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azureserval214Lv1

17 Feb 2021

The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10^-4 at 3500°C. If the equilibrium partial pressures of SO₂ and SO₃ are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O₂ in the system?

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For the system SO3 ( g) â SO2 (g ) + 1 2 O2 ( g) at 1000 K, K = 0.45. Sulfur trioxide, originally at 1.00 atm pressure, partially dissociates to SO2 and O2 at 1000 K. what is its partial pressure at equilibrium?

At 900 K, the following reaction has K_p = 0.345:

2 SO₂(g) + O₂(g) 2 SO₃(g)

In an equilibrium mixture the partial pressures of SO₂ and O₂ are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO₃ in the mixture?

ambermole700

Sulfur dioxide reacts with oxygen to form sulfur trioxide.
2 SO₂ (g) + O₂ (g) --> 2 SO₃.
In a 1.00 L flask, 2.00 atm of SO₂ react with 5.00 atm of O₂. Assuming that the temperature remains constant, what is the final pressure?

a. 2.00 atm
b. 5.00 atm
c. 6.00 atm
d. 7.00 atm

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The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10^-4 at 3500°C. If the equilibrium partial pressures of SO₂ and SO₃ are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O₂ in the system?

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The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10-4 at 3500°C. If the equilibrium partial pressures of SO2 and SO3 are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O2 in the system?

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Related textbook solutions

Basic Chemistry

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The equilibrium constant Kp for the oxidation of sulfur dioxide into sulfur trioxide is 5.6×10^-4 at 3500°C. If the equilibrium partial pressures of SO₂ and SO₃ are 0.64 atm and 0.58 atm, respectively, what is the partial pressure of O₂ in the system?