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Furkat [3]
3 years ago
14

What is the volume of 2.1 moles of chlorine gas (Cl2) at standard temperature and pressure (STP)?

Chemistry
1 answer:
uysha [10]3 years ago
5 0
Given:
<span> 2.1 moles of chlorine gas (Cl2) at standard temperature and pressure (STP)
Required:
volume of CL2
Solution:
Use the ideal gas law
PV = nRT
V = nRT/P
V = (2.1 moles Cl2) (0.08203 L - atm / mol - K) (273K) / (1 atm)
V = 47 L</span>
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Taking advantage of their large differences in pKa values, describe how a mixture of phenol and benzoic acid in diethyl ether so
Marat540 [252]

Answer:

By adding bicarbonate.

Explanation:

The pka of the phenol (C₆H₅OH) is 10 and the pka of the benzoic acid (C₆H₅COOH) is 4, which means that the benzoic acid is a stronger acid than phenol, so if we want to separate phenol from benzoic acid in diethyl ether we need to first use a weak base that will react with benzoic acid and not with the phenol:  

C₆H₅-COOH + HCO₃⁻  ⇄  C₆H₅-COO⁻  +  H₂CO₃

C₆H₅-OH + HCO₃⁻  ⇄  no reaction

The reaction of the benzoic acid with bicarbonate will produce the benzoate ion that will be soluble in the aqueous layer, while the phenol will remain dissolved in the organic layer, so we can separate the two of them by the separation of the two immiscible layers.      

Having the two layers separated, the benzoic acid can be recovered from the aqueous layer by adding HCl:

C₆H₅-COO⁻ + HCl  ⇄  C₆H₅-COOH + Cl⁻

<u>This acid will precipitate from the aqueous solution, and the solid can be isolated by filtration</u>.  

The phenol in the organic layer can be dissolved into an aqueous layer by the adding of a strong base like NaOH:

C₆H₅-OH + OH⁻  ⇄  C₆H₅-O⁻ + H₂O

The phenoxide ion soluble in the aqueous layer can be recovered later by the adding of HCl, which will form the original phenol:

C₆H₅-O⁻ + HCl  ⇄  C₆H₅-OH + Cl⁻  

<u>The precipitated phenol can be isolated by filtration. </u>

This way we can separate a mixture of phenol and benzoic acid in diethyl ether solution.  

I hope it helps you!

6 0
3 years ago
How many moles of carbon dioxide are present in 14g of co2
Tomtit [17]

0.32 moles

You just do 14/ 44.01 (the atomic mass of carbon + oxygen's atomic massX2)

8 0
3 years ago
Using the molarity equation, calculate how many grams of salt you need in order to make 80ml of a 2M solution (MW = 58.44g/mole)
ollegr [7]

Answer:

9.35g

Explanation:

The molarity equation establishes that:

\textrm{molarity}=\frac{\textrm{moles  of solute}}{\textrm{liters of solution}}

So, we have information about molarity (2M) and volume (80 ml=0.08 l), with that, we can find the moles of solute:

\textrm{moles of solute}=\textrm{molarity}*\textrm{liters of solution}

\textrm{moles of solute}= 0.08 \textrm{ l} *2\textrm{ M} = 0.16 \textrm{ mol}

The  mathematical equation that establishes the relationship between molar weight, mass and moles is:

\textrm{molar weight}= \frac{\textrm{mass}}{\textrm{moles}}

\textrm{MW}= \frac{\textrm{m}}{\textrm{n}}

We have MW (58.44g/mole) and n (0.16 mol), and we need to find m (grams of salt needed) to solve the problem:

\textrm{m} = \textrm{MW * n}= 58.44\frac{\textrm{g}}{\textrm{mol}} * 0.16 \textrm{ mol} = 9.35 \textrm{ g}

8 0
3 years ago
Name the three parts of the atom.
mart [117]
A. Protons, neutrons, and electrons
6 0
3 years ago
In your home, you can turn off your television set but all of your other appliances will stay on. This is because the appliances
Leto [7]

Answer:

in parallel

Explanation:

4 0
3 years ago
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