<h3>Answer:
</h3>
The Empirical formula of copper chloride based on the experiment data is CuCl₃
<h3>Solution and Explanation:
</h3>
- Empirical formula of a compound is the formula that shows simplest whole number ratio of the atoms contained in a particular compound.
- It may be found when the percentage composition by mass or the mass of each atom in the compound is known.
In this case we first determine the mass of each atom in the compound from data given.
<h3>Step 1: Average mass of copper.
</h3>
Mass of copper in Trial A = 1.694 - 0.908 = 0.786
Mass of copper in Trial B = 1.693 - 0.922 = 0.771
Mass of copper in Trial C = 1.588 - 0.919 = 0.669
Average mass of copper = (0.786 + 0.771 + 0.669) ÷ 3
= 0.742 g of Copper
<h3>Step 2: Average Volume of copper chloride </h3>
Volume in Trial A = 49.6 ml
Volume in Trial B = 48.3 ml
Volume in Trial C = 42.2 ml
Average volume of copper chloride = (49.6 + 48.3 + 42.2) ÷ 3
= 46.7 ml or
= 0.046 L
But we are given 42.62 g of copper chloride in a liter, therefore;
<h3>Step 3: Mass of copper Chloride in the average Volume </h3>
Using proportions
1 L = 42.62 g Copper chloride
0.046 L will contain;
= (42.62 g CuClₓ × 0.0467 L) ÷ 1
= 1.99 g Copper Chloride
<h3>Step 4: Mass of chlorine
</h3>
Mass of chlorine = Mass of copper chloride – mass of copper
= 1.99 g – 0.742 g
= 1.24 g chlorine
<h3>Step 5: Moles of each atom in the compound (copper chloride)
</h3>
Moles = mass / atomic mass
Moles of copper = 0.742 g / 63.55 g/mol
= 0.0117 moles copper
Moles of Chlorine = 1.24 g/35.45 g/mol
= 0.0350 moles Chlorine
<h3>Step 6: Mole ratio </h3>
Copper: Chlorine
0.0117 moles : 0.0350 moles
= 1 : 2.98
= 1 : 3 (whole number ratio)
Therefore, the empirical formula of copper chloride is CuCl₃
