654 Chapter 14 Chemicat Euse 14.76 Amixtore of t 47 mote or , nd 3.59 motes of ICT 14.84 The equilibris ** heated to 2800 C Calculate the equilibrium par ial pressures of H Cl. and HCI if the total pres- sure is 2.00 atm. For the reaction tion is 4.31 x H,C) + ClCe) 2HCICR) In a certe 0.862 atm volume ve A is 193 at 2800 C. 1477 When heated at high temperatures, iodine vapor dis- sociates as follows: 14.85 A quan heated graphi equilit (R) 21(g) In one experiment, a chemist finds that when 0.054 mole of I, was placed in a flask of volume 0.48 L at 587 K, the degree of dissociation (that is, the fraction of I, dissociated) was 0.0252. Calculate K and Kp for the reaction at this temperature. 14.78 One mole of N, and three moles of H2 are placed in a flask at 375°C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31 × 10*. 14.79 At 1130°C the equilibrium constant (K.) for the Und the tio pr is 14.86 reaction 2H,S(g) = 2H2(g) + S2(g) is 2.25 x 10-4. If [H,S] = 4.84 × 10~3M and [H2]= 1.50 × 10¬³ M, calculate [S2]. 14.80 A quantity of 6.75 g of SO2C12 was placed in a 2.00-L flask. At 648 K, there is 0.0345 mole of SO2 present. Calculate K. for the reaction eriw SO,Cl2(g) SO2(g) + Cl2(g) 14 14.81 The formation of SO3 from SO, and O, is an inter- mediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant Kp for the reaction 2SO2(g) + O2(g) = 2SO3(g) ds9 is 0.13 at 830°C. In one experiment 2.00 mol SO2 and 2.00 mol O, were initially present in a flask. wWhat must the total pressure at equilibrium be in order to have an 80.0 percent yield of SO,? 82 Consider the dissociation of iodine: HW#13
654 Chapter 14 Chemicat Euse 14.76 Amixtore of t 47 mote or , nd 3.59 motes of ICT 14.84 The equilibris ** heated to 2800 C Calculate the equilibrium par ial pressures of H Cl. and HCI if the total pres- sure is 2.00 atm. For the reaction tion is 4.31 x H,C) + ClCe) 2HCICR) In a certe 0.862 atm volume ve A is 193 at 2800 C. 1477 When heated at high temperatures, iodine vapor dis- sociates as follows: 14.85 A quan heated graphi equilit (R) 21(g) In one experiment, a chemist finds that when 0.054 mole of I, was placed in a flask of volume 0.48 L at 587 K, the degree of dissociation (that is, the fraction of I, dissociated) was 0.0252. Calculate K and Kp for the reaction at this temperature. 14.78 One mole of N, and three moles of H2 are placed in a flask at 375°C. Calculate the total pressure of the system at equilibrium if the mole fraction of NH3 is 0.21. The Kp for the reaction is 4.31 × 10*. 14.79 At 1130°C the equilibrium constant (K.) for the Und the tio pr is 14.86 reaction 2H,S(g) = 2H2(g) + S2(g) is 2.25 x 10-4. If [H,S] = 4.84 × 10~3M and [H2]= 1.50 × 10¬³ M, calculate [S2]. 14.80 A quantity of 6.75 g of SO2C12 was placed in a 2.00-L flask. At 648 K, there is 0.0345 mole of SO2 present. Calculate K. for the reaction eriw SO,Cl2(g) SO2(g) + Cl2(g) 14 14.81 The formation of SO3 from SO, and O, is an inter- mediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. The equilibrium constant Kp for the reaction 2SO2(g) + O2(g) = 2SO3(g) ds9 is 0.13 at 830°C. In one experiment 2.00 mol SO2 and 2.00 mol O, were initially present in a flask. wWhat must the total pressure at equilibrium be in order to have an 80.0 percent yield of SO,? 82 Consider the dissociation of iodine: HW#13
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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14.80
![654
Chapter 14 Chemicat Euse
14.76 Amixtore of t 47 mote or , nd 3.59 motes of ICT
14.84 The equilibris
** heated to 2800 C Calculate the equilibrium par
ial pressures of H Cl. and HCI if the total pres-
sure is 2.00 atm. For the reaction
tion is 4.31 x
H,C) + ClCe) 2HCICR)
In a certe
0.862 atm
volume ve
A is 193 at 2800 C.
