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Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which K = 9.30 × 108 at 700°C: 2 H₂S(g) 2 H₂(g) + S₂(g) If 0.49 mol of H₂S is placed in a 3.0-L container, what is the equilibrium concentration of H₂(g) at 700°C? M

Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which K = 9.30 × 108 at 700°C: 2 H₂S(g) 2 H₂(g) + S₂(g) If 0.49 mol of H₂S is placed in a 3.0-L container, what is the equilibrium concentration of H₂(g) at 700°C? M

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section: Chapter Questions
Problem 38GQ: At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g)...
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Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which K = 9.30 × 108 at 700°C: 2 H₂S(g) 2 H₂(g) + S₂(g) If 0.49 mol of H₂S is placed in a 3.0-L container, what is the equilibrium concentration of H₂(g) at 700°C? M
Transcribed Image Text:Enter your answer in the provided box. Hydrogen sulfide decomposes according to the following reaction, for which K = 9.30 × 108 at 700°C: 2 H₂S(g) 2 H₂(g) + S₂(g) If 0.49 mol of H₂S is placed in a 3.0-L container, what is the equilibrium concentration of H₂(g) at 700°C? M
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