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2 years ago

If a 10.0ml sample of unknown liquid has a mass of 7.553g what is the density of the unknown liquid

Chemistry

1 answer:

Burka [1]2 years ago

6 0

The density of the unknown liquid has a mass of 7.553g is 0.7553 g/ml

<h3>What is density?</h3>

Density is the measurement of how tightly a material is packed together.

Given data:

Weight =7.553g

Volume = 10.0ml

Density = $\frac{mass}{volume}$

Density = $\frac{7.553g}{10.0ml}$

Density = 0.7553 g/ml

Hence, the density of the unknown liquid has a mass of 7.553g is 0.7553 g/ml.

Learn more about density here:

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Be sure to answer all parts. For an aqueous solution of sodium chloride (NaCl), determine the molarity of 4.05 L of a solution t

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Answer:

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Explanation:

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Volume of solution = $25.35\ \text{L}$

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A compound is 2. 00% H by mass, 32. 7% S by mass, and 65. 3% O by mass. What is its empirical formula? The final step is to use

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Given the following data:

Percentage of H = 2.00%

Percentage of S = 32.7%

Percentage of O = 65.3%

Scientific data:

Molar mass of hydrogen (H) = 1.0 g/mol.

Molar mass of sulfur (S) = 32 g/mol.

Molar mass of oxygen (O) = 16 g/mol.

To determine the empirical formula of this compound:

Note: We would assume that the mass of the compound is 100 grams.

Hence, the mass of its constituent elements are:

Mass of hydrogen (H) = 2.00 grams

Mass of sulfur (S) = 32.7 grams

Mass of oxygen (O) = 65.3 grams

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$Number\;of\;moles = \frac{2.00}{1}$

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For sulfur (S):

$Number\;of\;moles = \frac{32.7}{32}$

Number of moles = 1.0 moles

For oxygen (O):

$Number\;of\;moles = \frac{65.3}{16}$

Number of moles = 4.0 moles

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