Al+NH4ClO4--->Al2O3+NO+H2O
1. what mass of NH4ClO4 should be used if 1.50 kg of Aluminum is available?
2.How many moles of AlCl3 would be produced?
3. what mass (in grams) of AlCl3 would be produced?
2006-12-13 04:33:47 · 1 answers · asked by Anonymous in Environment
The first step is always to balance the equation. The Aluminum oxide product in your equation tells us nothing to determine the Aluminum chloride of the last parts of your question. It is also missing the element Chlorine in any product.
A possible equation is:
2 Al + 2 NH4ClO4 ---> Al2O3 + 2 NO + 3 H2O + 2 HCl
but this has no AlCl3 as a product. Some of the Aluminum oxide could react with the HCl to give:
Al2O3 + 6 HCl ---> 2 AlCl3 + 3 H2O
If you are not aware, the mixture you describe is an Incendiary. The link below contains cautions:
2006-12-16 02:51:29 · answer #1 · answered by Richard 7 · 58⤊ 0⤋