Asked by Anonymous
how many liters of ammonia at STP are required to produce 4.65 grams of hydrogen fluoride?
Answers
Answered by
DrBob222
What are you reacting the NH3 with?
Answered by
Anonymous
fluorine
Answered by
DrBob222
You may have a different equation but this is what I have.
2NH3 + 6F2 → 6HF + 2NF3
mols HF = 4.65 g/molar mass HF = ?
Using the coefficients in the balanced equation, convert mols HF to mols NH3.
Then remember that 1 mol NH3 at STP occupies 22.4 L.
2NH3 + 6F2 → 6HF + 2NF3
mols HF = 4.65 g/molar mass HF = ?
Using the coefficients in the balanced equation, convert mols HF to mols NH3.
Then remember that 1 mol NH3 at STP occupies 22.4 L.
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