While studying the equilibrium below at 448 °C, a chemist mixed 1.0 mole of H2 with 1.0 mole of I2 in a 1.0-L flask. H2 (g) + 12 (g) = 2 HI (g) a. After reaching equilibrium, [I2] was found to be 0.22 M. What is the value of Ke at this temperature? b. If she had mixed 1.0 mole of each reactant in a 2.0-L flask at this temperature, what would [HI] be at equilibrium?

While studying the equilibrium below at 448 °C, a chemist mixed 1.0 mole of H2 with 1.0 mole of I2 in a 1.0-L flask. H2 (g) + 12 (g) = 2 HI (g) a. After reaching equilibrium, [I2] was found to be 0.22 M. What is the value of Ke at this temperature? b. If she had mixed 1.0 mole of each reactant in a 2.0-L flask at this temperature, what would [HI] be at equilibrium?

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...

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