caitieidson15191 caitieidson15191
  • 03-08-2018
  • Chemistry
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If 25.16 g of chlorine react with 12.99 g of manganese metal, what is the empirical formula of the compound?

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Chlidonias
Chlidonias Chlidonias
  • 03-08-2018

We use the given masses of the reactants to calculate the moles of Mn and Cl. Empirical formula represents the simplest mole ratio of atoms present in a compound.

Moles of Mn = [tex] 12.99 g Mn * \frac{1 mol Mn}{54.94 g Mn} = 0.236 mol Mn [/tex]

Moles of Cl = [tex] 25.16 g Cl_{2} *\frac{1 mol Cl_{2}}{70.91 g Cl_{2}} * \frac{2 mol Cl}{1 mol Cl_{2}} [/tex] = 0.710 mol Cl

Simplest mole ratio: [tex] Mn_{\frac{0.236}{0.236}}Cl_{\frac{0.710}{0.236}} [/tex]

So the empirical formula is [tex] MnCl_{3} [/tex]

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