Question
In: Chemistry
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?
Solutions
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 0.315 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
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,...
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.)
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]
=...
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
1.42×10-2 at 504 K.
PCl5(g) --> PCl3(g) + Cl2(g)
An equilibrium mixture of the three gases in a 10.9 L container
at 504 K contains 0.279 M PCl5, 6.29×10-2 M PCl3 and 6.29×10-2 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 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
4.56 L container at 525 K
contains 0.243 M PCl5,
8.77×10-2 M
PCl3 and
8.77×10-2 M
Cl2. What will be the concentrations of
the three gases once equilibrium has been reestablished, if the
volume of the container is increased to 10.3
L?
[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 0.218 M
PCl5, 5.11×10-2 M PCl3 and 5.11×10-2 M Cl2. What will be the
concentrations of the three gases once equilibrium has been
reestablished, if 3.92×10-2 mol of PCl3(g) is added to the flask?
[PCl5] = M
[PCl3] = M
[Cl2] = M
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