Question

PLEASE HELP ASAP

Use the equation below to answer the following questions.
2Al(s) + 3Cu(NO3)2(aq) 3Cu(s) + 2Al(NO3)3(aq)

Determine the oxidation state of the atoms in the equation's reactants and products: (6 points)

Oxidation state of Al in reactant:
in product:

Oxidation state of Cu in reactant:
in product:

Oxidation state of N in reactant:
in product:

Oxidation state of O in reactant:
in product:

Explain why this is a redox reaction.

Thank you!

Answer 1

The aluminum and copper change their oxidation states during the reaction, indicating a redox reaction with Al being oxidized from 0 to +3 and Cu being reduced from +2 to 0.

Step-by-step explanation:

To determine the oxidation state() of the atoms in the reactants and products of the given equation, we must look at each atom individually:

• Oxidation state of Al in reactant: 0 (as a pure element)
• Oxidation state of Al in product: +3 (in Al(NO3)3)
• Oxidation state of Cu in reactant: +2 (as part of Cu(NO3)2)
• Oxidation state of Cu in product: 0 (as a pure element)
• Oxidation state of N in reactant: +5 (in Cu(NO3)2)
• Oxidation state of N in product: +5 (in Al(NO3)3)
• Oxidation state of O in reactant: -2 (in Cu(NO3)2)
• Oxidation state of O in product: -2 (in Al(NO3)3)

This is a redox reaction because there is a transfer of electrons from one species to another. In the given equation, aluminum is oxidized as its oxidation state increases from 0 to +3, losing electrons. Conversely, copper is reduced as its oxidation state decreases from +2 to 0, gaining electrons.