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