN22 + O + O22 + Br + Br22 2NOBr 2NOBr
Calculate the equilibrium constant KCalculate the equilibrium constant Kpp
for this reaction, given the following for this reaction, given the following information at 298K:information at 298K:
2NO + Br2NO + Br22 2NOBr K 2NOBr Kcc = 2.0 = 2.0
2NO 2NO N N22 + O + O22 K Kcc = 2.1 x 10 = 2.1 x 103030
KKpp = 3.76 x 10 = 3.76 x 10-32-32
Q 100Q 100
If QIf Qcc > K > Kcc, how must the reaction , how must the reaction
proceed to reach equilibrium?proceed to reach equilibrium?
leftleft
Q 200Q 200
What is the difference between Q What is the difference between Q and K?and K?
K uses equilibrium concentrations K uses equilibrium concentrations or partial pressures and Q uses or partial pressures and Q uses
concentrations or partial pressures concentrations or partial pressures at any time.at any time.
Q 300Q 300KKpp for the equilibrium N for the equilibrium N2(g)2(g) + 3H + 3H2(g)2(g)
2NH2NH3(g) 3(g) is 4.51 x 10is 4.51 x 10-5-5 at 450 at 450ooC. Indicate C. Indicate
whether the mixture is at equilibrium. If whether the mixture is at equilibrium. If it is not at equilibrium, indicate the it is not at equilibrium, indicate the
direction in which the reaction must direction in which the reaction must shift to achieve equilibrium.shift to achieve equilibrium.
98 atm NH98 atm NH33, 45 atm N, 45 atm N22, 55 atm H, 55 atm H22
1.28 x 101.28 x 10-3-3 shifts to the left shifts to the left
Q 400Q 400KKpp for the equilibrium N for the equilibrium N2(g)2(g) + 3H + 3H2(g)2(g)
2NH2NH3(g) 3(g) is 4.51 x 10is 4.51 x 10-5-5 at 450 at 450ooC. Indicate C. Indicate
whether the mixture is at equilibrium. If whether the mixture is at equilibrium. If it is not at equilibrium, indicate the it is not at equilibrium, indicate the
direction in which the reaction must direction in which the reaction must shift to achieve equilibrium.shift to achieve equilibrium.
57 atm NH57 atm NH33, 143 atm N, 143 atm N22, and no H, and no H22
0 in denominator, shifts to the left0 in denominator, shifts to the left
Q 500Q 500KKpp for the equilibrium N for the equilibrium N2(g)2(g) + 3H + 3H2(g)2(g)
2NH2NH3(g) 3(g) is 4.51 x 10is 4.51 x 10-5-5 at 450 at 450ooC. C.
Indicate whether the mixture is at Indicate whether the mixture is at equilibrium. If it is not at equilibrium, equilibrium. If it is not at equilibrium,
indicate the direction in which the indicate the direction in which the reaction must shift to achieve reaction must shift to achieve
equilibrium.equilibrium.
13 atm NH13 atm NH33, 27 atm N, 27 atm N22, and 82 atm H, and 82 atm H22
1.14 x 101.14 x 10-5-5 shifts to the right shifts to the right
Calculating Equilibrium Calculating Equilibrium Constants 100Constants 100
An equilibrium mixture in a 2L An equilibrium mixture in a 2L vessel is found to contain 0.0406 vessel is found to contain 0.0406 mol CHmol CH33OH, 0.170 mol CO, and OH, 0.170 mol CO, and
0.302 mol H0.302 mol H22 at 500K. Calculate at 500K. Calculate
KKcc at this temperature. at this temperature.
COCO(g)(g) + 2H + 2H2(g)2(g) CH CH33OHOH(g)(g)
10.4710.47
Calculating Equilibrium Calculating Equilibrium Constants 200Constants 200
The equilibrium NOThe equilibrium NO(g)(g) + Cl + Cl2(g)2(g)
NoClNoCl(g)(g) is established at 500K. An is established at 500K. An
equilibrium mixture of the three equilibrium mixture of the three gases has partial pressures of 0.095 gases has partial pressures of 0.095 atm NO, 0.171 atm Clatm NO, 0.171 atm Cl22, and 0.28 atm , and 0.28 atm
NOCl. Calculate KNOCl. Calculate Kpp for this reaction for this reaction50.850.8
Calculating Equilibrium Calculating Equilibrium Constants 300Constants 300
A flask contains 1.5 atm NA flask contains 1.5 atm N22OO44 and 1 and 1
atm NOatm NO22 and the following and the following
equilibrium is achieved Nequilibrium is achieved N22OO4(g)4(g)
2NO2NO2(g)2(g). After equilibrium is . After equilibrium is
reached, the partial pressure of reached, the partial pressure of NONO22 is 0.512 atm. Calculate the is 0.512 atm. Calculate the
value of Kvalue of Kpp for this reaction. for this reaction.0.15030.1503
Calculating Equilibrium Calculating Equilibrium Constants 400Constants 400
A mixture of 0.2 mol COA mixture of 0.2 mol CO22, 0.1 mol H, 0.1 mol H22, ,
and 0.16 mol Hand 0.16 mol H22O is placed in a 2L O is placed in a 2L
vessel. The following equilibrium is vessel. The following equilibrium is established: COestablished: CO2(g)2(g) + H+ H2(g)2(g)
COCO(g) (g) + H+ H22OO(g)(g). At equilibrium P. At equilibrium PH2OH2O = =
3.51 atm. Calculate K3.51 atm. Calculate Kpp for the for the
reaction at 500K.reaction at 500K.0.110.11
Calculating Equilibrium Calculating Equilibrium Constants 500Constants 500
A mixture of 1.374g HA mixture of 1.374g H22 and 70.31g and 70.31g
BrBr22 is heated in a 2L vessel at is heated in a 2L vessel at
700K. These substances react as 700K. These substances react as follows: Hfollows: H2(g)2(g) + Br + Br2(g)2(g) 2HBr 2HBr(g)(g). At . At
equilibrium the vessel is found to equilibrium the vessel is found to contain 0.566g of Hcontain 0.566g of H22. Calculate K. Calculate Kcc..
