Question

2 NO_{2}(g) <---------> 2 NO(g) +
O_{2}(g)

Starting with pure NO_{2} , the flask is heated and he
partial pressure of O2 at equlibrium is 0.133 am. Calculate the
partial pressures of NO and NO_{2} at equlibrium and the
total pressure in the flask at equlibrium.

P_{NO} ____________________atm

P_{NO2}____________________atm

P_{total}____________________atm

Answer #1

The given reaction is

2 NO_{2} (g) -------> 2 NO (g) + O_{2}
(g)

As per the balanced stoichiometric equation, the molar ratio of the reactants and products is 2:2:1.

Therefore, as per the molar equation, the mole fraction of
O_{2} in the gaseous mixture (both reactants and products
combined) is 1 mole/(2 + 2 + 1) mole = 1/5.

Assuming all the gases to behave ideally and applying Dalton’s law, we must have,

P_{O2} = (mole fraction of
O_{2})*P_{total}

Given P_{O2} = 0.133 atm at equilibrium,

0.133 atm = (1/5)*P_{total}

====> P_{total} = (0.133 atm)*5 = 0.665 atm

P_{NO2} = (mole fraction of
NO_{2})*P_{total} = (2/5)I*0.665 atm = 0.266
atm

P_{NO} = (mole fraction of NO)*P_{total} =
(2/5)*0.665 atm = 0.266 atm

P_{total} = 0.665 atm (ans).

At 1000 K, a sample of pure NO2 gas decomposes: 2NO2(g) ⇌ 2NO(g)
+ O2(g) The equilibrium constant, KP, is 158. Analysis shows that
the partial pressure of O2 is 0.45 atm at equilibrium. Calculate
the pressure of NO and NO2 in the mixture

Nitrogen Dioxide decomposes according to the reaction 2 NO2 (g)
<----> 2 NO(g) + O2 (g) Where Kp= 4.48 x 10-13 at a certain
temperature. If 0.08 atm of NO2 is added to a container and allowed
to come to equilibrium, what are the equilibrium partial pressures
of NO(g) and O2(g)?

The oxidation of nitric oxide
NO + 0.5 O2 --> NO2
takes place in an isothermal batch reactor. The reactor is charged
with a mixture containing 20.0
volume percent NO and the balance air at an initial pressure of 380
kPa (absolute).
(a) Assuming ideal-gas behavior, determine the composition of the
mixture (component mole
fractions) and the final pressure (kPa) if the conversion of NO is
90%.
(b) Suppose the pressure in the reactor eventually equilibrates
(levels out) at 360...

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
N2O4?
Calculate the value of Kp for the
reaction
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
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 flask is charged with 1.500 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 0.514
atm .
Calculate Kc for the reaction.

A flask is charged with 1.500 atm
N2O4(g) and 1.00 atm
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
0.512 atm. What is the equilibrium partial pressure of N2O4?

Introduced into a 1.50 L flask is 0.100 mol PCl5(g).
The flask is held at 227°C until equilibrium is established. What
are the partial pressures and the total pressure of the gases in
the flask at equilibrium?
PCl5(g) ↔ PCl3(g) + Cl2(g)
1) Calculate ∆H°rxn
2) Calculate ∆S°rxn
3) Calculate Keq
4) Calculate Pinitial
(PCl5)
5) Calculate equilibrium pressures for PCl5(g),
PCl3(g), Cl2(g)
6) calculate total pressure of this gas mixture at
equilibrium

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