Question
In: Chemistry
The equilibrium constant K=0.36 for the reaction PCl5 (g) PCl3 (g) +Cl2 (g). (a) Given...
The equilibrium constant K=0.36 for the reaction PCl5 (g) PCl3 (g) +Cl2 (g). (a) Given that 2.0 g of PCl5 was initially placed in the reaction chamber of volume 250 cm3, determine the molar concentration in the mixture at equilibrium. (b) What is the percentage of PCl5 decomposed.
Solutions
Expert Solution
PCl5 moles = mass / Molar mass of PCl5 = ( 2g) / ( 208.24g/mol) = 0.0096
volume = 250 cm3 = 250 ml = 0.25L
[PCl5] = ( 0.0096/0.25) = 0.0384 M
PCl5 (g) <------> PCl3 (g) + Cl2 (g)
Initial 0.0384 0 0
equilibrium 0.0384 -X X X
Kc = [PCl3] [Cl2] /[PCl5]
0.36 = ( X^2) / ( 0.0384-X)
X^2 + 0.36X - 0.01383 = 0
X = 0.035
at equilibrium [PCl3] =[Cl2] = 0.035M
[PCl5] = 0.0384-0.035 = 0.0034 M
b) % of PCl5 decomposed = 100 x ( PCl5 decomposed (i,e X) / PCl5 initial amount)
( 100 x 0.035/0.0384) = 91.15 %
queen_honey_blossom answered 2 years agoRelated Solutions
1.For the reaction, PCl5(g) <-----> PCl3(g) + Cl2(g) Kp = 24.6 at 500 K calculate the equilibrium...
1.For the reaction,
PCl5(g) <-----> PCl3(g) +
Cl2(g) Kp
= 24.6 at 500 K
calculate the equilibrium partial pressures of the reactants and
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0.610 atm, PPCl3 = 0.400 atm and
PCl2 = 0.000 atm.
PPCl5 = PPCl3 =
PCl2 =
2.
H2O(g) + Cl2O(g) <----->
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calculate the equilibrium concentrations of the reactants and
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9. The equilibrium constant Kc for the reaction PCl3(g) + Cl2(g) PCl5(g) is 49 at 230°C....
9. The equilibrium constant Kc for the reaction PCl3(g) +
Cl2(g) PCl5(g) is 49 at 230°C. If 0.70 mol of PCl3 is
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is the concentration of PCl3 when equilibrium has been
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A. 0.049 M
B. 0.11 M
C. 0.30 M
D. 0.59 M
E. 0.83 M
The equilibrium constant for the reaction PCl3(g) + Cl2(g) ------- PCl5(g) equals 49 at 230°C. If 0.367...
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Cl2(g) ------- PCl5(g)
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The equilibrium constant, K, for the following reaction is 1.87×10-2 at 511 K. PCl5(g) <--------->>>PCl3(g) +...
The equilibrium constant, K, for the following reaction is
1.87×10-2 at 511
K.
PCl5(g)
<--------->>>PCl3(g) +
Cl2(g)
An equilibrium mixture of the three gases in a
13.1 L container at 511 K
contains 0.209 M PCl5,
6.24×10-2 M
PCl3 and
6.24×10-2 M
Cl2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if the
equilibrium mixture is compressed at constant temperature to a
volume of 7.01 L?
[PCl5]
=
M
[PCl3]
=
M
[Cl2]
=...
The equilibrium constant, K, for the following reaction is 1.42×10-2 at 504 K. PCl5(g) --> PCl3(g)...
The equilibrium constant, K, for the following reaction is
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PCl5(g) --> PCl3(g) + Cl2(g)
An equilibrium mixture of the three gases in a 10.9 L container
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equilibrium has been reestablished, if the equilibrium mixture is
compressed at constant temperature to a volume of 4.95 L?
[PCl5] = M
[PCl3] = M
[Cl2]...
The equilibrium constant, K, for the following reaction is 3.16×10-2 at 525 K. PCl5(g) <----->PCl3(g) +...
The equilibrium constant, K, for the following reaction is
3.16×10-2 at 525
K.
PCl5(g)
<----->PCl3(g) +
Cl2(g)
An equilibrium mixture of the three gases in a
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contains 0.243 M PCl5,
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8.77×10-2 M
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the three gases once equilibrium has been reestablished, if the
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[PCl5]
=
M
[PCl3]
=
M
[Cl2]
=
M
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The equilibrium constant, K, for the following reaction is
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of the three gases in a 1.00 L flask at 500 K contains 0.218 M
PCl5, 5.11×10-2 M PCl3 and 5.11×10-2 M Cl2. What will be the
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reestablished, if 3.92×10-2 mol of PCl3(g) is added to the flask?
[PCl5] = M
[PCl3] = M
[Cl2] = M
The equilibrium constant, K, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) PCl3(g) +...
The equilibrium constant, K, for the following reaction is
1.20×10-2 at 500 K. PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture
of the three gases in a 1.00 L flask at 500 K contains 0.200 M
PCl5, 4.90×10-2 M PCl3 and 4.90×10-2 M Cl2. What will be the
concentrations of the three gases once equilibrium has been
reestablished, if 3.12×10-2 mol of Cl2(g) is added to the
flask?
[PCl5] =
[PCl3] =
[Cl2] =
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g)...
The equilibrium constant, Kp, for the following
reaction is 2.01 at 500 K:
PCl3(g) +
Cl2(g)
<----->PCl5(g)
Calculate the equilibrium partial pressures of all species when
PCl3 and
Cl2, each at an intitial partial
pressure of 1.56 atm, are introduced into an
evacuated vessel at 500 K.
PPCl3
=
atm
PCl2
=
atm
PPCl5
=
atm
The equilibrium constant, Kp, for the following reaction is 2.01 at 500 K: PCl3(g) + Cl2(g)...
The equilibrium constant, Kp, for the following
reaction is 2.01 at 500 K:
PCl3(g) +
Cl2(g)
<<<----->>PCl5(g)
Calculate the equilibrium partial pressures of all species when
PCl3 and
Cl2, each at an intitial partial
pressure of 1.01 atm, are introduced into an
evacuated vessel at 500 K.
PPCl3
=
atm
PCl2
=
atm
PPCl5
=
atm
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