67.6167.61
Applications of k 100Applications of k 100
At 100At 100ooC, KC, Kcc = 0.078 for the reaction = 0.078 for the reaction
SOSO22ClCl2(g) 2(g) SO SO2(g) 2(g) + Cl+ Cl2(g)2(g). In an . In an
equilibrium mixture of the three gases, equilibrium mixture of the three gases, the concentrations of SOthe concentrations of SO22ClCl2 2 is 0.180M is 0.180M
and SOand SO22 is 0.052M. What is the is 0.052M. What is the
concentration of Clconcentration of Cl22 in the equilibrium in the equilibrium
mixture?mixture?0.162M0.162M
Applications of k 200Applications of k 200
At 900K the following reaction has KAt 900K the following reaction has Kpp = =
0.345: 2SO0.345: 2SO2(g) 2(g) ++ OO2(g) 2(g) 2SO 2SO3(g)3(g). In . In
an equilibrium mixture the partial an equilibrium mixture the partial pressures of SOpressures of SO22 is 0.135 atm and O is 0.135 atm and O22
is 0.455 atm. What is the equilibrium is 0.455 atm. What is the equilibrium partial pressure of SOpartial pressure of SO33 in the mixture? in the mixture?
0.054 atm0.054 atm
Applications of k 300Applications of k 300
At 373K, KAt 373K, Kpp = 0.416 for the equilibrium = 0.416 for the equilibrium
2NOBr2NOBr(g) (g) 2NO 2NO(g) (g) + Br+ Br2(g)2(g). If the . If the
pressures of NOBrpressures of NOBr(g) (g) and NOand NO(g) (g) are are
equal, what is the equilibrium equal, what is the equilibrium pressure of Brpressure of Br2(g)2(g)??
0.416 atm0.416 atm
Applications of k 400Applications of k 400
At 218At 218ooC, KC, Kcc = 1.2 x 10 = 1.2 x 10-4-4 for the for the
equilibrium NHequilibrium NH44HSHS(s)(s) NH NH3(g) 3(g) + +
HH22SS(g)(g). Calculate the equilibrium . Calculate the equilibrium
concentrations of NHconcentrations of NH33 and H and H22S if a S if a
sample of solid NHsample of solid NH44HS is placed in a HS is placed in a
closed vessel and decomposes until closed vessel and decomposes until equilibrium is reached.equilibrium is reached.
[NH[NH33] = 0.011M, [H] = 0.011M, [H22S] = 0.011MS] = 0.011M
Applications of k 500Applications of k 500
For the equilibrium BrFor the equilibrium Br22 + Cl + Cl22 2BrCl 2BrCl
at 400K, Kat 400K, Kcc = 7.0. If 0.2 mol Br = 7.0. If 0.2 mol Br22 and and
0.25 mol Cl0.25 mol Cl22 are introduced into a 1L are introduced into a 1L
container at 400K, what will be the container at 400K, what will be the equilibrium concentrations of Brequilibrium concentrations of Br22, Cl, Cl22, ,
and BrCl?and BrCl?[Br[Br22] = 0.073 M, [Cl] = 0.073 M, [Cl22] = 0.123 M, ] = 0.123 M,
[BrCl] = 0.254 M[BrCl] = 0.254 M
Le Chatelier’s Principle 100Le Chatelier’s Principle 100Consider 4NHConsider 4NH3(g) 3(g) + O+ O2(g) 2(g) 4NO 4NO(g) (g)
+6H+6H22OO(g)(g), , H = -904.4kJ. How does H = -904.4kJ. How does
increasing [NHincreasing [NH33] affect the yield of ] affect the yield of
NO at equilibrium?NO at equilibrium?
Equilibrium shifts to the right, Equilibrium shifts to the right, so [NO] increases. so [NO] increases.
