# Problem: Copper(II) chloride (CuCl2; 0.98 g) was dissolved in water and a piece of aluminum wire (AL; 0.56 g) was placed in the solution. The blue color due to copper(II) chloride soon faded and a red precipitate of solid copper was observed. After the blue color had disappeared completely, the leftover aluminum wire was removed from the solution and weighed. The mass of the leftover aluminum wire was 0.43 g.1. Calculate the number of moles of (a) copper(II) chloride and (b) aluminum that reacted. 2. What is the mole ratio of copper(II) chloride to aluminum metal? Express to the nearest whole number ratio.3. What happened to the aluminum metal that was consumed in this reaction? Write the formula of the most probable aluminum-containing product.4. Write a balanced chemical equation for the single replacement reaction of copper(II) chloride with aluminum. 5. Would it be possible for the entire piece of aluminum wire (0.56 g) to react with copper(II) chloride used in the procedure described above? Explain your reasoning using the concept of the limiting reactant.

###### FREE Expert Solution

The problem consists of the reaction of copper (II) chloride with aluminum wire in solution.

For it, we´re asked to determine the number of moles of each reactant that reacted, the mole ratio of copper (II) chloride to aluminum metal, the most probable aluminum-containing product, a balanced equation for this reaction, and if it’s possible for all aluminum to react.

Remember that the Molar Mass (MM) relates the mass and the moles of a species.

The expression of this relationship is:

$\overline{){\mathbf{M}}{\mathbf{M}}{\mathbf{=}}\frac{\mathbf{m}\mathbf{a}\mathbf{s}\mathbf{s}}{\mathbf{m}\mathbf{o}\mathbf{l}\mathbf{e}\mathbf{s}}}$

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###### Problem Details

Copper(II) chloride (CuCl2; 0.98 g) was dissolved in water and a piece of aluminum wire (AL; 0.56 g) was placed in the solution. The blue color due to copper(II) chloride soon faded and a red precipitate of solid copper was observed. After the blue color had disappeared completely, the leftover aluminum wire was removed from the solution and weighed. The mass of the leftover aluminum wire was 0.43 g.

1. Calculate the number of moles of (a) copper(II) chloride and (b) aluminum that reacted.

2. What is the mole ratio of copper(II) chloride to aluminum metal? Express to the nearest whole number ratio.

3. What happened to the aluminum metal that was consumed in this reaction? Write the formula of the most probable aluminum-containing product.

4. Write a balanced chemical equation for the single replacement reaction of copper(II) chloride with aluminum.

5. Would it be possible for the entire piece of aluminum wire (0.56 g) to react with copper(II) chloride used in the procedure described above? Explain your reasoning using the concept of the limiting reactant.