Question

An equilibrium mixture contains N_{2}O_{4},
(*P*= 0.28 atm ) and NO_{2} (*P*= 1.0 atm )
at 350 K. The volume of the container is doubled at constant
temperature.

Part A

Calculate the equilibrium pressure of N_{2}O_{4}
when the system reaches a new equilibrium.

Express your answer using two significant figures.

Part B

Calculate the equilibrium pressure of NO_{2} when the
system reaches a new equilibrium.

Express your answer using two significant figures.

Answer #1

N2O4 -------->2NO2

Initial

0.28 .............1.0

Kp = (1.0)^2/(0.28) = 3.57

Now

When Volume is Doubled.....Pressure will be halved ...at constant temperature .....

therefore

N2O4 ----------------> 2NO2

Initial

0.14..........................0.5

Final

0.14-x........................0.5+2x

Kp = (0.5+2x)^2/(0.14-x)

3.57*(0.14-x) = (0.5+2x)^2

0.4998 - 3.57x = 0.25 + 4x^2 + 2x

4x^2 +5.57x -0.25 =0

solving for x

we get

x =0.0435

a) Equilibrium pressure of N2O4 = 0.14 - x = 0.10 atm

b) Equilibrium pressure of NO2 = 0.5 +2x = 0.59 atm

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.

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.

Calculate the equilibrium concentrations of N2O4 and NO2 at 25
∘C in a vessel that contains an initial N2O4 concentration of
0.0438 M . The equilibrium constant Kc for the reaction
N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C. Express your answers using
four decimal places separated by a comma. [N2O4], [NO2] =
_________________________
The air pollutant NO is produced in automobile engines from the
high-temperature reaction
N2(g)+O2(g)⇌2NO(g);Kc=1.7×10−3at
2300 K.
If the initial concentrations of N2 and O2 at 2300 K are...

A flask is charged with 1.800 atm of N2O4(g)and 1.00
atm NO2(g) at 25 ∘C, and the following equilibrium is
achieved:
N2O4(g)⇌2NO2
After equilibrium is reached, the partial pressure of NO2 is 0.517
atm .
1)What is the equilibrium partial pressure of N2O4?
Express your answer with the appropriate units.
2)Calculate the value of Kp for the
reaction.
3)Calculate Kc for the reaction.

A flask is charged with 1.550 atm of N2O4(g)and 1.00
atm NO2(g) at 25 ∘C, and the following equilibrium is
achieved:
N2O4(g)⇌2NO2
After equilibrium is reached, the partial pressure of NO2 is 0.519
atm .
1.What is the equilibrium partial pressure of N2O4?Express your
answer with the appropriate units.
2. Calculate the value of Kp for the
reaction.
3.Calculate the value of Kc for the reaction.

A flask is charged with 1.800 atm of
N2O4(g) and 1.00 atm of
NO2(g) at 25 ∘C , and the following
equilibrium is achieved:
N2O4(g)⇌2NO2(g)
After equilibrium is reached, the partial pressure of
NO2 is 0.519 atm .
Part A:
What is the partial pressure of N2O4 at
equilibrium?
Part B:
Calculate the value of Kp for the
reaction.
Part C:
Calculate the value of Kc for the
reaction.

A system at equilibrium contains I2(g) at a pressure of
0.23 atm and I(g) at a pressure of 0.24 atm . The system
is then compressed to half its volume.
Find the pressure of I2 when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.
Find the pressure of I when the system returns to
equilibrium.
Express your answer to two significant figures and include the
appropriate units.

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

Calculate the equilibrium concentrations of N2O4 and NO2 at 25
∘C in a vessel that contains an initial N2O4 concentration of
0.0365 M . The equilibrium constant Kc for the reaction
N2O4(g)⇌2NO2(g) is 4.64×10−3 at 25 ∘C.
Express your answers using four decimal places separated by a
comma.

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.

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 25 minutes ago

asked 28 minutes ago

asked 29 minutes ago

asked 37 minutes ago

asked 45 minutes ago

asked 49 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago