on temp, pressue, assume they do not change.
I think you are off track, this is not a gas law problem.
it takes 5 volumes of O2 to react with 2 volumes C2H2.
volumeO2=5/2 * 89.2Liters
Law: You need to read the Law of combining volumes: https://en.wikipedia.org/wiki/%E2%80%93Lussac_law#Law_of_combining_volumes
Using the following equation 2C2H2 + 5O2 -> 4CO2 + 2H2O
what volume of oxygen would be needed to react with 89.6L of C2H2 at a temp of 273 and a pressure of 101.3 kpa.
I can't seem to figure out my first step. Using PV=NRT should I do initial and final conditions?
I thibk this is a two step question but I don't know what law to use first to find the final volume
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