(NH4)2 CR2 O7 –> N2+ CR2O3 + H2O
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12 января 2025 20:43
The reaction you provided is the thermal decomposition of ammonium dichromate ((NH_4)_2Cr_2O_7). When heated, it decomposes to form nitrogen gas ((N_2)), chromium(III) oxide ((Cr_2O_3)), and water ((H_2O)).
To balance the reaction, we can start by writing the unbalanced equation:
[ (NH_4)_2Cr_2O_7 \rightarrow N_2 + Cr_2O_3 + H_2O ]
Balancing the Equation:
Count the number of each element on both sides of the equation.
On the left (reactants):
- Nitrogen (N): 2 (from ((NH_4)_2))
- Hydrogen (H): 8 (from ((NH_4)_2))
- Chromium (Cr): 2 (from (Cr_2O_7))
- Oxygen (O): 7 (from (Cr_2O_7))
On the right (products):
- Nitrogen (N): 2 (from (N_2))
- Hydrogen (H): 2 (from (H_2O) - to be balanced)
- Chromium (Cr): 2 (from (Cr_2O_3))
- Oxygen (O): 3 (from (Cr_2O_3)) + 1 (from (H_2O)) = 4
Balance the Hydrogen: Since there are 8 hydrogens on the left, we need 4 water molecules on the right to balance hydrogen: [ (NH_4)_2Cr_2O_7 \rightarrow N_2 + Cr_2O_3 + 4H_2O ]
Now recap the counts on the right:
- N: 2 (from (N_2))
- H: 8 (from (4H_2O))
- Cr: 2 (from (Cr_2O_3))
- O: 3 (from (Cr_2O_3)) + 4 (from (4H_2O)) = 7
The balanced chemical reaction is then:
[ (NH_4)_2Cr_2O_7 \rightarrow N_2 + Cr_2O_3 + 4H_2O ]
This equation shows that one mole of ammonium dichromate decomposes to yield one mole of nitrogen gas, one mole of chromium(III) oxide, and four moles of water.
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