Question
In: Chemistry
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 . 3. In order to reach equilibrium NO must be consumed . 4. Qc is greater than Kc. 5. The reaction is at equilibrium. No further reaction will occur.
Solutions
Expert Solution
4. Qc = 3.367*10^-3 , Qc<Kc Ans: statement is 'False'
5. At equilibruim no net reaction takes place but further reaction takes place in both forward and backward direction. Ans: statement is 'False".
queen_honey_blossom answered 2 years agoRelated Solutions
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...
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....
The equilibrium constant, Kc, for the following reaction is 6.50×10-3 at 298K. 2NOBr(g)<====> 2NO(g) + Br2(g)...
The equilibrium constant, Kc, for the following reaction
is 6.50×10-3 at
298K.
2NOBr(g)<====>
2NO(g) +
Br2(g)
If an equilibrium mixture of the three gases in a
16.4 L container at 298K contains
0.383 mol of NOBr(g) and
0.230 mol of NO, the equilibrium
concentration of Br2 is____M
The equilibrium constant, Kc , for the following
reaction is 7.00×10-5 at
673 K.
NH4I(s)
<====>NH3(g) +
HI(g)
If an equilibrium mixture of the three compounds in a
5.04 L container at 673...
The equilibrium constant, Kc, for the following reaction is 1.05×10-3 at 446 K. PCl5(g) PCl3(g) +...
The equilibrium constant, Kc, for the following reaction is
1.05×10-3 at 446 K. PCl5(g) PCl3(g) + Cl2(g) When a sufficiently
large sample of PCl5(g) is introduced into an evacuated vessel at
446 K, the equilibrium concentration of Cl2(g) is found to be 0.498
M. Calculate the concentration of PCl5 in the equilibrium mixture.
____M
_______________________________________________________________________________________________________________
A student ran the following reaction in the laboratory at 689 K:
N2(g) + 3H2(g) 2NH3(g) When she introduced 4.06×10-2 moles of N2(g)
and 5.20×10-2...
1. The decomposition reaction of NOBr(g) to 2 NO(g) and Br2(g) is second order with k...
1. The decomposition reaction of NOBr(g) to 2 NO(g) and Br2(g)
is second order with k = 0.90
M-1∙s-1.
2 NOBr(g) …….> 2 NO(g) + Br2(g)
What is the half-life of this reaction if the initial
concentration of NOBr is 0.78 M?
2. The decomposition reaction of NOBr(g) to 2 NO(g) and Br2(g)
is second order with k = 0.90
M-1∙s-1.
2 NOBr(g) …….> 2 NO(g) + Br2(g)
How much time would pass before a 4.00 g sample of NOBr...
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) ---> H2(g)...
The equilibrium constant, Kc, for the following reaction is
1.80×10-2 at 698 K.
2HI(g) ---> H2(g) + I2(g)
Calculate the equilibrium concentrations of reactant and
products when 0.384 moles of HI are introduced into a 1.00 L vessel
at 698 K.
[HI] = M
[H2] = M
[I2] = M
The equilibrium constant, Kc, for the following reaction is 1.80×10-2 at 698 K. 2HI(g) -->H2(g) +...
The equilibrium constant, Kc, for the following
reaction is 1.80×10-2 at
698 K.
2HI(g)
-->H2(g) +
I2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.257 moles of HI are
introduced into a 1.00 L vessel at 698
K.
[HI]
=
M
[H2]
=
M
[I2]
=
M
The equilibrium constant, Kc, for the following
reaction is 83.3 at 500 K.
PCl3(g) +
Cl2(g)
-->PCl5(g)
Calculate the equilibrium concentrations of reactant and products
when 0.420 moles of
PCl3 and...
Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is...
Consider the following reaction occurring at 298 K:
N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is not
spontaneous under standard conditions by calculating ΔG∘rxn.
Part B If a reaction mixture contains only N2O and NO2 at
partial pressures of 1.0 atm each, the reaction will be spontaneous
until some NO forms in the mixture. What maximum partial pressure
of NO builds up before the reaction ceases to be spontaneous?
Part C What temperature is required to make the reaction
spontaneous...
1) The equilibrium constant, Kc, for the following reaction is 1.20×10-2 at 500 K. PCl5(g) <---...
1) The equilibrium constant, Kc, for the following reaction is
1.20×10-2 at 500 K. PCl5(g) <--- --->PCl3(g) + Cl2(g)
Calculate the equilibrium concentrations of reactant and products
when 0.279 moles of PCl5(g) are introduced into a 1.00 L vessel at
500 K. [PCl5] = M [PCl3] = M [Cl2] = M 2) The equilibrium constant,
Kc, for the following reaction is 55.6 at 698 K. H2 (g) + I2 (g)
<---- ----> 2 HI (g) Calculate the equilibrium concentrations
of...
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