Howdy, all you fine folks.
I'm in Accelerated General Chem, and I have encountered the problem copied below.
""Strike anywhere" matches contain the compound tetraphosphorus trisulfide, which burns to form tetraphosphorus decaoxide and sulfur dioxide gas. How many milliliters of sulfur dioxide, measured at 732 torr and 32°C, can be produced from burning 0.841 g of tetraphosphorus trisulfide?"
I believe I can field the problem if I could just write and balance the equation. What I have so far is:
P4S3 --> P4O10 + SO2(g)
...but obviously the oxygen is not present on the reactant side of the equation. Where does it appear? Is it a reactant as O2 gas which is used to burn the P4S3?