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IgorC [24]
3 years ago
14

Select the fastest way to differentiate between the organic and aqueous layers of an extraction.a. Hold a white piece of paper b

ehind the separatory funnel. The organic layer will have a slight yellow color, while the aqueous layer will be colorless.b. Add a few drops of one of the layers to a test tube containing 1 mL of water. Shake the test tube to determine the solubility of the layer in water.c. Separate the layers and heat them. The organic layer will have the lowest boiling point.d. Weigh equal volumes of each layer. The aqueous layer will have the highest mass.
Chemistry
1 answer:
valentinak56 [21]3 years ago
6 0

Answer:

b. Add a few drops of one of the layers to a test tube containing 1 mL of water. Shake the test tube to determine the solubility of the layer in water

Explanation:

Option a is not true, it depends on the compound being extracted.

Option c is not true, although most of the solvents used in extractions have lower boiling point than water there are exceptions, for example toluene.

Option  d is not true. Again most of the solvents used in extractions are less dense than water, there are many exceptions, for example chloroform, so for equal volumes the chloroform layer will weigh more.

Option b. is the correct one.

One will test the  miscibility of the layer in water. If it inmiscible then one would know is the organic layer. If it is the aqueous layer then it will completely be miscible.

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What volume. In liters, of H2O(g) measured at STP is produced by the combustion of 15.63 g of natural gas (CH4) according to the
fomenos

Answer:

V = 43.95 L

Explanation:

Given data:

Mass of CH₄ decomposed = 15.63 g

Volume of H₂O produced at STP = ?

Solution:

Chemical equation:

CH₄ + 2O₂    →       2H₂O  + CO₂

Number of moles of CH₄:

Number of moles = mass/molar mass

Number of moles = 15.63 g/ 16 g/mol

Number of moles = 0.98 mol

Now we will compare the moles of H₂O with CH₄.

                         CH₄              :              H₂O

                           1                 :                2

                        0.98             :            2×0.98 = 1.96 mol

Volume of hydrogen:

PV = nRT

1 atm × V = 1.96 mol × 0.0821 atm.L/mol.K × 273.15 K

V = 43.95atm.L / 1atm

V = 43.95 L

3 0
3 years ago
These statements describe three different reactions.
Naily [24]

An atom gains an electron from another atom. Hence, option B is the correct answer.

<h3>What is an atom?</h3>

An atom is a particle of matter that uniquely defines a chemical element. An atom consists of a central nucleus that is usually surrounded by one or more electrons.

When an atom shares electrons with another atom then it results in the formation of a covalent bond.

Whereas when an atom transfer electrons from one atom to another then it results in the formation of an ionic bond.

When the nucleus of an atom splits then it represents a nuclear fission reaction and energy is released during this process.

Hence, option B is the correct answer.

Learn more about the atom here:

brainly.com/question/1566330

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5 0
2 years ago
What information do we need to determine the molecular formula of a compound from the empirical formula?
defon

Answer:

Molecular mass

Explanation:

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Thus if the molecular mass is known, then we can find the value of n which results to molecular formula.

6 0
4 years ago
A 250 mL sample of gas is collected over water at 35°C and at a total pressure of 735 mm Hg. If the vapor pressure of water at 3
ELEN [110]

Answer:

The volume of the gas sample at standard pressure is <u>819.5ml</u>

Explanation:

Solution Given:

let volume be V and temperature be T and pressure be P.

V_1=250ml

V_2=?

P_{total}=735 mmhg

1 torr= 1 mmhg

42.2 torr=42.2 mmhg

so,

P_{water}=42.2mmhg

T_1=35°C=35+273=308 K

Now

firstly we need to find the pressure due to gas along by subtracting the vapor pressure of water.

P_{gas}=P_{total}-P_{water}

=735-42.2=692.8 mmhg

Now

By using combined gas law equation:

\frac{P_1*V_1}{T_1} =\frac{P_2*V_2}{T_2}

V_2=\frac{P_1*}{P_2}*\frac{T_2}{T_1} *V_1

V_2=\frac{P_gas}{P_2}*\frac{T_2}{T_1} *V_1

Here P_2 \:and\: T_2 are standard pressure and temperature respectively.

we have

P_2=750mmhg \:and\: T_2=273K

Substituting value, we get

V_2=\frac{692.8}{750}*\frac{273}{308} *250

V_2= 819.51 ml

4 0
2 years ago
Give five properties of water.
Gelneren [198K]
Polarity, cohesion, adhesion, surface tension, high specific heat, and evaporating cooling
3 0
3 years ago
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