Le Chatelier’s Principle 200Le Chatelier’s Principle 200
Consider 4NHConsider 4NH3(g) 3(g) + O+ O2(g) 2(g) 4NO 4NO(g) (g)
+6H+6H22OO(g)(g), , H = -904.4kJ. How does H = -904.4kJ. How does
decreasing [Odecreasing [O22] affect the yield of ] affect the yield of
NO at equilibrium?NO at equilibrium? Equilibrium shifts to the left, so Equilibrium shifts to the left, so
[NO] decreases.[NO] decreases.
Le Chatelier’s Principle 300Le Chatelier’s Principle 300
Consider 4NHConsider 4NH3(g) 3(g) + O+ O2(g) 2(g) 4NO 4NO(g) (g)
+6H+6H22OO(g)(g), , H = -904.4kJ. How does H = -904.4kJ. How does
decreasing the volume of the decreasing the volume of the container in which the reaction container in which the reaction occurs affect the yield of NO at occurs affect the yield of NO at
equilibrium?equilibrium?Equilibrium shifts to the left, so Equilibrium shifts to the left, so
[NO] decreses.[NO] decreses.
Le Chatelier’s Principle 400Le Chatelier’s Principle 400
Consider 4NHConsider 4NH3(g) 3(g) + O+ O2(g) 2(g) 4NO 4NO(g) (g)
+6H+6H22OO(g)(g), , H = -904.4kJ. How does H = -904.4kJ. How does
adding a catalyst affect the yield of adding a catalyst affect the yield of NO at equilibrium?NO at equilibrium?
No shift in equilibrium, so No shift in equilibrium, so no change in [NO].no change in [NO].
Le Chatelier’s Principle 500Le Chatelier’s Principle 500
Consider 4NHConsider 4NH3(g) 3(g) + O+ O2(g) 2(g) 4NO 4NO(g) (g)
+6H+6H22OO(g)(g), , H = -904.4kJ. How does H = -904.4kJ. How does
increasing temperature affect the increasing temperature affect the yield of NO at equilibrium?yield of NO at equilibrium?
Equilibrium shifts to the left, so Equilibrium shifts to the left, so [NO] decreases.[NO] decreases.
Surprise 100Surprise 100
At 1000K, KAt 1000K, Kpp = 1.85 for the reaction = 1.85 for the reaction
SOSO2(g)2(g) + 1/2O + 1/2O2(g)2(g) SO SO3(g)3(g). What . What
is the value of Kis the value of Kpp for the reaction for the reaction
SOSO3(g)3(g) SO SO2(g) 2(g) + 1/2O+ 1/2O2(g)2(g)??
0.5410.541
Surprise 200Surprise 200
Consider the following equilibrium: Consider the following equilibrium: 2H2H2(g)2(g) + S + S2(g)2(g) 2H 2H22SS(g) (g) KKcc = 1.08 = 1.08
x 10x 1077 at 700 at 700ooC. Does the C. Does the equilibrium mixture contain mostly equilibrium mixture contain mostly
HH22 and S and S22 or mostly H or mostly H22S?S?
HH22SS
Surprise 300Surprise 300
When 2.00 mol of SOWhen 2.00 mol of SO22ClCl22 is placed in is placed in
a 2L flask at 303K, 56% of the a 2L flask at 303K, 56% of the SOSO22ClCl22 decomposes to SO decomposes to SO22 and and
ClCl22: SO: SO22ClCl2(g)2(g) SO SO2(g) 2(g) + Cl+ Cl2(g)2(g). .
Calculate KCalculate Kcc for this reaction at this for this reaction at this
temperature.temperature.0.7130.713
Surprise 400Surprise 400A mixture of CHA mixture of CH44 and H and H22O is passed O is passed
over a nickel catalyst at 1000K. over a nickel catalyst at 1000K. The emerging gas is collected in a The emerging gas is collected in a
5L falsk and is found to contain 5L falsk and is found to contain 8.62g CO, 2.6g H8.62g CO, 2.6g H22, 43g CH, 43g CH44, and , and
48.4g H48.4g H22O. Assuming that O. Assuming that
equilibrium has been reached, equilibrium has been reached, calculate Kcalculate Kcc for the reaction. for the reaction.
3.74 x 103.74 x 10-3-3
Surprise 500Surprise 500At 80At 80ooC, KC, Kcc = 1.87 x 10 = 1.87 x 10-3-3 for the for the
reaction PHreaction PH33BClBCl3(s)3(s) PH PH3(g) 3(g) + +
BClBCl3(g)3(g). Calculate the equilibrium . Calculate the equilibrium
concentrations of PHconcentrations of PH33 and BCl and BCl33 if a if a
solid sample of PHsolid sample of PH33BClBCl33 is placed is placed
in a closed vessel and in a closed vessel and decomposes until equilibrium is decomposes until equilibrium is
reached.reached.[PH[PH33] = 0.043M, [BCl] = 0.043M, [BCl33] = 0.043M] = 0.043M