I assume this is O2 at 0C and O2 at 100 C and it ISN'T dissolved in H2O.
Use PV = nRT. I would substitute P in atm (convert bar to atm), R = 0.08206 L*atm/mol*K and T = 273. Solve for n.
Do the same for the 373 system and solve for n.
Subtract to find the difference and convert mols to grams.
There are two flask, one filled with a)ice bath, and b)boiling water.
Ice bath: 1.00 L O^2(g) at STP
Boiling water: 1.00 O^2(g)
If we want the pressure to remain at 1.00bar when the O^2(g) is heated to 373K, what mass of O^2 must we release from the flask?
I know that I should use the general gas equation, but I don't know what quantities I should plug in!
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