Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g): 2HI(g) The equilibrium constant K for this reaction is 8.57 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.

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Chapter19: The Chemistry Of The Main-group Elements
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Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2HI(g)
The equilibrium constant K for this reaction is 8.57 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
Transcribed Image Text:Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 8.57 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
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