Given the reaction PCI3 (g) = PCI3(g) + Cl2(g) with an equilibrium constant Kp= 1.05 at 250°C. a. Write the equilibrium constant in terms of the Partial pressures of each gas. b. If we start with 2.5 grams of PClgin a 5.0I container, what is the Partial pressure of each gas at equilibrium? Consider the degree of dissociation to be the amount of reactant that reacted relative to its initial pressure. c. What is the degree of dissociation?

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Given the reaction PCI5 (g) = PC13(g) + Cl2(g) with an equilibrium constant Kp= 1.05 at 250°C.
a. Write the equilibrium constant in terms of the Partial pressures of each gas.
b. If we start with 2.5 grams of PCI5in a 5.0 I container, what is the Partial pressure of each gas at equilibrium?
Consider the degree of dissociation to be the amount of reactant that reacted relative to its initial pressure.
c. What is the degree of dissociation?
If we write the reaction as
2PCI5 (g) = 2PCI3(g) + 2C1½(g)
d. Write the equilibrium constant in terms of the Partial pressures of each gas.
e. Is Kp be the same as before?
Justify your answer using the relationship between AG° and Kp
Transcribed Image Text:Given the reaction PCI5 (g) = PC13(g) + Cl2(g) with an equilibrium constant Kp= 1.05 at 250°C. a. Write the equilibrium constant in terms of the Partial pressures of each gas. b. If we start with 2.5 grams of PCI5in a 5.0 I container, what is the Partial pressure of each gas at equilibrium? Consider the degree of dissociation to be the amount of reactant that reacted relative to its initial pressure. c. What is the degree of dissociation? If we write the reaction as 2PCI5 (g) = 2PCI3(g) + 2C1½(g) d. Write the equilibrium constant in terms of the Partial pressures of each gas. e. Is Kp be the same as before? Justify your answer using the relationship between AG° and Kp
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