Asked by eng
If 0.836 g of solid Al reacts stoichiometrically according to the balanced equation in a reaction solution with a total volume of 1160 mL, what mass (g) of gaseous H2 is produced?
6 HClO4(aq) + 2 Al(s) → 3 H2(g) + 2 Al(ClO4)3(aq)
0.836g/molecular weight Al=mole of Al
mole of Al x3/2=mole of H2
mole of H2 x molecular weight H2=gram H2
6 HClO4(aq) + 2 Al(s) → 3 H2(g) + 2 Al(ClO4)3(aq)
0.836g/molecular weight Al=mole of Al
mole of Al x3/2=mole of H2
mole of H2 x molecular weight H2=gram H2
Answers
Answered by
DrBob222
That looks ok to me.