Stoichiometry

[reverdybrune]

When aluminum is heated in oxygen, aluminum oxide is formed. What weight of the oxide can be obtained from 25.0g of the metal?

From my stoichiometry worksheet. (I've done this problem already.)

Note: Re-posted from my old OO.net blog

Comments

[reverdybrune]

Qwertz (on OO.net) commented:

25.00g Al (26.98g/mol) is .93mol Al. Al2O3 (101.96g/mol) contains 2 atoms of Al, so .93mol Al will produce (.93/2)mol, or .47mol of Al2O3. .47mol Al2O3 has mass of 47.92g, so 25.00g Al will produce 47.92g Al2O3.

| 25.00g Al | 1mol Al | 1mol Al2O3 | 101.96g Al2O3 | | 47.92g Al2O3 |
------------------------------------------------------------------------------------- = --------------------
| | 26.98g Al | 2mol Al | 1mol Al2O3 | | |

-Q

[reverdybrune]

I got 47.2 grams, but that's just a difference in the way we rounded. Good job!

BTW~ I notice you're a newbie. Welcome to OO.net. (And my blog, of course.)