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Ch.15 - Chemical Equilibrium

Chapter 15, Problem 46

At 900 K, the following reaction has 𝐾𝑝 = 0.345: 2 SO2(𝑔) + O2(𝑔) β‡Œ 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?

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Hello everyone today. We are being given the following problem and asked to solve for it. So it says the equilibrium constant K. P. For the oxidation of nitric oxide is 1152 at 1 50 degrees Celsius. Were then given the following chemical reaction In that reaction mixture at equilibrium oxygen has a partial pressure of .345 atmospheres. While the partial pressure of nitrogen dioxide is .225 atmospheres were then asked to calculate the partial pressure of nitric oxide at equilibrium. So the first thing we want to do does he want to calculate, we want to write out our K. P. For the expression below. So R. K. P. It's going to be equal to the pressures of our products over reactivates. And so putting this together, We have our pressure of our only product which is nitrogen dioxide in 02. And since there is a two coefficient we're going to make this exponent into a. two and our denominator we have to react. It's present. We have nitric oxide and so we have the pressure of N. O. Nitric oxide and that has a two coefficient as well. So we're going to give that an exponent of two. And lastly we're going to multiply the second reactant from by the first one which is just molecular oxygen. And so we have our K. P. Expression below. We also were given a partial pressure of oxygen and the partial pressure of pressure of nitrogen dioxide. And so ultimately we want to find the partial pressure of nitric oxide. So we're gonna label that X. And so Plugging our values in to this reaction that we just found we have our K. P. or equilibrium constant being 1,152. And that's going to equal Our partial pressure of our nitrogen dioxide. Which in the question Stem said that it was 0.225 atmospheres. And we're going to square that and then we're going to divide that by our partial pressure of nitric oxide, which we don't know. So we're just gonna say X. And we're gonna square that as well. And then our partial pressure for molecular oxygen or 02 is 0.345 atmospheres, solving for X. We get an X. is equal to 0.0113 atmospheres. In other words, this is our partial pressure of nitric oxide. I hope this helped. And until next time.
Related Practice
Textbook Question

Indicate whether each of the following statements about the reaction quotient Q is true or false: (a) The expression for 𝑄𝑐 looks the same as the expression for 𝐾𝑐.

Textbook Question

Indicate whether each of the following statements about the reaction quotient Q is true or false: (b) If 𝑄𝑐 < 𝐾𝑐, the reaction needs to proceed to the right to reach equilibrium.

Textbook Question

At 100Β°C, the equilibrium constant for the reaction COCl2(𝑔) β‡Œ CO(𝑔) + Cl2(𝑔) has the value 𝐾𝑐 = 2.19Γ—10βˆ’10. Are the following mixtures of COCl2, CO, and Cl2 at 100Β°C at equilibrium? If not, indicate the direction that the reaction must proceed to achieve equilibrium. (a) [COCl2] = 2.00Γ—10βˆ’3 𝑀, [CO] = 3.3Γ—10βˆ’6 𝑀, [Cl2] = 6.62Γ—10βˆ’6𝑀

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Textbook Question

At 218Β°C, 𝐾𝑐 = 1.2Γ—10βˆ’4 for the equilibrium NH4SH(𝑠) β‡Œ NH3(𝑔) + H2S(𝑔) (a) Calculate the equilibrium concentrations of NH3 and H2S if a sample of solid NH4SH is placed in a closed vessel at 218Β°C and decomposes until equilibrium is reached.

Textbook Question

At 80Β°C, 𝐾𝑐 = 1.87Γ—10βˆ’3 for the reaction PH3BCl3(𝑠) β‡Œ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80Β°C and decomposes until equilibrium is reached.

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Textbook Question

At 80Β°C, 𝐾𝑐 = 1.87Γ—10βˆ’3 for the reaction PH3BCl3(𝑠) β‡Œ PH3(𝑔) + BCl3(𝑔) (a) Calculate the equilibrium concentrations of PH3 and BCl3 if a solid sample of PH3BCl3 is placed in a closed vessel at 80Β°C and decomposes until equilibrium is reached. (b) If the flask has a volume of 0.250 L, what is the minimum mass of PH3BCl3(𝑠) that must be added to the flask to achieve equilibrium?

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