Question

2) Suppose the initial pressure Po= 0.600 atm at 25 oC for N2O4 before dissociation. Calculate the partial pressures PN2O4 and PNO2 at equilibrium and the fraction of N2O4 molecules that have dissociated. Keq = 8.8 at 25 oC.

Answer #1

At 25 oC, Po (N2O4) = 0.600 atm

Keq = 8.8

N2O4
2NO2

Initially 0.600 0

Finally 0.600 - P 2P

Keq = [P (NO2)]^{2} / P(N2O4)

8.8 = (2P)^{2} / (0.600 - P)

8.8 * (0.600 - P) = (2P)^{2}

5.28 - 8.8P = 4P^{2}

4P^{2} + 8.8P - 5.28 = 0

Solving above equation:

P = 0.49 atm

Hence,

Partial pressure of NO2 = 2P = 0.98 atm

Partial pressure of N2O4 = 0.600 - P = 0.11 atm

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

At 365 K and a total equilibrium pressure of 0.985 atm, the
fractional dissociation of CH2Cl2 is 0.850 for the reaction
2CH2Cl2(g) <----> CH4(g) + CCl4(g)
This means that 850 of every 1000 molecules of CH2Cl2 originally
present have dissociated. Calculate the equilibrium constant in
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Kp = _______

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 0.515
atm .
What is the equilibrium partial pressure of
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Calculate the value of Kp for the
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Calculate Kc for the
reaction.

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
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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 flask is charged with 1.500 atm of N2O4(g) and 1.00 atm NO2(g)
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After equilibrium is reached, the partial pressure of NO2 is 0.514
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Calculate Kc for the reaction.

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2) Calculate the equilibrium concentration of NO2.
I have worked through this problem several times and keep
getting the wrong answer. I think I'm making a math error along the
way. Could you show as much work...

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