calculate the amount of heat evolved in the complete oxidation of 8.17g of Al at 25 degrees C and 1 atm pressure. change in H for Al2O3 is -1676kJ/mol.

4Al(s) + 3O2(g)--> 2Al2O3(s)
please giv me the steps to solving this

thanx.

delta H = -1676 kJ/mol
How many mols do you have?
mols = g/molar mass = 8.17 g Al/27 =??
??mols x -1676 kJ/mol = xx kJ.
I rounded for the atomic mass of Al; I think it is 26.98 and you should look up the actual value and use that number instead of my rounded number.