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Tresset [83]
3 years ago
8

Show the empirical formula manganese fluoride; 59.1% Mn and 40.9% F. Fill in the subscripts on the formula below. Make sure to h

ave a whole number of each subscript, even if it is a 1. Mn____ F____.

Chemistry
2 answers:
Alex_Xolod [135]3 years ago
8 0

Answer :  The empirical formula of manganese fluoride is Mn_1F_2.

Solution :  Given,

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of Mn = 59.1 g

Mass of F = 40.9 g

Molar mass of Mn = 54.94 g/mole

Molar mass of F = 18.99 g/mole

Step 1 : convert given masses into moles.

Moles of Mn = \frac{\text{ given mass of Mn}}{\text{ molar mass of Mn}}\times 1\text{ mole of Mn} = \frac{59.1g}{54.94g/mole}\times 1\text{ mole of Mn} = 1.076 moles

Moles of F = \frac{\text{ given mass of F}}{\text{ molar mass of F}}\times 1\text{ mole of F} = \frac{40.9g}{18.99g/mole}\times 1\text{ mole of F} = 2.154 moles

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For Mn = 1.076/1.076 = 1

For F = 2.154/1.076 ≈ 2

Mn : F = 1 : 2 

The mole ratio of the element is represented by subscripts in empirical formula.

Therefore, the Empirical formula = Mn_1F_2



Gre4nikov [31]3 years ago
3 0

Hey there!:

Given % of Mn=59.1% means 59.1 g of Mn present in 100 g of manganese fluoride.

Molar mass of Mn= 54.938 g/mol

Moles of Mn = mass / molar mass

59.1 /54.938 => 1.07 ≈ 1 mol.

and % of F=40.9% means 40.9 g of of F present in 100 g of manganese fluoride.

Molar mass of F=18.998 g/mol

Moles of F :

40.9 / 18.999 => 2.15 mol ≈ 2 mol.

The mole ratio between Mn:F=  1 : 2

Therefore the empirical formula of manganese fluoride:

=> MnF2=Mn1F2

Hope that helps!

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