1. ## Chemistry Problem help!

The major source of aluminum in the world is bauxite (mostly
aluminum oxide). Its thermal decomposition can be represented by
If aluminum is produced this way, how many grams of aluminum can
form when 1.000x103 kJ of heat is transferred?

Al2O3(s----> 2Al(s) + 3/2 O2(g) ∆Hrxn = 1676 kJ

MM Al = 26.982 g/mol

2. $\text{Al}_{2}\text{O}_{3 (s)} \rightarrow 2\text{Al}_{(s)} + \frac{3}{2} \text{O}_{2 (g)} \qquad \Delta H_{\text{rxn}} = 1676 \ \text{kJ}$

Treat it as a stoichiometry question with 1676 kJ of heat as the product. Note that the question is saying for every 1 mole of aluminium oxide consumed, 1676 kJ and 2 moles of aluminium is produced. So, by just simply looking at the units so that they cancel:

$\left(1.000 \cdot 10^{3} \ \text{kJ}\right) \ \cdot \ \frac{2 \ \text{mol Al}_{(s)} }{1676 \ \text{kJ} } \ \cdot \ \frac{26.982 \ \text{g} }{1 \ \text{mol Al}_{(s)} } = \hdots$