The following reaction 2H₂S(g) = 2H₂(g) + S2(g), Kc = 1.67 × 10-7 at 800°C is carried out at 800 °C with the following initial concentrations: [H₂S] = 0.100M, [H₂] = 0.100M, and [S₂] = 0.00 M. Find the equilibrium concentration of S2. Express the molarity to three significant figures.

The following reaction 2H₂S(g) = 2H₂(g) + S2(g), Kc = 1.67 × 10-7 at 800°C is carried out at 800 °C with the following initial concentrations: [H₂S] = 0.100M, [H₂] = 0.100M, and [S₂] = 0.00 M. Find the equilibrium concentration of S2. Express the molarity to three significant figures.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter9: Chemical Reactions

Section: Chapter Questions

Problem 9.76EP: Calculate the value of the equilibrium constant for the reaction N2(g)+2O2(g)2NO2(g) if the...

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The following reaction
2H₂S(g) 2H2(g) + S₂(g), Kc = 1.67 x 10-7 at 800°C
is carried out at 800 °C with the following initial concentrations: [H₂S] = 0.100M,
[H₂] = 0.100M, and [S₂] = 0.00 M. Find the equilibrium concentration of S2.
Express the molarity to three significant figures.

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