Question

1. Read the Chapter on Chemical Equilibrium: In particular, read the section on the Le Chatelier Principle, as it relates to the effects of concentration, pressure/volume, and temperature on the position of a chemical equilibrium. 2. Solve the following related problems involving the equilibrium between dinitrogen tetroxide and nitrogen dioxide. N2O4 <==> 2 NO2 The equilibrium constant for this reaction is Kp = 0.60 at 350 degrees Kelvin. A 1.0 L vessel contains the above two gases in equilibrium at 350 K. The total pressure of the two gases, P(NO2) + P(N2O4), in the vessel is 0.50 atm. From this information, calculate the equilibrium partial pressure for each gas. This is the initial equilibrium position for the reaction, which you will use to consider the effects of the following perturbations. This equilibrium mixture is subjected to the following four perturbations: a. addition of N2O4 gas to the vessel (which had been at the above equilibrium) to give a total concentration (before readjustment of the equilibrium position) of 0.375 atm in the reactant gas; b. decreasing the total volume of the vessel to 0.50 L (in answering b-d, go back to the initial equilibrium mixture before then applying the perturbation); c. increasing the total pressure inside the vessel to 1.5 atm by adding 1.0 atm of N2 gas; d. increasing the temperature of the gas mixture to 700 degrees K, a temperature at which the equilibrium constant is 2.40. 3. Hints: Note that the equilibrium constant is a Kp value and that reactant and product concentrations are given in terms of partial pressures. For each of these perturbations, you can solve for the equilibrium partial pressures of the two gases. To do this you may have to set up an ICE table. Note that in �b�, the inverse relationship between P and V in the ideal gas law allows you to easily determine the partial pressures of the reactant and product gases immediately after the volume increase. Then you can calculate the final equilibrium concentrations following this perturbation. Finally, the exact solution to part �d� is challenging. You should first consider the effect, on the partial pressures of the reactant and product gases, of an increase in temperature from 350 to 700 degrees K. (Remember that the ideal gas law indicates a direct proportionality of P and T.) Then you should consider a shift in the equilibrium concentrations, along with the new equilibrium constant for the higher temperature.

Answer #1

At a particular temperature, Kp = 0.26 for the reaction below.
N2O4(g) equilibrium reaction arrow 2 NO2(g) (a) A flask containing
only N2O4 at an initial pressure of 4.9 atm is allowed to reach
equilibrium. Calculate the equilibrium partial pressures of the
gases. b) he volume of the container in part (a) is decreased to
one-half the original volume. Calculate the new equilibrium partial
pressures.

In the gas phase, nitrogen dioxide is actually a mixture
of nitrogen dioxide (NO2) and
dinitrogen tetroxide
(N2O4). If
the density of such a mixture is 6.76 g/L at 74°C
and 3.50 atm, calculate the partial pressures of
the gases and KP for the
dissociation of N2O4.
Pressure of
NO2:
Pressure of
N2O4:
KP:

An equilibrium mixture contains N2O4, (P= 0.27atm ) and
NO2 (P= 1.1 atm ) at 350 K. The volume of the container is
doubled at constant temperature.
A) Calculate the equilibrium pressure of
N2O4 when the system reaches a new equilibrium.
B) Calculate the equilibrium pressure of
NO2 when the system reaches a new equilibrium.

At 25°C, the equilibrium partial pressures of NO2 and N2O4 are
0.150 atm and 0.200 atm, respectively. If the volume is increased
by 1.60 fold at constant temperature, calculate the partial
pressures of the gases when a new equilibrium is established.
PNO2 = atm
PN2O4 = atm

During lecture, the following chemical equilibrium between
nitrogen dioxide and dinitrogen tetroxide
was presented and discussed.
2 NO2(g)<=> N2O4(g) Kp = 7.5 at 300.0 K.
(a) If the total pressure in the container, which has a volume of
100.0 mL, is 0.85 atm, what are the
partial pressures (in atm) of NO2(g) and N2O4(g) in this container
at 300.0 K?
(b) Using your answer to (b), what are the equilibrium
concentrations (in M) of NO2(g) and N2O4(g) in
this container...

An equilibrium mixture contains N2O4,
(P= 0.28 atm ) and NO2 (P= 1.0 atm )
at 350 K. The volume of the container is doubled at constant
temperature.
Part A
Calculate the equilibrium pressure of N2O4
when the system reaches a new equilibrium.
Express your answer using two significant figures.
Part B
Calculate the equilibrium pressure of NO2 when the
system reaches a new equilibrium.
Express your answer using two significant figures.

An equilibrium mixture consists of 0.31 atm NO2(g) and 0.45 atm
N2O4(g). 2 NO2(g) <—> N2O4(g) A chemist adds enough NO2 to
this mixture to increase the equilibrium partial pressure of NO2(g)
to 0.40 atm. What additional pressure of NO2 did she add to the
container? Assume that the temperature and volume remain
constant.

During lecture, the following chemical equilibrium between
nitrogen dioxide and dinitrogen tetroxide was presented and
discussed.
2 NO2(g) N2O4(g) Kp = 7.5 at 300.0
(a) (4 pts) If the total pressure in the container, which has a
volume of 100.0 mL, is 0.85 atm, what are the partial pressures (in
atm) of NO2(g) and N2O4(g) in this container at 300.0 K?
(b) (2 pts) Using your answer to (b), what are the equilibrium
concentrations (in M) of NO2(g) and N2O4(g)...

Calculating Equilibrium Constants.
The equilibrium constant, K, of a reaction at a
particular temperature is determined by the concentrations or
pressures of the reactants and products at equilibrium.
For a gaseous reaction with the general form
aA+bB⇌cC+dD
the Kc and Kp expressions are given by
Kc=[C]c[D]d[A]a[B]b
Kp=(PC)c(PD)d(PA)a(PB)b
The subscript c or p indicates whether K is expressed
in terms of concentrations or pressures. Equilibrium-constant
expressions do not include a term for any pure solids or liquids
that may be involved...

In the gas phase, nitrogen dioxide is actually a mixture of
nitrogen dioxide (NO2) and dintrogen tetroxide (N2O4). Assume the
density of such a mixture (at 74.0°C and 1.30 atm) is 2.70 g/L.
What would be the partial pressures of the gases and KP.
PNO2 = atm
PN2O4 = atm
KP =

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