Asked by Brigitte
how many liters of oxygen are required to react completely with 12.5 liters of hydrogen sulfide at stp?
Answers
Answered by
DrBob222
You need an equation and it must be balanced.
Convert 12.5 L H2S to mols. That is 12.5L/22.4 = ? mols H2S.
Use the coefficients in the balanced equation to convert mols H2S to mols Oxygen.
Now convert mols oxygen to L.
mols O2 x 22.4L= ?
There is a shortcut you can use if you wish. Since all are gases, you may omit the mols step at the front and back and just convert L H2S to L O2 directely using the coefficients as above
Convert 12.5 L H2S to mols. That is 12.5L/22.4 = ? mols H2S.
Use the coefficients in the balanced equation to convert mols H2S to mols Oxygen.
Now convert mols oxygen to L.
mols O2 x 22.4L= ?
There is a shortcut you can use if you wish. Since all are gases, you may omit the mols step at the front and back and just convert L H2S to L O2 directely using the coefficients as above
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