Question

a compound is analyzed as 33.9% ge and 66.1% cl. what is the empirical formula of the substance? gecl ge₂cl₅ ge₄cl gecl₄

Explanation:

Step1: Assume 100g of the compound

If we assume 100g of the compound, then the mass of Ge is \(m_{Ge}=33.9g\) and the mass of Cl is \(m_{Cl} = 66.1g\).

Step2: Calculate the number of moles of each element

The molar mass of Ge (\(M_{Ge}\)) is \(72.63g/mol\), and the molar mass of Cl (\(M_{Cl}\)) is \(35.45g/mol\).
The number of moles of Ge, \(n_{Ge}=\frac{m_{Ge}}{M_{Ge}}=\frac{33.9g}{72.63g/mol}\approx0.467mol\)
The number of moles of Cl, \(n_{Cl}=\frac{m_{Cl}}{M_{Cl}}=\frac{66.1g}{35.45g/mol}\approx1.865mol\)

Step3: Find the mole - ratio

Divide each number of moles by the smaller number of moles (\(n = 0.467mol\))
For Ge: \(\frac{n_{Ge}}{n}=\frac{0.467mol}{0.467mol}=1\)
For Cl: \(\frac{n_{Cl}}{n}=\frac{1.865mol}{0.467mol}\approx4\)

Answer:

\(GeCl_{4}\)