Question #ea84f

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Question #ea84f

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Answer 1 · 2017-05-24T11:49:45

$0.40$ $0.40$ mol

Explanation:

You are given CuSO $_{4} \cdot 5$ $""_4*5$ H $_{2}$ $""_2$ O

Strategy: First find the weight of hydrated copper sulfate in grams per mole. Then, using that discovery as a conversion factor, find the number of moles in 100 grams.

Weight of hydrated copper sulfate

Step 1. Get the atomic mass and number of each atom per molecule

Cu: 1 copper atom at 63.456 g/mol
S: 1 sulfur atom at 32.06 g/mol
O $_{4}$ $""_4$ : 4 oxygen atoms at 15.999 g/mol
5(H $_{2}$ $""_2$ ): 10 hydrogen atoms at 1.008 g/mol
5(O): 5 oxygen atoms at 15.999 g/mol

Step 2. Multiply and add the terms of get the number of moles found in one gram.

$1 \times 63.456 + 1 \times 32.06 + 9 \times 15.999 + 10 \times 1.008 = 249.6$ $1xx63.456+1xx32.06+9xx15.999+10xx1.008=249.6$ g/mol

The number of moles
Step 3. Multiply 100 grams times that result as a conversion factor.

$100 g \times (\frac{1 mol}{249.6 g}) = 0.40$ $100" g"xx ((1" mol")/(249.6" g")) =0.40$ mol

Because 1 mole is equivalent to $6.02 \times 10^{23}$ $6.02xx10^23$ objects, there are $2.41 \times 10^{23}$ $2.41xx10^23$ molecules in CuSO $_{4} \cdot 5$ $""_4*5$ H $_{2}$ $""_2$ O.

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Question #ea84f

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