2. Hydrogen sulfide (H2S) is colorless, flammable gas, which has a pungent odor reminiscent of rotten eggs. The threshold for perception is about 0.13 ppm, please show the concentration of 1 mol H2S at standard ambient temperature and pressure (SATP) in terms of ?g/m³. (MW: H =1 g/mol; S =32 g/mol)
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- The molar mass of hydrogen (H) is 1 g/mol. - The molar mass of sulfur (S) is 32 g/mol. - Therefore, the molar mass of H₂S is: \[ \text{Molar mass of H}_2\text{S} = 2 \times 1 \, \text{g/mol} + 32 \, \text{g/mol} = 34 \, \text{g/mol} \] Show more…
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Hydrogen Sulphide (H2S) occurs in the atmosphere naturally at a concentration of 0.05 ppb. Determine whether or not this concentration represents equilibrium with respect to H2O, SO2 and O2 (all in the gaseous phase). A) Convert the concentration of H2S to its partial pressure, assuming an atmospheric pressure of 1atm. B) Write the appropriate chemical reaction that governs the concentration of H2S in the atmosphere if equilibrium were maintained between SO2, H2O, H2S, and O2. Important: Place O2 on the right hand side of the raction. The equilibrium constant for this reaction is 10-86.74. C) Calculate the partial pressure of H2S as if the raction is controlled by chemical equilibrium.
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