A strip of zinc metal was placed in a beaker that contained 120mL of a solution of copper(2) nitrate, Cu(NO3)2(aq). The mass of the copper produced was 0.813g. Find the initial concentration of the solution of copper(2)nitrate.

Can u help me out with making the balanced chemical equation and stating the gives and unknowns then I will try to do the rest..hmm... lets see if I get it right this time:D

Thanks!!

Zn + Cu(NO3)2 ==> Zn(NO3)2 + Cu

You know grams Cu produced which should allow you to calculate the mols Cu(NO3)2 initially.
You now know mols, you want mols/L for M.

0.11 mol

Of course! I'd be happy to help you with the balanced chemical equation and identifying the reactants and products.

The balanced chemical equation for the reaction between zinc metal (Zn) and copper(II) nitrate (Cu(NO3)2) can be written as follows:

Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq)

In this reaction, zinc metal reacts with copper(II) nitrate to form copper metal and zinc nitrate.

Now let's identify the given and unknown quantities:

Given:
- Mass of copper produced = 0.813 g

Unknown:
- Initial concentration of the copper(II) nitrate solution

Please let me know if you have any further questions or if I can assist you with anything else!

Of course! I'd be happy to help you set up the balanced chemical equation and identify the given and unknown quantities.

The reaction you are describing involves the displacement of copper by zinc. The balanced chemical equation for this reaction can be written as:

Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq)

In this reaction, zinc (Zn) displaces copper (Cu) from the copper(II) nitrate solution, resulting in the formation of copper metal and zinc nitrate.

Now, let's identify the given and unknown quantities:
Given:
- Mass of copper produced: 0.813 g
- Volume of copper(II) nitrate solution: 120 mL (which is equivalent to 120 cm³)

Unknown:
- Initial concentration of the copper(II) nitrate solution (Cu(NO3)2(aq))

To find the initial concentration of the copper(II) nitrate solution, we need to use the given mass of copper produced and the balanced chemical equation. Here's how:

1. Determine the number of moles of copper produced:
- Convert the mass of copper produced (in grams) to moles using the molar mass of copper (Cu), which is 63.55 g/mol. Divide the given mass by the molar mass to find the number of moles of copper.

2. Use the stoichiometry of the balanced chemical equation:
- From the balanced equation, you can see that one mole of copper(II) nitrate (Cu(NO3)2) reacts with one mole of copper (Cu).
- Since the reaction is 1:1, the number of moles of copper is equal to the number of moles of copper(II) nitrate.

3. Calculate the molarity (concentration) of the copper(II) nitrate solution:
- The molarity (M) is defined as moles of solute per liter of solution.
- Convert the given volume of the solution (120 mL) to liters (L).
- Divide the number of moles of copper(II) nitrate by the volume in liters to find the concentration in moles per liter.

Once you have the concentration in moles per liter, you can convert it to the desired units, such as mol/dm³ or g/L, if necessary.

I hope this helps! Let me know if you have any further questions or if there's anything else I can assist you with.