Aluminum and iron (III) oxide, Fe2O3, react to form aluminum oxide, Al2O3, and ironFor each mole of aluminum used, 426.9 kJ of energy is released under standard conditionsWrite the thermochemical equation that shows the consumption of 4 mol of Al(All of the substances are solids)Please help me how the chemical equation is sopposed to look like as wellIm sooo stucked! Please help!
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This looks like a single replacement reaction, but I can be wrongOfcourse you know that risk when asking on here Single replacement: A+BC AC +B, in this case A is aluminum, B is iron and C is oxideAl + Fe203 Al2O3 + Fe, Then balance it so: 2Al + Fe203 Al2O3 + 2Fe It didn't really ask to solve any quantity in terms of energy so I guess I've leave it at that.
