Please help!!!
what mass of sulfur must be used to produce 29.4 L of gaseous sulfur dioxide at STP according to the following equation?
S8 + 8 02 yields 8 SO2
2007-04-17 09:58:18 · 3 answers · asked by nikki 1 in Science & Mathematics ➔ Chemistry
PV = nRT, n = PV/RT
STP: 1 atm, 298 K
n = (1atm)(29.4L)/(0.08205)(298)
n = 1.202 mol SO2
S8 + 8O2 ---> 8SO2
8 mol SO2 : 1 mol S8
1.202 mol SO2 : 0.1503 mol S8
0.1503 mol S8 x 256g/mol = 38.5g S8
2007-04-17 10:15:16 · answer #1 · answered by moneymonty 3 · 0⤊ 0⤋
This is a traditional stoichiometry question. You need to convert the L into moles (using PV=nRT) then convert moles SO2 into moles sulfur using the mole ratio in the reaction. Then convert the moles into mass using the molar mass (the thing you add up from the atomic masses on the periodic table).
Pretty much all stoichiometry problems can be broken down into three steps. 1) Convert given to moles. 2) convert mols of given to moles of unknown. 3) convert moles of unknown to what you want your answer to be.
2007-04-17 10:18:31 · answer #2 · answered by Anonymous · 0⤊ 0⤋
29.4LSO2 x 1molSO2/22.4LSO2 x 1molS/1molSO2 x 32gS/1molS = 42gS
One has to cut past the 8mols/8mols and realize that the 8's cancel.
2007-04-17 10:09:31 · answer #3 · answered by steve_geo1 7 · 0⤊ 1⤋