How many L of O2 are needed to react completely with 63.0 L of H₂S at STP? (show your work) 2H₂S(g) + 3O₂(g) → 2SO₂(g) + 2H₂O(g)

Question

photon336 · Answer

STP = standard temperature and pressure, 293K 1 atm

photon336 · Answer

$$pV =nRT $$

we know R, T and V and P we just need n the number of moles of H2S

$$\frac{ pV }{ RT } = n$$

plug in our values 

$$\frac{ (1atm)(63.0L) }{ (273K)(0.08K ^{-1})Lmol ^{-1}atm }  = 2.90 moles, H_{2}S$$

one you know this number the number of moles which we just got. figuring out how many liters of O2 is easy. you can multiply by the molar ratio 

Do this and you'll get the number of moles of O2 

$$2.90 mol H_{2}S *(\frac{ 3O_{2} }{ 2H_{2}S }) = moles of O_{2}$$

then you can easily find the number of liters atstp

anonymous · Answer

can you help? how would i do that?

photon336 · Answer

see above what I did try it out first the tell me what you would get