$$\ce{Cu2S + 2 O2 -> 2 CuO + SO2}$$
Why are not these oxides $\ce{Cu2O}$, $\ce{SO}$ or $\ce{SO3}$? Is it connected to the stability of these molecules?
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$\begingroup$ There should be CuO in the heading :) $\endgroup$ – Maciek Rudnicki Jun 10 '16 at 15:57
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$\begingroup$ Appreciate that. $\endgroup$ – Maciek Rudnicki Jun 10 '16 at 16:03
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The reaction gives different products when combusted at different temperature.
- $$\ce{8Cu2S + 15O2 ->[\Delta] 6Cu2O + 4CuSO4 + 4SO2}$$
Copper(I) sulfide react with oxygen to produce copper(I) oxide, copper sulfate and sulfur dioxide. This reaction takes place at a temperature of 500-600°C.Here
- $$\ce{2Cu2S + 3O2 ->[\Delta] 2Cu2O + 2SO2}$$
Copper(I) sulfide react with oxygen to produce copper(I) oxide and sulfur dioxide. This reaction takes place at a temperature of 1200-1300°C.Here
Sulfur monoxide is very unstable and it is unlikely to exist in Earth's atmosphere but it exist in interstellar spaces. Sulfur trioxide will not form from sulfur dioxide as it requires an oxidising agent.
answered Jun 10 '16 at 16:37
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Right reaction is $$\ce{2Cu2S + 3O2 -> 2Cu2O + 2SO2}$$
$\ce{Cu2O}$ is because copper in this compound has oxidation state +1 and $\ce{2Cu + O2 -> 2CuO}$.
$\ce{SO2}$ is because $\ce{SO}$ is unstable and $\ce{S + O2 -> SO2}$.
Upd. This answer isn't right. See comments of @Jan under it.
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1$\begingroup$ Your explaining arguments don’t really make sense … $\endgroup$ – Jan Jun 10 '16 at 17:35
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$\begingroup$ Because all they do is explain the simple redox process coming from the elements. I can do that, too: $\ce{C + O2 -> CO2}$, yet there are many reactions that cleanly produce $\ce{CO}$, never $\ce{CO2}$. $$~$$ It’s like saying ‘the result of mixing yellow and blue is green, because plants are green.’ It has nothing to do with each other. $\endgroup$ – Jan Jun 10 '16 at 18:18
