Question

part a
0.665 mol magnesium fluoride
m$_{\text{mgf}_2}$ =
\boxed{} g
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Explanation:

Step1: Find molar mass of MgF₂

Molar mass of Mg: \(24.305\space g/mol\), F: \(18.998\space g/mol\). For \(MgF_2\), molar mass \(M = 24.305 + 2\times18.998 = 24.305 + 37.996 = 62.301\space g/mol\).

Step2: Calculate mass using \(m = n\times M\)

Given \(n = 0.665\space mol\), \(M = 62.301\space g/mol\). So \(m = 0.665\times62.301\approx 41.43\space g\).

Answer:

\(41.4\) (or more precise \(41.43\))