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KatRina [158]
3 years ago
12

A 2.89 g sample of a metal chloride, MCl2, is dissolved in water and treated with excess aqueous silver nitrate. The silver chlo

ride that formed weighed 6.41 g. Calculate the molar mass of M. Question 3 options: 70.9 g/mol 29 g/mol 58.0 g/mol 65 g/mol 72.4 g/mol
Chemistry
1 answer:
dsp733 years ago
6 0

Answer:

58.0 g/mol

Explanation:

The reaction that takes place is:

  • MCl₂ + 2AgNO₃ → 2AgCl + M(NO₃)₂

First we <u>calculate how many moles of silver chloride</u> were produced, using its <em>molar mass</em>:

  • 6.41 g AgCl ÷ 143.32 g/mol = 0.0447 mol AgCl

Then we <u>convert AgCl moles into MCl₂ moles</u>, using the <em>stoichiometric ratio</em>:

  • 0.0447 mol AgCl * \frac{1molMCl_2}{2molAgCl} = 0.0224 mol MCl₂

Now we<u> calculate the molar mass of MCl₂</u>, using the original<em> mass of the sample</em>:

  • 2.86 g / 0.0224 mol = 127.68 g/mol

We can write the molar mass of MCl₂ as:

  • Molar Mass MCl₂ = Molar Mass of M + (Molar Mass of Cl)*2
  • 127.68 g/mol = Molar Mass of M + (35.45 g/mol)*2

Finally we<u> calculate the molar mass</u> of M:

  • Molar Mass of M = 57 g/mol

The closest option is 58.0 g/mol.

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