6. A mixture of 0.500 mol H2 and 0.500 mol I2 was placed in a 1.00 - L stainless-steel flask at 430 °C. The equilibrium constant Ke for the reaction, H2(g) + I2(g) → 2HI(g) is 54.3 at this temperature. Calculate the concentrations of H2, I2 and HI at equilibrium.
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6. A mixture of 0.500 mol H₂ and 0.500 mol I₂ was placed in a 1.00-L stainless steel flask at 430°C. The equilibrium constant Kₑ for the reaction,
\[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2\text{HI}(g) \]
is 54.3 at this temperature. Calculate the concentrations of H₂, I₂, and HI at equilibrium.
7. The pH of a 0.10 M solution of acetic acid (CH₃COOH) is 2.39. What is the \( K_a \) of acetic acid?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e830786-058e-49dd-8798-047547f22476%2Fafa98dc2-e494-4408-8bf8-e3a4856996b7%2F7rp4af.jpeg&w=3840&q=75)
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