At 460°C, 0.02 g of hydrogen reacts with 2.54 g of iodine until equilibrium is reached. Upon analysis, the equilibrium mixture contains 0.0021 moles of iodine. What is the equilibrium constant (Kc) for this reaction?

Question

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566. To find the equilibrium constant Kc for the reaction involving hydrogen and iodine, the given masses are converted to moles, and then Kc is calculated based on the equilibrium concentrations, yielding a value of 566.

At 460°C, 0.02 g of hydrogen reacts with 2.54 g of iodine until equilibrium is reached. Upon analysis, the equilibrium mixture contains 0.0021 moles of iodine. What is the equilibrium constant (Kc) for this reaction?

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