sour gas H2S(g) can establish the following equalibrium system under certain conditions.
note that S2(g) is a violet coloured gas. both sour gas and hydrogen gas are colourless
2H2S(g) ---> 2H2(g) + S2(g)
state the effect each of the following stressers will have on this system in terms of the colour of the system: darker violet, lighter violet, or no colour change to the colour of the system.
5 years ago
Answered By Emily H
You neglected to mention the specific stressors in your question, but if we assume that one of the three gasses will be added to the reaction cell, we can say this:
If H2S is added, then this will move the equilibrium to the right, but as the ratio $\frac{S_2}{H_2+H_2S}$S2H2+H2S won't be affected, there won't be any change to the colour.
If either H2 or S2 are added, the equilibrium will shift to the left, so if hydrogen is added, we will be decreasing the ratio of coloured to colourless gases above so the colour will become lighter. Conversely, if sulfur is added we will be increasing the ratio so the colour will be darker.