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Chapter 15, Problem 53

At 373 K, 𝐾_𝑝= 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br₂(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br₂(𝑔)?

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Chapter 15, Problem 53

At 373 K, 𝐾𝑝 = 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br2(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br2(𝑔)?

At 373 K, 𝐾_𝑝= 0.416 for the equilibrium 2 NOBr(𝑔) ⇌ 2 NO(𝑔) + Br₂(𝑔) If the pressures of NOBr(𝑔) and NO(𝑔) are equal, what is the equilibrium pressure of Br₂(𝑔)?