Question
In: Chemistry
The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) +...
The equilibrium constant, K, for the following reaction is
1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at 600 K contains 0.315 M COCl2, 6.38×10-2 M CO and 6.38×10-2 M Cl2. What will be the concentrations of the three gases once equilibrium has been reestablished, if 3.31×10-2 mol of Cl2(g) is added to the flask?
[COCl2] =____ M [CO] =____ M [Cl2] = ____M
Solutions
Expert Solution
CoCl2 
CO + Cl2
initial concentration: a 0 0
first equilibrium concentration: a-x x x
.315 moles 6.38*10-2 6.38*10-2 (given in question) K=1.29*10-2
after adding n moles = 3.31*10-2moles of Cl2 equilibrim shifts to right , whereas equilibrium constant remains same
new equilibrium concentration a-x+n x-n x+n
therefore,
[COCl2] = a-x+n= .315+3.31*10-2= .3481 moles
[CO]= x-n = 6.38*10-2- 3.31*10-2= 6.07*10-2
[Cl2] = x+n = 6.38*10-2+3.31*10-2 = 9.69*10-2
queen_honey_blossom answered 2 years agoRelated Solutions
The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) CO(g) +...
The equilibrium constant, K, for the following reaction is
1.29×10-2 at 600 K. COCl2(g) CO(g) + Cl2(g) An equilibrium mixture
of the three gases in a 1.00 L flask at 600 K contains 0.294 M
COCl2, 6.16×10-2 M CO and 6.16×10-2 M Cl2. What will be the
concentrations of the three gases once equilibrium has been
reestablished, if 4.50×10-2 mol of CO(g) is added to the flask?
[COCl2] = M
[CO] = M
[Cl2] = M
1) The equilibrium constant, K, for the following reaction is 1.29×10-2 at 600 K. COCl2(g) <---...
1) The equilibrium constant, K, for the following reaction is
1.29×10-2 at 600
K.
COCl2(g) <--- --->
CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
600 K contains 0.206
M COCl2,
5.16×10-2 M CO and
5.16×10-2M
Cl2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
2.88×10-2 mol of CO(g)
is added to the flask?
[COCl2]
=
M
[CO]
=
M
[Cl2]
=
M
2) The equilibrium constant,...
The equilibrium constant, K, for the following reaction is 3.35×10-2 at 629 K. COCl2(g) <---->CO(g) +...
The equilibrium constant, K, for the following reaction is
3.35×10-2 at 629 K.
COCl2(g) <---->CO(g) + Cl2(g)
An equilibrium mixture of the three gases in a 11.0 L container
at 629 K contains 0.217 M COCl2, 8.52×10-2 M CO and 8.52×10-2 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 5.95 L?
The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K: CO(g) + Cl2(g)...
The equilibrium constant, Kp, for the following reaction is 1.57
at 600 K:
CO(g) + Cl2(g) COCl2(g)
Calculate the equilibrium partial pressures of all species when
CO and Cl2, each at an intitial partial pressure of 1.65 atm, are
introduced into an evacuated vessel at 600 K.
PCO = ______ atm
PCl2= _______ atm
PCOCl2 = _______ atm
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g)...
The equilibrium constant, Kc, for the following reaction is 77.5
at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium
concentrations of reactant and products when 0.576 moles of CO and
0.576 moles of Cl2 are introduced into a 1.00 L vessel at 600
K.
[CO] = M
[Cl2] = M
[COCl2] = M
At 100.0 C, the equilibrium constant for the reaction: CO (g) + Cl2 (g) <--> COCl2...
At 100.0 C, the equilibrium constant for the reaction: CO (g) +
Cl2 (g) <--> COCl2 (g) has a value of
4.6 x 109. If 0.40 mol of COCl2 is placed
into a 10.0 L flask at 100.0 C, what will be the equilibrium
concentration of all species? (A simplifying approximation that
will make the solution of the resulting equation easier is to note
that x is much less than 0.040mol/L. This means that 0.040 -x is
approximately 0.040.)
Consider the following reaction where Kp = 1.57 at 600 K: CO(g) + Cl2(g) COCl2(g) If...
Consider the following reaction where Kp = 1.57 at 600 K: CO(g)
+ Cl2(g) COCl2(g) If the three gases are mixed in a rigid container
at 600 K so that the partial pressure of each gas is initially one
atm, what will happen?
Indicate True (T) or False (F) for each of the following:
1. A reaction will occur in which COCl2(g) is produced
2. Kp will decrease.
3. A reaction will occur in which CO is produced.
4. Q...
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) <----->H2(g) +...
The equilibrium constant, K, for the following reaction is
1.80×10-2 at 698
K.
2HI(g)
<----->H2(g) +
I2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
698 K contains 0.322 M
HI, 4.32×10-2 M
H2 and
4.32×10-2 M
I2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
3.12×10-2 mol of
I2(g) is added to the flask?
[HI]
=
M
[H2]
=
M
[I2]
=
M
The equilibrium constant, K, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) <----><H2(g) +...
The equilibrium constant, K, for the following reaction is
1.80×10-2 at 698
K.
2HI(g)
<----><H2(g) +
I2(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
698 K contains 0.307 M
HI,
4.13×10-2 M
H2 and
4.13×10-2 M
I2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if
0.173 mol of HI(g) is added to
the flask?
[HI]
=
M
[H2]
=
M
[I2]
=
M
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]
=...
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