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Cu + 4HNO3 → Cu(NO3)2 + 2H2O + 2NO2 | , Phản ứng oxi-hoá khử
Cu | copper | solid + HNO3 | nitric acid | solid = Cu(NO3)2 | copper(ii) nitrate | solid + H2O | water | solid + NO2 | nitrogen dioxide | solid | Temperature: temperature, Other Condition excess chlorine
Introduce
Detailed information about the equation
Reaction conditions when applied Cu + HNO3
- Catalyst: not available
- Temperature: normal
- Pressure: normal
- Other conditions: not available
Reaction process Cu + HNO3
Process: Copper reacts with HNO3 acid solution
Note: HNO3 can oxidate most of metals including weak reducing metals such as Cu. Then, metal is oxidated until a level of high oxidation and creates nitrate salt. If using concentrated HNO3, the product will be NO2, and with diluted solution, NO will be created.
The result of the reaction Cu + HNO3
The phenomenon: Red solid of copper (Cu) dissolves gradually in solution and bubbles appear when reddish brown gas (NO2) is created
Detailed information on the reactants
Information about Cu (copper)
Information about HNO3 (nitric acid)
Detailed information about the products of the reaction
Information about Cu(NO3)2 (copper(ii) nitrate)
Information about H2O (water)
Information about NO2 (nitrogen dioxide)
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The equations for preparation Cu
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
normal
Pressure
normal
Other conditions
normal
Catalyst
normal
Temperature
temperature
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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