The reaction mixture shown below initially contains 2.8 M H2O and 2.6 M SO2. If

Question

The reaction mixture shown below initially contains 2.8 M H2O and 2.6 M SO2. If Kc for the reaction at this temperature is 1.3x10^-6
2 H2O + 2 SO2 --> 2H2S + 3 O2
A. Determine the initial equilibrium concentration of each gas species?


B. What are the new equilibrium concentrations of each gas when the concentration of SO2 changes to 1.25M? The reaction mixture shown below initially contains 2.8 M H2O and 2.6 M SO2. If Kc for the reaction at this temperature is 1.3x10^-6
2 H2O + 2 SO2 --> 2H2S + 3 O2
A. Determine the initial equilibrium concentration of each gas species?


B. What are the new equilibrium concentrations of each gas when the concentration of SO2 changes to 1.25M?
2 H2O + 2 SO2 --> 2H2S + 3 O2
A. Determine the initial equilibrium concentration of each gas species?


B. What are the new equilibrium concentrations of each gas when the concentration of SO2 changes to 1.25M?

Explanation / Answer

2 H2O + 2 SO2 --> 2H2S + 3 O2

2 moles of H2O reacts with 2 moles of SO2 to form 2 moles of 2H2S and 3 moles of O2

2.6 M of So2 will react with 2.6 moles of H2O to form 2.6 moles of H2S and 3.9 moles of O2

Kc= [x

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