Question
assume that 13.5g of AL react with excess HCl according to the following balanced equation, at STP: 2Al(s) + 6HCl(aq) ---> 2AlCl3 + 3H2(g)
how mang liters of H2 at STP are produced?
how mang liters of H2 at STP are produced?
Answers
DrBob222
mols Al = grams/molar mass = ?
Using the coefficients in the balanced equation, convert mols Al to mols H2.
Then remember that 1 mol H2 occupies 22.4 L at STP.
Using the coefficients in the balanced equation, convert mols Al to mols H2.
Then remember that 1 mol H2 occupies 22.4 L at STP.