5. 6.0 moles H2S are placed in a 2.0L container. At equilibrium 5.0 moles H2 are present.Calculate the Keq_H₂S (g) _H2(g) + _S2 (g)6. At 800°C, Keq = 0.279 forCO2 (g) + H2 (g) CO(g) + H₂O (g).If 2.00 moles CO(g) and 2.00 moles H₂O (g) are placed in a 500 ml container, calculate allequilibrium concentrations.7. CO (g) + H₂O(g) + CO2(g) + H₂ (g) Keq= 10.0 at 690°C. If at a certain time [CO] = 0.80M, [H₂O] =0.050M, [CO₂] = 0.50M and [H₂] = 0.40M, is the reaction at equilibrium? If not, how will itshift in order to get to equilibrium

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5. 6.0 moles H2S are placed in a 2.0L container. At equilibrium 5.0 moles H2 are present. Calculate the Keq _H₂S (g) _H2(g) + _S2 (g)

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

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Question

5. 6.0 moles H2S are placed in a 2.0L container. At equilibrium 5.0 moles H2 are present.
Calculate the Keq
_H₂S (g) _H2(g) + _S2 (g)
6. At 800°C, Keq = 0.279 for
CO2 (g) + H2 (g) CO(g) + H₂O (g).
If 2.00 moles CO(g) and 2.00 moles H₂O (g) are placed in a 500 ml container, calculate all
equilibrium concentrations.
7. CO (g) + H₂O(g) + CO2(g) + H₂ (g) Keq= 10.0 at 690°C. If at a certain time [CO] = 0.80M, [H₂O] =
0.050M, [CO₂] = 0.50M and [H₂] = 0.40M, is the reaction at equilibrium? If not, how will it
shift in order to get to equilibrium

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