Help please am kind of confused on this problem, am mostly confused on what state the products will be.
Find net ionic equation?
2Al(s)+ 3CuCl3(aq)-> 2AlCl3(?)+ 2Cu(?)
Two questions.
1. The equation isn't balanced as a molecular equation; therefore, one can't take this one and convert to an ionic equation.
2. Do you intend for CuCl3 as a reactant. That gives Cu in a +3 oxidation state which isn't impossible but likely improbable.
To find the net ionic equation, we need to break down the given equation into its ionic components. Here's how you can do it step by step:
Step 1: Write the balanced equation.
2Al(s) + 3CuCl3(aq) -> 2AlCl3(?) + 2Cu(?)
Step 2: Identify the compounds and their states.
In the given equation:
- Al is a solid (s).
- CuCl3 is an aqueous solution (aq).
- AlCl3 is the product of interest, but its state is not specified.
- Cu is another product of interest, but its state is also not specified.
Step 3: Write the ionic equation.
The ionic equation shows the dissociated ions involved in the reaction. Since only the aqueous solution dissociates, we need to break down CuCl3 into its ions.
2Al(s) + 3Cu3+(aq) + 9Cl^-(aq) -> 2AlCl3(?) + 2Cu(?)
Step 4: Write the net ionic equation.
The net ionic equation removes the spectator ions, which are the ions that appear on both sides of the equation and do not participate in the reaction. In this case, Al and Cl ions are spectator ions.
Net ionic equation:
2Al(s) + 3Cu3+(aq) -> 2AlCl3(?) + 2Cu(?)
Please note that the state of AlCl3 and Cu is still undetermined in this net ionic equation, as it was not specified in the original equation.