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EleoNora [17]
3 years ago
8

If 25.16 g of chlorine react with 12.99 g of manganese metal, what is the empirical formula of the compound?

Chemistry
1 answer:
WARRIOR [948]3 years ago
6 0

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 = 12.99 g Mn * \frac{1 mol Mn}{54.94 g Mn} = 0.236 mol Mn

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

Simplest mole ratio: Mn_{\frac{0.236}{0.236}}Cl_{\frac{0.710}{0.236}}

So the empirical formula is MnCl_{3}

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 <u><em> calculation</em></u>

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H₂C₂O₄.2H₂O  + 2 KOH   →    K₂C₂O₄ +4 H₂O

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from  periodic  table the  molar mass H₂C₂O₄.2H₂O= (1 x2) +(12 x2) +(16 x4)  + 2(18)=126 g/mol

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therefore the  moles of KOH  =0.00159 x 2 = 0.00318  moles

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6 0
3 years ago
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