3. Consider the reaction for the decomposition of hydrogen disulfide.2 H₂S (g) + 2 H₂(g) + S₂ (g) Ke=1.67 x 10-7If the initial concentration of H₂S is 0.0250 M, what are the equilibrium concentration of H₂and S₂?Answer:InitialChangeEquilibriumCH 122 General Chemistry2 H₂S (g)0.02500.0250-xK =[H₂][S₂][H₂S]1.67 x 10-7-2 H₂(g) +0+XX(x)(x)0.0250-x 0.0250S₂ (g)0Equilibrium Solved Problemsx = 6.32 x 10-5The equilibrium concentrations of H₂ and S2 are 6.32 x 10-5 M+XX

Given:Initial concentration of H2S = 0.0250 MChemical equilibrium is a dynamic state in a reversible…

3. Consider the reaction for the decomposition of hydrogen disulfide. 2 H₂S (g) + 2 H₂(g) + S₂ (g) K₂ = 1.67 x 10-7 If the initial concentration of H₂S is 0.0250 M, what are the equilibrium concentration of H₂ and S₂?

3. Consider the reaction for the decomposition of hydrogen disulfide. 2 H₂S (g) + 2 H₂(g) + S₂ (g) K₂ = 1.67 x 10-7 If the initial concentration of H₂S is 0.0250 M, what are the equilibrium concentration of H₂ and S₂?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 4ALQ

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Question

3. Consider the reaction for the decomposition of hydrogen disulfide.
2 H₂S (g) + 2 H₂(g) + S₂ (g) Ke=1.67 x 10-7
If the initial concentration of H₂S is 0.0250 M, what are the equilibrium concentration of H₂
and S₂?
Answer:
Initial
Change
Equilibrium
CH 122 General Chemistry
2 H₂S (g)
0.0250
0.0250-x
K =
[H₂][S₂]
[H₂S]
1.67 x 10-7-
2 H₂(g) +
0
+X
X
(x)(x)
0.0250-x 0.0250
S₂ (g)
0
Equilibrium Solved Problems
x = 6.32 x 10-5
The equilibrium concentrations of H₂ and S2 are 6.32 x 10-5 M
+X
X

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