Question
How many litres of oxygen are needed to react completely with 25.0L of H2S at STP according to the following reaction: 2H2S + 3o2 --> 2so2 + 2H2O
At STP temperature is 273 K pressure is 101.3 Kpa R is 8.314 so PV=nRT
101.3×25= n× 8.314× 273
n= 1.11 so using the molar ratio we find the moles of o2= 1.70 now how do I find the volume of O2 with only the moles and no concentration?!
At STP temperature is 273 K pressure is 101.3 Kpa R is 8.314 so PV=nRT
101.3×25= n× 8.314× 273
n= 1.11 so using the molar ratio we find the moles of o2= 1.70 now how do I find the volume of O2 with only the moles and no concentration?!
Answers
bobpursley
YOu are doing it the very hard way. All the reactants are gases, same temp, pressure, so you can use the EQual Volumes law (John Dalton)
so for each 2 volumes of H2S, you need three volumes of O2
VolumesO2=3/2 * 25 liters
so for each 2 volumes of H2S, you need three volumes of O2
VolumesO2=3/2 * 25 liters
I agree with Bob Pursley that you are/were doing it the hard way; however, the answer to your question is this. After you know mols O2 = 1.70, then you know that at STP the volume of any gas is 22.4 L for one mole.
So 1.70 mols x (22.4 L/mol) = ? L.
So 1.70 mols x (22.4 L/mol) = ? L.
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