8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10³ mol/L and [NO] = 4 x 10+ M

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8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g)
Kp 4.10 x 10³ at 2000°C
a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen
monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to
reach equilibrium? Show all work to justify your answer.
b) What is the concentration of each gas when equilibrium is reached at 2000°C?
Show all your work.
Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm
Use PV = nRT
Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M
Transcribed Image Text:8. Consider the equilibrium reaction: N2(g) + O2(g) = 2 NO(g) Kp 4.10 x 10³ at 2000°C a) If 1.00 atm of nitrogen gas and 1.00 atm of oxygen gas is mixed with 0.10 atm of nitrogen monoxide in a 500.0 mL container at 2000°C, in which direction will the reaction proceed to reach equilibrium? Show all work to justify your answer. b) What is the concentration of each gas when equilibrium is reached at 2000°C? Show all your work. Equilibrium Partial Pressures: PN₂ = Po₂ = 1.02 atm and PNO = 0.07 atm Use PV = nRT Answer: Equilibrium Concentrations: [N₂] = [0₂] = 5.47 x 10-3 mol/L and [NO] = 4 x 10+ M
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