1. Use the following balanced net ionic equation to determine the volume of 6.0 M HNO3 needed to react completely with 5.00 g of copper.

8H+(aq) + 2NO3-(aq) + 3Cu(s) → 2NO(g) + 4H2O(l) + 3Cu2+(aq)

mols Cu = grams/atomic mass = ?

Use the equation to convert mols Cu to mols H^+.
Then M HNO3 = mols H^+/L HNO3. YOu know mols H^+ and M HNO3, solve for L HNO3.

To determine the volume of 6.0 M HNO3 needed to react completely with 5.00 g of copper, you need to follow these steps:

1. Determine the molar mass of copper (Cu).
- The molar mass of copper is 63.55 g/mol.

2. Calculate the moles of copper (Cu) used.
- Moles = mass / molar mass
- Moles of Cu = 5.00 g / 63.55 g/mol

3. Use the coefficients in the balanced equation to determine the moles of HNO3 needed.
- From the balanced equation, the ratio of Cu to HNO3 is 3:8
- Moles of HNO3 = (moles of Cu) x (8 moles of HNO3 / 3 moles of Cu)

4. Calculate the volume of 6.0 M HNO3 needed using the molarity equation.
- Molarity (M) = Moles / Volume (L)
- Rearrange the equation to solve for volume:
Volume (L) = Moles / Molarity
- Since the given concentration of HNO3 is 6.0 M and we know the moles of HNO3, we can now calculate the volume:
Volume of HNO3 = (moles of HNO3) / (6.0 mol/L)

By following these steps, you can determine the volume of 6.0 M HNO3 needed to react completely with 5.00 g of copper using the balanced net ionic equation given.