Aluminium nitrate, represented by the chemical formula Al(NO3)2, is a chemical compound composed of aluminium and nitrate ions. When Al(NO3)2 reacts with chromium, it results in a redox reaction, which involves the transfer of electrons between the reactants.
Redox Reaction:
Al0 - 2 e- → AlII (oxidation)
2 NIII - 4 e- → 2 NV (oxidation)
CrVI + 6 e- → Cr0 (reduction)
In this reaction, Al is oxidized to AlII, which means it loses electrons, while N is oxidized to NV, which means it gains electrons. On the other hand, CrVI is reduced to Cr0, which means it gains electrons. Al acts as a reducing agent, while Cr(NO3)2 acts as both a reducing and oxidizing agent.
Input Interpretation:
The balanced chemical equation for the reaction between Cr(NO3)2 and Al can be represented as follows:
Cr(NO3)2 + Al → Al(NO3)2 + Cr
This equation shows that Al and Cr(NO3)2 react to form Al(NO3)2 and Cr.
Balanced Equation:
To balance the chemical equation algebraically, we can follow these steps:
Add stoichiometric coefficients, c1, to the reactants and products:
c1Cr(NO3)2 + c2Al → c3Al(NO3)2 + c4Cr
Set the number of atoms in the reactants equal to the number of atoms in the products for Cr, N, O and Al:
Cr: c1 = c4
N: 2c1 = 2c3
O: 6c1 = 6c3
Al: c2 = c3
Choose an arbitrary coefficient value to keep the coefficients small. In this example, we will set c1 = 1 and solve the system of equations for the remaining coefficients:
c1 = 1
c2 = 3
c3 = 1
c4 = 1
Substitute the coefficients into the chemical reaction to obtain the balanced equation:
Cr(NO3)2 + 3Al → Al(NO3)2 + Cr