1477 When heated at high temperatures, iodine vapor dis-
sociates as follows:
14.85 A quan
heated
graphi
equilit
(R) 21(g)
In one experiment, a chemist finds that when
0.054 mole of I, was placed in a flask of volume
0.48 L at 587 K, the degree of dissociation (that is,
the fraction of I, dissociated) was 0.0252. Calculate
K and Kp for the reaction at this temperature.
14.78 One mole of N, and three moles of H2 are placed in
a flask at 375°C. Calculate the total pressure of the
system at equilibrium if the mole fraction of NH3 is
0.21. The Kp for the reaction is 4.31 × 10*.
14.79 At 1130°C the equilibrium constant (K.) for the
Und
the
tio
pr
is
14.86
reaction
2H,S(g) = 2H2(g) + S2(g)
is 2.25 x 10-4. If [H,S] = 4.84 × 10~3M and [H2]=
1.50 × 10¬³ M, calculate [S2].
14.80
A quantity of 6.75 g of SO2C12 was placed in a
2.00-L flask. At 648 K, there is 0.0345 mole of SO2
present. Calculate K. for the reaction
eriw
SO,Cl2(g)
SO2(g) + Cl2(g)
14
14.81
The formation of SO3 from SO, and O, is an inter-
mediate step in the manufacture of sulfuric acid, and
it is also responsible for the acid rain phenomenon.
The equilibrium constant Kp for the reaction
2SO2(g) + O2(g) = 2SO3(g)
ds9 is 0.13 at 830°C. In one experiment 2.00 mol SO2
and 2.00 mol O, were initially present in a flask.
wWhat must the total pressure at equilibrium be in
order to have an 80.0 percent yield of SO,?
82 Consider the dissociation of iodine:
HW#13](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdce7689d-4520-4a5f-90cf-3f573cfd3075%2F11c30a81-43ad-4cec-b608-0cfb746e0e03%2Ftxzljuq.jpeg&w=3840&q=75)
Transcribed Image Text:654
Chapter 14 Chemicat Euse
14.76 Amixtore of t 47 mote or , nd 3.59 motes of ICT
14.84 The equilibris
** heated to 2800 C Calculate the equilibrium par
ial pressures of H Cl. and HCI if the total pres-
sure is 2.00 atm. For the reaction
tion is 4.31 x
H,C) + ClCe) 2HCICR)
In a certe
0.862 atm
volume ve
A is 193 at 2800 C.
1477 When heated at high temperatures, iodine vapor dis-
sociates as follows:
14.85 A quan
heated
graphi
equilit
(R) 21(g)
In one experiment, a chemist finds that when
0.054 mole of I, was placed in a flask of volume
0.48 L at 587 K, the degree of dissociation (that is,
the fraction of I, dissociated) was 0.0252. Calculate
K and Kp for the reaction at this temperature.
14.78 One mole of N, and three moles of H2 are placed in
a flask at 375°C. Calculate the total pressure of the
system at equilibrium if the mole fraction of NH3 is
0.21. The Kp for the reaction is 4.31 × 10*.
14.79 At 1130°C the equilibrium constant (K.) for the
Und
the
tio
pr
is
14.86
reaction
2H,S(g) = 2H2(g) + S2(g)
is 2.25 x 10-4. If [H,S] = 4.84 × 10~3M and [H2]=
1.50 × 10¬³ M, calculate [S2].
14.80
A quantity of 6.75 g of SO2C12 was placed in a
2.00-L flask. At 648 K, there is 0.0345 mole of SO2
present. Calculate K. for the reaction
eriw
SO,Cl2(g)
SO2(g) + Cl2(g)
14
14.81
The formation of SO3 from SO, and O, is an inter-
mediate step in the manufacture of sulfuric acid, and
it is also responsible for the acid rain phenomenon.
The equilibrium constant Kp for the reaction
2SO2(g) + O2(g) = 2SO3(g)
ds9 is 0.13 at 830°C. In one experiment 2.00 mol SO2
and 2.00 mol O, were initially present in a flask.
wWhat must the total pressure at equilibrium be in
order to have an 80.0 percent yield of SO,?
82 Consider the dissociation of iodine:
HW#13
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