Consider the equilibrium system involving the decomposition of hydrogen iodide. 2HI(g) H₂(g) + I₂(9) [HI] = [H₂] = [1₂] = A A flask originally contains 0.322 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases. M M M K= Check & Submit Answer [H₂] [12] [HI]² = 2.41x10-2 at 1040 K Show Approach
Consider the equilibrium system involving the decomposition of hydrogen iodide. 2HI(g) H₂(g) + I₂(9) [HI] = [H₂] = [1₂] = A A flask originally contains 0.322 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases. M M M K= Check & Submit Answer [H₂] [12] [HI]² = 2.41x10-2 at 1040 K Show Approach
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter14: Chemical Equilibrium
Section: Chapter Questions
Problem 30P
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![Tutored Practice Problem 15.3.4 COUNTS TOWARDS GRADE
Use K and initial concentrations to calculate equilibrium concentrations.
Consider the equilibrium system involving the decomposition of hydrogen iodide.
2HI(g) H₂(g) + I₂(g)
[HI] =
[H₂]=
[1₂] =
=
ΣΣΣ
K =
Check & Submit Answer
[H₂] [1₂]
[HI]²
A flask originally contains 0.322 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases.
=
Show Approach
2.41x10-2 at 1040 K
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Transcribed Image Text:Tutored Practice Problem 15.3.4 COUNTS TOWARDS GRADE
Use K and initial concentrations to calculate equilibrium concentrations.
Consider the equilibrium system involving the decomposition of hydrogen iodide.
2HI(g) H₂(g) + I₂(g)
[HI] =
[H₂]=
[1₂] =
=
ΣΣΣ
K =
Check & Submit Answer
[H₂] [1₂]
[HI]²
A flask originally contains 0.322 M hydrogen iodide. Calculate the equilibrium concentrations of the three gases.
=
Show Approach
2.41x10-2 at 1040 K
Close Pro
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