2006-08-25 02:59:36 · 3 answers · asked by wakeupandlivelife 2 in Science & Mathematics ➔ Chemistry
it really depends on what you are oxidising and what products you want. See example below......
Cuprous Oxide, Cu2O reacts with DILUTE Nitric Acid, HNO3, in the cold to form a solution of Cupric Nitrate, Cu(NO3)2, and Copper, Cu.
Cu2O + 2 HNO3 ==> Cu(NO3)2 + Cu + H2O
Cuprous Oxide, Cu2O reacts with CONC Nitric Acid, HNO3, or with dilute Nitric Acid, HNO3, on heating, when the Cuprous Oxide, Cu2O dissolves with evolution of Nitric Oxide, NO.
3Cu2O + 14HNO3 ==> 6Cu(NO3)2 + 2NO + 7H2O
2006-08-25 03:08:24 · answer #1 · answered by Anonymous · 0⤊ 0⤋
Concentrated! More oxidizer to the ounce! It is a powerful oxidizer in concentrated form, and I have presonally witnessed (well, perpetrated) an out of control reaction of concentrated HNO3 with a hydrocarbon. Luckily it was under a hood and on ice. Else it would have exploded and filled the room with noxious gas.
P.S. don't try this at home; the out of control reaction was SUPPOSED to have been controlled and was carefully set up, and look what happened?
2006-08-25 10:13:57 · answer #2 · answered by Black Dog 6 · 0⤊ 0⤋
CONCentrated
2006-08-25 10:03:56 · answer #3 · answered by metatron 4 · 0⤊ 0⤋