1. Hydrogen sulphide (H 2 S) occurs in the atmosphere naturally at a concentrati

Question

1. Hydrogen sulphide (H2S) occurs in the atmosphere naturally at a concentration of 0.05 ppb. Determine whether or not this concentration represents equilibrum 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 1 atm.

b) Write the approprate chemical reaction that governs the conccentration 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 reaction. The equilibriu constant for this reaction is 10-86.74.

c) Calculate the partial pressure of H2S as if the reaction is controlled by chemical equilibrium.

Explanation / Answer

The concentration of H2S is in equilibrium with with respect to H2O, SO2, and O2

(a): Given the concentration of H2S = 0.05 ppb

Hence partial pressure due to H2S = (0.05 / 109 ) x 1 atm = 5.0x10-11 atm

(b): The chemical reaction is

2SO2(g) + 2H2O(l) <====> 2 H2S(g) + 3O2(g) : K = 10-86.74   

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