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.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.