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8090 [49]
3 years ago
9

A chemist adds of a M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has add

ed to the flask. Round your answer to significant digits.
Chemistry
1 answer:
weqwewe [10]3 years ago
3 0

corrected question: A chemist adds 135mL of a 0.21M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has added to the flask. Round your answer to significant digits.

Answer:

5.37g

Explanation:

0.21M means ; 0.21mol/dm³

1dm³=1L , so we can say 0.21mol/L

if 0.21mol of Zinc nitrate is contained in 1L of water

x   will be contained in 135mL of water

x= 0.21*135*10³/1

=0.02835moles

number of moles=  mass/ molar mass

mass= number of moles *molar mas

molar mass of Zn(NO₃)₂=189.36 g/mol

mass= 0.02835 *189.36

mass=5.37g

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Answer:

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Explanation:

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In this case:

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Replacing:

\frac{0.730 L}{301K}=\frac{V2}{273K}

Solving:

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<u><em>The volume of the air is 0.662 L</em></u>

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