1. Convert Masses to Moles
* Nickel (Ni): 0.587 g Ni / 58.69 g/mol Ni = 0.0100 mol Ni
* Chlorine (Cl): 1.065 g Cl₂ / 70.90 g/mol Cl₂ = 0.0150 mol Cl₂
* Note: We use the molar mass of Cl₂ (70.90 g/mol) because chlorine gas exists as a diatomic molecule (Cl₂).
2. Determine the Mole Ratio
* Divide the number of moles of each element by the smallest number of moles:
* Ni: 0.0100 mol / 0.0100 mol = 1
* Cl: 0.0150 mol / 0.0100 mol = 1.5
3. Find the Simplest Whole Number Ratio
* Since we have a ratio of 1:1.5, we need to multiply both sides by 2 to get whole numbers:
* Ni: 1 x 2 = 2
* Cl: 1.5 x 2 = 3
4. Write the Empirical Formula
* The empirical formula of the nickel chloride product is NiCl₃.
Important Note: Nickel chloride is usually found as NiCl₂. The reaction described in this problem might produce a different, less common form of nickel chloride with a 1:3 ratio of nickel to chlorine.
