Colorful fireworks often involve the decomposition of barium nitrate and potassium chlorate and the reaction of the metals magnesium, aluminum, and iron with oxygen.

Write separate balanced equations for the reactions of the solid metals magnesium, aluminum, and iron with diatomic oxygen gas to yield the corresponding solid metal oxides. (Assume the iron oxide contains Fe3 ions. Use the lowest possible whole number coefficients. Include states-of-matter under the given conditions in your answer.) Magnesium

4Al(s) + 3O2(g) >2Al2O3(s)

2Mg(s) + O2(g) >2MgO(s)

3Fe(s) + 2O2(g) > Fe3O4(s)

Explanation:

Aluminum reacts with moist air forming a coat of aluminum oxide. This oxide formed prevents further reaction of the metal with atmospheric oxygen or water under normal circumstances.

Magnesium undergoes oxidation in moist air forming a film of magnesium oxide because it is a very electripositive metal and has strong affinity for oxygen.

Iron on exposure to air, gradually rusts as a result of the hydrated iron (111) oxide formed. This reaction continues until all the iron has been converted to the oxide as the iron (III) does not prevent further reaction.

But on heating, finely divided iron combines with oxygen to firm iron (II) diiron(III) oxide.

the temperature of the gas, in k, not celsius.