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2 years ago

How is emission spectra produced?

Chemistry

2 answers:

Scorpion4ik [409]2 years ago

7 0

Answer:

emission spectra are produced by thin gases in which the atoms do not experience many collisions (because of the low density). The emission lines correspond to photons of discrete energies that are emitted when excited atomic states in the gas make transitions back to lower-lying levels.

Explanation:

gulaghasi [49]2 years ago

3 0

Answer:

Atomic emission spectra are produced when excited electrons return to the ground state.

Explanation:

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In one kind of nuclear reaction, two nuclei fuse, or join together, to form a larger nucleus. This kind of reaction happens only

Vladimir79 [104]

High pressures are necessary to create such reaction so that the particles will be able to overcome electrostatic repulsion. The particles that make up a particular atom are covered by shells of energy that react to different impulses like pressure. When particles are exposed to extreme environmental pressure it has the tendency to split its particles and undergo nuclear fusion successfully.

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3 years ago

A nucleotide consists of a phosphate group, a pentose sugar, and a __________________, all linked together by covalent bonds. po

Genrish500 [490]

The correct answer would be the fourth option. A nucleotide consists of a phosphate group, a pentose sugar, and a nitrogen containing base that are all linked together by covalent bonds. Nucleotides are the monomer units of nucleic acids and is the basic unit of the DNA.

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3 years ago

How many liters of nitrogen gas are needed to make 25 mol of nitrogen trifluoride

ikadub [295]

The reaction between N₂ and F₂ gives Nitrogen trifluoride as the product. The balanced equation is;

N₂ + 3F₂ → 2NF₃

The stoichiometric ratio between N₂ and NF₃ is 1 : 2
Hence,
moles of N₂ / moles of F₂ = 1 / 2
moles of N₂ / 25 mol = 0.5
moles of N₂ = 0.5 x 25 mol = 12.5 mol

Hence N₂ moles needed = 12.5 mol

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Hence needed N₂ volume = 22.4 L mol⁻¹ x 12.5 mol
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6 0

3 years ago

A dilute solution of bromine in carbon tetrachloride behaves as an ideal-dilute solution. The vapour pressure of pure CCl4 is 33

ANEK [815]

Explanation:

The given data is as follows.

Vapour pressure of pure $CCl_{4}$ = 33.85 Torr

Temperature = 298 K

Mole fraction of $Br_{2}$ = 122.36 torr

Therefore, calculate the vapor pressure of $Br_{2}$ as follows.

Vapour pressure of $Br_{2}$ = mole fraction of $Br_{2}$ x K of $Br_{2}$

= 0.050 x 122.36 Torr

= 6.118 Torr

So, vapor pressure of $Br_{2}$ is 6.118 Torr .

Now, calculate the vapor pressure of carbon tetrachloride as follows.

Vapour pressure of $CCl_{4}$ = mole fraction of $CCl_{4}$ x Pressure of $CCl_{4}$

= (1 - 0.050) × 33.85 Torr

= 32.1575 Torr

So, vapor pressure of $CCl_{4}$ is 32.1575 Torr .

Hence, the total pressure will be as follows.

= 6.118 Torr + 32.1575 Torr

= 38.2755 Torr

Therefore, composition of $CCl_{4}$ = $\frac{32.1575 Torr}{38.2755 Torr}$

= 0.8405

Composition of $CCl_{4}$ is 0.8405 .

And, composition of $Br_{2}$ = $\frac{6.118 Torr}{38.2755 Torr}$

= 0.1598

Composition of $Br_{2}$ is 0.1598 .

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3 years ago

Hi everyone! :)) How is your day going, let me know!

Masja [62]

Answer:

its doing great!

Explanation:

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3 years ago

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