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. 

FREE Expert Solution
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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:

MM=massmoles


96% (449 ratings)
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. 

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Limiting Reagent concept. You can view video lessons to learn Limiting Reagent Or if you need more Limiting Reagent practice, you can also practice Limiting Reagent practice problems .

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Based on our data, we think this problem is relevant for Professor Griffith's class at UMD.