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Readme [11.4K]
3 years ago
13

What is the total number of distinct 13C NMR signals that may be observed for the product, methyl-3-nitrobenzoate, and for the r

eactant, methylbenzoate?What is the total number of distinct 13C NMR signals that may be observed for the product, methyl-3-nitrobenzoate, and for the reactant, methylbenzoate?

Chemistry
1 answer:
tigry1 [53]3 years ago
8 0

Answer:

See explaination

Explanation:

methyl-3-nitrobenzoate = 3-NO2-C6H4-COOCH3

Singlet at 4 ppm = CH3 from ester (COOCH3)

Triplet at 7.6 ppm = Aromatic, H5 proton

Doublet at 8.2 ppm - Aromatic, H4 and H6 protons

Singlet at 8.8 ppm - Aromatic, H2 proton

See attached file for diagrammatic representation and further solution.

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Which of the following is a chemical change?
FromTheMoon [43]

<u>Answer:</u>

<em>Silver tarnishing as the silver metal reacts with sulphur is a chemical change.</em>

<u>Explanation:</u>

Tarnishing is the process of chemical change occurring on the surface of objects leading to corrosion or other defects on the surface. The remaining options like dilution, eroding is a physical change where the concentration of salt and rock particles will be decreased, respectively.

Similarly for soil drying also the concentration of water will be decreased leading to a physical change from wetty or dry soil.

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4 0
3 years ago
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What is a single celled orginium able to do
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Which of the following natural resources cant be reused
ohaa [14]
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6 0
3 years ago
How many grams in 11.9 moles of sulfur? Avogadro’s number: 6.02x1023 atoms = 1 mole Molar mass of sulfur: 32.06 g sulfur = 1 mol
sergiy2304 [10]

Answer:

Mass = 0.37 g

Explanation:

Given data:

Number of moles of sulfur = 11.9 mol

Mass of sulfur in 11.9 mol = ?

Molar mass of sulfur = 32.06 g

Solution:

Number of moles = mass/molar mass

by putting values,

11.9 mol = mass/ 32.06 g/mol

Mass = 11.9 mol × 32.06 g/mol

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4 0
3 years ago
How many photons are produced in a laser pulse of 0.862 J at 691 nm?
Inga [223]
To calculate how many photons are in a certain amount of energy (joules) we need to know how much energy is in one photon.
Start by using two equations:
Energy of a photon = Frequency * Planck's constant (6.626 * 10^(-34) J-s)
Speed of light (constant 3 * 10^8 m/s) = Frequency * Wavelength
Which means:
frequency = Speed of Light / Wavelength
So energy of a photon = (Speed of light * Planck's constant)/(Wavelength)
You may have seen this equation as E = hc/<span>λ</span>
We have a wavelength of 691 nm or 691 * 10^-9 meters
So we can plug in all of our knowns:
E = (6.626 * 10^(-34) J-s) * (3.00 * 10^8 m/s) / (691 * 10^-9 m) = 
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Now we have joules per photon, and the total number of joules (0.862 joules)
,so divide joules by joules per photon, and we have the number of photons:
0.862 J/ (2.88 * 10^(-19) J/photon) = 3.00 * 10^18 photons.

4 0
3 years ago
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