Consider the following gas-phase reaction: 2 A ( g ) + B ( g ) ⇌ C ( g ) + D ( g ) . An equilibrium mixture of reactants and products is subjected to the following changes: A decrease in volume An increase in temperature Addition of reactants Addition of a catalyst Addition of an inert gas Which of these changes affect the composition of the equilibrium mixture but leave the value of the equilibrium constant K c unchanged? Which of the changes affect the value of K c ? Which affect neither the composition of the equilibrium mixture nor K c ?
Consider the following gas-phase reaction: 2 A ( g ) + B ( g ) ⇌ C ( g ) + D ( g ) . An equilibrium mixture of reactants and products is subjected to the following changes: A decrease in volume An increase in temperature Addition of reactants Addition of a catalyst Addition of an inert gas Which of these changes affect the composition of the equilibrium mixture but leave the value of the equilibrium constant K c unchanged? Which of the changes affect the value of K c ? Which affect neither the composition of the equilibrium mixture nor K c ?
Solution Summary: The author explains that a chemical reaction is said to be in equilibrium if there is no further change in its concentration with time.
Consider the following gas-phase reaction:
2
A
(
g
)
+
B
(
g
)
⇌
C
(
g
)
+
D
(
g
)
.
An equilibrium mixture of reactants and products is subjected to the following changes:
A decrease in volume
An increase in temperature
Addition of reactants
Addition of a catalyst
Addition of an inert gas
Which of these changes affect the composition of the equilibrium mixture but leave the value of the equilibrium constant
K
c
unchanged? Which of the changes affect the value of
K
c
? Which affect neither the composition of the equilibrium mixture nor
K
c
?
Are there any alternative methods better than the MOHR titration to quantitatively determine salt in a sample?
hybridization of nitrogen of complex molecules
Using reaction free energy to predict equilibrium composition
Consider the following equilibrium:
2NO2 (g) = N2O4(g)
AGº = -5.4 kJ
Now suppose a reaction vessel is filled with 4.53 atm of dinitrogen tetroxide (N2O4) at 279. °C. Answer the following questions about this system:
Under these conditions, will the pressure of N2O4 tend to rise or fall?
Is it possible to reverse this tendency by adding NO2?
In other words, if you said the pressure of N2O4 will tend to rise, can that
be changed to a tendency to fall by adding NO2? Similarly, if you said the
pressure of N2O4 will tend to fall, can that be changed to a tendency to
'2'
rise by adding NO2?
If you said the tendency can be reversed in the second question, calculate
the minimum pressure of NO 2 needed to reverse it.
Round your answer to 2 significant digits.
00
rise
☐ x10
fall
yes
no
☐ atm
G
Ar
1
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