At 500 °C, hydrogen iodide decomposes according to 2HI(g) – --- H2(g)+l2(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0.494 M , [12]=0.494 M, and [HI]=4.18 M . If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached?

At 500 °C, hydrogen iodide decomposes according to 2HI(g) – --- H2(g)+l2(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2]=0.494 M , [12]=0.494 M, and [HI]=4.18 M . If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached?

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 12.35PAE: In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial...

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