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iris [78.8K]
2 years ago
12

A 66.4 gram sample of Ba(ClO4)2 3 H2O was heated thoroughly in a porcelain crucible, until its weight remained constant. After h

eating, how many grams of the anhydrous compound remained?
Chemistry
1 answer:
PSYCHO15rus [73]2 years ago
3 0

Answer:

57.2 g

Explanation:

First we <u>convert 66.4 grams of Ba(ClO₄)₂·3H₂O into moles</u>, using its <em>molar mass</em>:

  • Molar mass of Ba(ClO₄)₂·3H₂O = Molar mass of Ba(ClO₄)₂ + (Molar Mass of H₂O)*3
  • Molar mass of Ba(ClO₄)₂·3H₂O = 390.23 g/mol
  • 66.4 g ÷ 390.23 g/mol = 0.170 mol Ba(ClO₄)₂·3H₂O

0.170 moles of Ba(ClO₄)₂·3H₂O would produce 0.170 moles of 0.170 moles of Ba(ClO₄)₂. Meaning we now <u>convert 0.170 moles of Ba(ClO₄)₂ into grams,</u> using the molar mass of Ba(ClO₄)₂:

  • 0.170 mol * 336.23 g/mol = 57.2 g
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