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3 years ago

How do you account for the formation of ethane during chlorination of methane

Chemistry

2 answers:

Brrunno [24]3 years ago

8 0

Answer:

ethane is formed due to side reaction

Explanation:

During chlorination of methane, ethane is formed due to side reaction in termination step by the combination of two methyl free radicals.

Cerrena [4.2K]3 years ago

6 0

Answer:

During chlorination of methane, ethane is formed due to side reaction in termination step by the combination of two methyl free radicals.

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A carbon-carbon triple bond is found in a molecule of

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A triple bond is a type of covalent bond. It involves a sigma bond and two pi bonds (each bond involves 2 electrons). A carbon atom is capable of 4 bonds...a carbon-carbon triple bond is found in all alkynes.

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4 years ago

Two liquids are shaken together in a test tube to produce a uniform liquid that does not separate into layers. Which of the foll

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It most likely would be "miscible" because "soluble" refers to something being able to dissolve in water, "insoluble" is something not being able to dissolve or mix such as oil and water and immiscible is something not being able to mix without forming layers.
Answer is: Miscible.

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3 years ago

Read 2 more answers

The concentration of a biomolecule insdie a rod-shaped prokaryotic cell is 0.0051 M. Calculate the number of molecule inside the

Ann [662]

Answer: The number of molecules inside the cell are $2.2\times 10^6$

Explanation:

We are given a prokaryotic cell, which is in the shape of rod or cylinder.

The equation used to calculate the volume of cylinder is:

$V=\pi r^2h$

where,

V = volume of cell = ?

r = radius of the celle = $\frac{d}{2}=\frac{1.7\mu m}{2}=0.85\mu m=8.5\times 10^{-7}m$ (Conversion factor: $1m=10^6\mu m$ )

h = length of the cell = $3.1\mu m=3.1\times 10^{-6}m$

Putting values in above equation, we get:

$V=(3.14)\times (8.5\times 10^{-7})^2\times 3.1\times 10^{-6}\\\\V=7.033\times 10^{-18}m^3$

To calculate the number of moles for given molarity of solution, we use the equation:

$\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}$

Molarity of biomolecule = 0.0051 M

Volume of solution = $7.033\times 10^{-18}m^3=7.033\times 10^{-15}L$ (Conversion factor: $1m^3=1000L$ )

Putting values in above equation, we get:

$0.0051M=\frac{\text{Moles of biomoleculel}}{7.033\times 10^{-15}L}\\\\\text{Moles of biomolecule}=(0.0051mol/L\times 7.033\times 10^{-15}L)=3.59\times 10^{-17}mol$

According to mole concept:

1 mole of a compound contains $6.022\times 10^{23}$ number of molecules

So, $3.59\times 10^{-17}$ moles of a biomolecule will contain = $(3.59\times 10^{-17}\times 6.022\times 10^{23}=2.2\times 10^6$ number of molecules

Hence, the number of molecules inside the cell are $2.2\times 10^6$

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3 years ago

The product gas is then passed through a concentrated solution of KOH to remove the CO2. After passage through the KOH solution,

Kamila [148]

Answer: The mass percent of nitrogen gas in the compound is 13.3 %

Explanation:

Assuming the chemical equation of the compound forming product gases is:

$\text{Compound}\xrightarrow[CuO(s)]{Hot}N_2(g)+CO_2(g)+H_2O(g)$

Now, the product gases are treated with KOH to remove carbon dioxide.

We are given:

$p_{Total}=726torr\\P_{water}=23.8torr\\$

So, pressure of nitrogen gas will be = $p_{Total}-p_{water}=726-23.8=702.2torr$

To calculate the number of moles of nitrogen, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of nitrogen gas = 702.2 torr = 0.924 atm (Conversion factor: 1 atm = 760 torr)

V = Volume of nitrogen gas = 31.8 mL = 0.0318 L (Conversion factor: 1 L = 1000 mL)

T = Temperature of nitrogen gas = $25^oC=[25+273]K=298K$

R = Gas constant = $0.0821\text{ L. atm }mol^{-1}K^{-1}$

n = number of moles of nitrogen gas = ?

Putting values in above equation, we get:

$0.924atm\times 0.0318L=n\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 298K\\n_{mix}=\frac{0.924\times 0.0318}{0.0821\times 298}=0.0012mol$

To calculate the mass of nitrogen gas, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$

Molar mass of nitrogen gas = 28 g/mol

Moles of nitrogen gas = 0.0012 moles

Putting values in above equation, we get:

$0.0012mol=\frac{\text{Mass of nitrogen gas}}{28g/mol}\\\\\text{Mass of nitrogen gas}=(0.0012mol\times 28g/mol)=0.0336g$

To calculate the mass percent of nitrogen gas in compound, we use the equation:

$\text{Mass percent of nitrogen gas}=\frac{\text{Mass of nitrogen gas}}{\text{Mass of compound}}\times 100$

Mass of compound = 0.253 g

Mass of nitrogen gas = 0.0336 g

Putting values in above equation, we get:

$\text{Mass percent of nitrogen gas}=\frac{0.0336g}{0.253g}\times 100=13.3\%$

Hence, the mass percent of nitrogen gas in the compound is 13.3 %

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4 years ago

What type of battery is your flashlight battery?

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The type of battery is dry cell batteries

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3 years ago

How do you account for the formation of ethane during chlorination of methane​

How do you account for the formation of ethane during chlorination of methane