1. 0.60 moles of H₂ and 1.4 moles of S are placed into a 2.0L flask and allowed to reach equilibrium. Calculate the [H₂] at equilibrium. _H2 (g) + _S (s) _H₂S (g) Keq= 14 2. Consider the following equilibrium system: _NO2(g) _N2O4 (g) Two sets of equilibrium data are listed for the same temperature. Container 1 2.00 L 0.12 moles NO2 Container 2 5.00 L 0.26 moles NO2 Determine the number of moles N204 in the second container. 0.16 moles N204 ? moles N204

1. 0.60 moles of H₂ and 1.4 moles of S are placed into a 2.0L flask and allowed to reach equilibrium. Calculate the [H₂] at equilibrium. _H2 (g) + _S (s) _H₂S (g) Keq= 14 2. Consider the following equilibrium system: _NO2(g) _N2O4 (g) Two sets of equilibrium data are listed for the same temperature. Container 1 2.00 L 0.12 moles NO2 Container 2 5.00 L 0.26 moles NO2 Determine the number of moles N204 in the second container. 0.16 moles N204 ? moles N204

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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