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Lelechka [254]
3 years ago
10

2. Calculate the density of a liquid in a beaker. The beaker has a mass of 15 grams when empty. The beaker plus an unknown liqui

d has a mass of 64 grams. What is the density (g/ml) of the liquid if its volume is 10. mL?
Chemistry
1 answer:
Pie3 years ago
5 0

Answer:

The density of the liquid is 4.9 g/ml

Explanation:

Density of a liquid is usually measured by filling a beaker of known weight and known capacity (total volume in ml you can fill it) and weighing it. The difference between the total weight (beaker+liquid) and the beaker weight is the liquid weight. Finally, you must divide <em>liquid weight/volume</em> to obtain density.

For the problem:

beaker=15 g

beaker+liquid=64 g

⇒liquid= 64 g - 15 g = 49 g

density= \frac{mass}{volume} = \frac{49 g}{10 ml} = 4.9 g/ml

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Answer: Option 1.

<u>Explanation:</u>

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6 0
3 years ago
Which element has 19 electrons surrounding the nuclei of its atoms?
QveST [7]
I think its potassium
5 0
3 years ago
Why doesn’t silicone (IV) oxide conduct electricity
choli [55]

Answer:

answer it by yourself and own way

4 0
2 years ago
The balanced equation for water is 2 H2 + O2 to 2 H2O. If I have 21.2g of a product , and I started with 5.6 g of H2, how many g
ANTONII [103]

Since 21.2 g H2O was produced, the amount of oxygen that reacted can be obtained using stoichiometry. The balanced equation was given:  2H₂ + O₂ → 2H₂O and the molar masses of the relevant species are also listed below. Thus, the following equation is used to determine the amount of oxygen consumed.

Molar mass of H2O = 18 g/mol

Molar mass of O2 = 32 g/mol

21.2 g H20 x 1 mol H2O/ 18 g H2O x 1 mol O2/ 2 mol H2O x 32 g O2/ 1 mol O2 = 18.8444 g O2

<span>We then determine that 18.84 g of O2 reacted to form 21.2 g H2O based on stoichiometry. It is important to note that we do not need to consider the amount of H2 since we can derive the amount of O2 from the product. Additionally, the amount of H2 is in excess in the reaction.</span>

7 0
3 years ago
Write the molecular formula for the compound that exhibits a molecular ion at M+ = 112.0499. Assume that C, H, N, and O might be
navik [9.2K]

Answer:

C₆H₁₀NO

Explanation:

In order to arrive at a molecular formula we have to make some assumptions and they are

Assuming there is one ( 1 ) N and one ( 1 ) O that is present in the said molecule

Total mass =   29.998

next step: subtract the total mass from 112.0499 = 82.501

next : assume the presence of 6 carbon atoms in said molecule

Total mass =  6 * 12 = 72

Mass of Hydrogens = 82.501 - 72 = 10.501

∴ number of hydrogens = 10.501 / 1.0078  ≈ 10

Hence Total mass = 29.998 + 82.501  ≈ 112.0499

Finally Molecular formula = C₆H₁₀NO

3 0
3 years ago
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