Jim4592
Sep12-10, 09:42 PM
1. The problem statement, all variables and given/known data
Elemental (metallic) aluminum (Al) is reacted with HCl to yield aluminum chloride (AlCl3) and hydrogen gas (H2). How many grams of metallic aluminum would be required to produce 1 gram of pure hydrogen gas?
2. Relevant equations
Al + HCl --> AlCl3 + H2
Balance Reaction: 2 Al + 6 HCl --> 2 AlCl3 + 3 H2
3. The attempt at a solution
let Z = the amount of Al needed
Z g Al * (1 mol Al / 26.98 g Al) * (3 mol H2/2 mol Al) * (2.02 g H2/1 mol H2) = 1 g H2
(6.04764 * Z) / 53.96 = 1
Z = 8.922 g Al
I was hoping someone could look over this and see if did the correct process and came up with the right answer.
Thanks!
Elemental (metallic) aluminum (Al) is reacted with HCl to yield aluminum chloride (AlCl3) and hydrogen gas (H2). How many grams of metallic aluminum would be required to produce 1 gram of pure hydrogen gas?
2. Relevant equations
Al + HCl --> AlCl3 + H2
Balance Reaction: 2 Al + 6 HCl --> 2 AlCl3 + 3 H2
3. The attempt at a solution
let Z = the amount of Al needed
Z g Al * (1 mol Al / 26.98 g Al) * (3 mol H2/2 mol Al) * (2.02 g H2/1 mol H2) = 1 g H2
(6.04764 * Z) / 53.96 = 1
Z = 8.922 g Al
I was hoping someone could look over this and see if did the correct process and came up with the right answer.
Thanks!