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Al + 6HNO3 → 3H2O + 3NO2 + Al(NO3)3 | , Phản ứng oxi-hoá khử
Al | aluminium | solid + HNO3 | nitric acid | solid = H2O | water | solid + NO2 | nitrogen dioxide | solid + Al(NO3)3 | aluminium nitrate | solid | Temperature: temperature, Other Condition excess chlorine
Introduce
Detailed information about the equation
Reaction conditions when applied Al + HNO3
- Catalyst: not available
- Temperature: normal
- Pressure: normal
- Other conditions: not available
Reaction process Al + HNO3
Process: Al reacts with HNO3 acid solution
Note: Nitric acid HNO3 can oxidize most of metals including weak reducing metals like Al. Metals are oxidized highly and nitrate salt is created. Normally, if concentrated HNO3 solution is used, the product will be NO2, and dilute HNO3 will create NO.
The result of the reaction Al + HNO3
The phenomenon: Silvery white solid (Al) dissolves in solution, and reddish brown Nitrogen dioxide (NO2) gas appears
Detailed information on the reactants
Information about Al (aluminium)
Information about HNO3 (nitric acid)
Detailed information about the products of the reaction
Information about H2O (water)
Information about NO2 (nitrogen dioxide)
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Information about Al(NO3)3 (aluminium nitrate)
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The equations for preparation Al
Catalyst
normal
Temperature
temperature
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
The equations for preparation HNO3
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
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