Question
In: Chemistry
Consider the following reaction where Kc = 10.5 at 350 K: 2 CH2Cl2 (g) CH4 (g)...
Consider the following reaction where Kc = 10.5 at 350 K:
2 CH2Cl2 (g) CH4 (g) + CCl4 (g)
A reaction mixture was found to contain 1.22×10-2 moles of CH2Cl2 (g), 5.20×10-2 moles of CH4 (g), and 4.18×10-2 moles of CCl4 (g), in a 1.00 liter container.
Indicate True (T) or False (F) for each of the following:
1. In order to reach equilibrium CH2Cl2(g) must be consumed .
2. In order to reach equilibrium Kc must increase .
3. In order to reach equilibrium CH4 must be consumed .
4. Qc is less than Kc.
5. The reaction is at equilibrium. No further reaction will occur.
Solutions
queen_honey_blossom answered 2 years agoRelated Solutions
The equilibrium constant, Kc, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) ------CH4(g) +...
The equilibrium constant, Kc, for the following reaction is 10.5
at 350 K.
2CH2Cl2(g) ------CH4(g) + CCl4(g)
Calculate the equilibrium concentrations of reactant and
products when 0.321 moles of CH2Cl2 are introduced into a 1.00 L
vessel at 350 K.
[CH2Cl2] = ------------M
[CH4] = ------- M
[CCl4] = ------ M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) CH4(g) +...
The equilibrium constant, K, for the following reaction is 10.5
at 350 K.
2CH2Cl2(g) CH4(g) + CCl4(g) An equilibrium mixture of the three
gases in a 1.00 L flask at 350 K contains 5.47×10-2 M CH2Cl2, 0.177
M CH4 and 0.177 M CCl4. What will be the concentrations of the
three gases once equilibrium has been reestablished, if 3.44×10-2
mol of CH2Cl2(g) is added to the flask?
[CH2Cl2] =_____ M
[CH4] = ________M
[CCl4] =________ M
The equilibrium constant, K, for the following reaction is 10.5 at 350 K. 2CH2Cl2(g) =CH4(g) +...
The equilibrium constant, K, for the following reaction is
10.5 at 350 K.
2CH2Cl2(g)
=CH4(g) +
CCl4(g)
An equilibrium mixture of the three gases in a 1.00 L flask at
350 K contains
5.12×10-2 M
CH2Cl2,
0.166 M CH4 and
0.166 M CCl4. What
will be the concentrations of the three gases once equilibrium has
been reestablished, if 0.121 mol of
CH4(g) is added to the flask?
[CH2Cl2]
=
_________M
[CH4]
=
_________ M
[CCl4]
=
_________ M
1. The equilibrium constant, Kp, for the following reaction is 10.5 at 350 K: 2CH2Cl2(g) <--->CH4(g)...
1. The equilibrium constant, Kp, for the following
reaction is 10.5 at 350 K:
2CH2Cl2(g)
<--->CH4(g) +
CCl4(g)
Calculate the equilibrium partial pressures of all species when
CH2Cl2(g) is introduced into
an evacuated flask at a pressure of 0.865 atm at
350 K.
PCH2Cl2
=____
atm
PCH4
=____
atm
PCCl4
=____
atm
2. The equilibrium constant, Kp, for the following
reaction is 0.215 at 673 K:
NH4I(s) <---->
NH3(g) + HI(g)
Calculate the equilibrium partial pressure of HI
when 0.413...
Consider the following reaction where Kc = 6.50×10-3 at 298 K 2 NOBr (g)-> 2 NO...
Consider the following reaction where Kc = 6.50×10-3 at 298
K
2 NOBr (g)-> 2 NO (g) + Br2 (g)
A reaction mixture was found to contain 8.52×10-2 moles of NOBr
(g), 2.31×10-2 moles of NO (g), and 4.58×10-2 moles of Br2 (g), in
a 1.00 liter container. Indicate True (T) or False (F) for each of
the following:
1. In order to reach equilibrium NOBr(g) must be consumed . 2.
In order to reach equilibrium Kc must increase ....
The equilibrium constant, Kc, for the following reaction is 33.3 at 297 K. 2CH2Cl2(g) <-------->>>CH4(g) +...
The equilibrium constant, Kc, for the following
reaction is 33.3 at 297 K.
2CH2Cl2(g)
<-------->>>CH4(g) +
CCl4(g)
When a sufficiently large sample of
CH2Cl2(g) is introduced into
an evacuated vessel at 297 K, the equilibrium
concentration of CCl4(g) is found to be
0.322 M.
Calculate the concentration of
CH2Cl2 in the equilibrium
mixture. M
The equilibrium constant, Kc, for the following reaction is 41.1 at 289 K. 2CH2Cl2(g) --> CH4(g)...
The equilibrium constant, Kc, for the following
reaction is 41.1 at 289 K.
2CH2Cl2(g)
--> CH4(g) +
CCl4(g)
When a sufficiently large sample of
CH2Cl2(g) is introduced into
an evacuated vessel at 289 K, the equilibrium
concentration of CCl4(g) is found to be
0.202 M.
Calculate the concentration of
CH2Cl2 in the equilibrium
mixture. ? M
2)The equilibrium constant, Kc, for the following
reaction is 1.80×10-2 at
698 K.
Calculate Kp for this reaction at this
temperature.
2HI(g) -->
H2(g)...
The reaction CH2Cl2 (g) --> CH4 (g) + CCl4 (g) has Kp = 1.33 at 400K....
The reaction CH2Cl2 (g) --> CH4 (g) + CCl4 (g) has Kp = 1.33
at 400K. A 5.00L reaction vessel is evacuated, and 15.00 g of
CH2Cl2 (l) is added to the flask. The CH2Cl2 (l) rapidly vaporizes
and the reaction starts. a. What will be all of the partial
pressures of the gases when equilibrium is reached? b. Sketch a
graph showing the initial concentration of each gas and how they
change as the mixture approaches equilibrium. Set-up your...
Consider the following reaction where Kc = 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) A...
Consider the following reaction where Kc =
1.80×10-4 at 298
K.
NH4HS(s)
NH3(g) +
H2S(g)
A reaction mixture was found to contain
5.91×10-2 moles of
NH4HS(s),
8.61×10-3 moles of
NH3(g), and
1.34×10-2 moles of
H2S(g), in a 1.00 liter
container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach
equilibrium?
The reaction quotient, Qc, equals
____________.
The reaction _____________
A. must run in the forward direction to reach
equilibrium.
B. must run in...
Consider the following reaction where Kc = 1.80×10-4 at 298 K. NH4HS(s) NH3(g) + H2S(g) A...
Consider the following reaction where Kc =
1.80×10-4 at 298
K.
NH4HS(s)
NH3(g) +
H2S(g)
A reaction mixture was found to contain
5.64×10-2 moles of
NH4HS(s),
8.66×10-3 moles of
NH3(g), and
1.34×10-2 moles of
H2S(g), in a 1.00 liter
container.
Is the reaction at equilibrium?
If not, what direction must it run in order to reach
equilibrium?
The reaction quotient, Qc, equals
.=_____________
The reaction____________________________
A. must run in the forward direction to reach
equilibrium.
B. must run in the...
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