- #1
RaamGeneral
- 50
- 1
Please don't ignore the template.
Hello, sorry to bother again.
A sample containing Al reacts with an aqueous solution of 5.05 g HCl producing 5.70 L of H2 at 20°C and 742 mmHg.
Find the mass percent of Al in the sample assuming hydrogen behaves like an ideal gas.I can't again understand this exercise, because I've never done any like this before.
The only reaction I know involving aluminium and HCl is:
[tex]\mathrm{2Al+6HCl \to 2AlCl_3 + 3H_2}[/tex]
but it doesn't seem useful.
I calculated 0.139 mol of Al and 0.231 mol of H2 using the ideal gas law.
I can't see any clue about my sample though.
A sample containing Al reacts with an aqueous solution of 5.05 g HCl producing 5.70 L of H2 at 20°C and 742 mmHg.
Find the mass percent of Al in the sample assuming hydrogen behaves like an ideal gas.I can't again understand this exercise, because I've never done any like this before.
The only reaction I know involving aluminium and HCl is:
[tex]\mathrm{2Al+6HCl \to 2AlCl_3 + 3H_2}[/tex]
but it doesn't seem useful.
I calculated 0.139 mol of Al and 0.231 mol of H2 using the ideal gas law.
I can't see any clue about my sample though.