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bearhunter [10]
3 years ago
15

Choose your favorite super hero that gained their powers from radiation. What

Chemistry
1 answer:
dmitriy555 [2]3 years ago
6 0

Answer:

Copy and paste "Electromagnetic waves are categorized according to their frequency f or, equivalently, according to their wavelength λ = c/f.  Visible light has a wavelength range from ~400 nm to ~700 nm.  Violet light has a wavelength of ~400 nm, and a frequency of ~7.5*1014 Hz.  Red light has a wavelength of ~700 nm, and a frequency of ~4.3*1014 Hz." into google, and the correct website pops up as the first result.

Explanation:

I tried to link the website that I use to convert wavelengths and frequencies into types of light, but it deleted my answer, so I guess we're doing it this way. As for converting the wavelength to energy, the same principles apply as before:

Frequency: ν       Wavelength: λ       Energy: E       Speed of light: C (3.00e8)       Planck's Constant: h (6.626e-34)

ν -> λ    λ = C/ν

λ -> ν    ν = C/λ

For either of these equations, wavelength must be converted to meters or nanometers, depending on the equation.

For ν -> λ, after doing the equation, convert the wavelength into nanometers by dividing by 1e-9.

For converting λ -> ν, convert the wavelength into meters by multiplying by 1e-9.

For energy: E = hν = hc/λ

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Use the reaction and bond information to answer the question. C2H6 → C2H4 H2 Reactant bond energies: H–C = 413 kJ/mol, C–C singl
nlexa [21]

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction.

Bond energy has been defined as the chemical energy possessed by the bonds in the chemical structure. The energy has been conserved in the chemical reaction.

<h3>Is the reaction endothermic or exothermic?</h3>

In the reaction in which bond energy of the reactant has been higher than the product, it has been an exothermic reaction.

In the reaction in which the bond energy of the product is higher than the reactant, it has been an endothermic reaction.

In the given reaction

\rm C_2H_6\;\rightarrow\;C_2H_4\;+\;H_2

The bond energies of reactant has been:

  • H-C bond = 413 kJ/mol
  • C-C bond = 347 kJ/mol

The total bond energy of the reactant has been:

\rm Reactant=6\;\times\;H-C\;bond\;+\;C-C\;bond \\Reactant=6\;\times\;413+347\;kJ/mol\\Reactant=2,825\;kJ/mol

The total bond energy of the reactant has been 2,825 kJ/mol.

The bond energies of product has been:

  • H-C = 413 kJ/mol
  • C=C = 614 kJ/mol
  • H-H = 432 kJ/mol

The total bond energy of the product has been:

\rm Product=4\;\times\;H-C\;bond\;+\;C=C\;bond\;+\;H-H\;bond\\Product=4\;\times\;413\;+\;614\;+\;432\;kJ/mol\\Product=2,698\;kJ/mol

The total bond energy of the product has been 2,698 kJ/mol.

The energy of the reactant has been higher than the energy of the product, Thus, the reaction has been an exothermic reaction, as energy can neither be created nor be destroyed. It has been conserved in the chemical reaction.

Learn more about exothermic reaction, here:

brainly.com/question/26203526

4 0
3 years ago
Is salt water a element
Likurg_2 [28]

no  an example of an element is like hydrogen oxygen carbon

7 0
3 years ago
What amount of SeC16 is needed to produce 4.45 mol of chlorine gas in the
AlladinOne [14]

Answer:

1.48 moles of SeCl6 are needed

Explanation:

Based on the reaction:

SeCl6 + O2 → SeO2 + 3Cl2

<em>1 mole of SeCl6 reacts producing 3 moles of Cl2.</em>

To solve this question we need to use the conversion factor:

1mol SeCl6 = 3mol Cl2

As we want to produce 4.45 moles of Cl2, we need:

4.45 mol Cl2 * (1mol SeCl6 / 3mol Cl2) =

<h3>1.48 moles of SeCl6 are needed</h3>
6 0
3 years ago
Calculate the percent yield of benzyl alcohol Sue obtained when doing the following reaction. Sue started with 2.1 g of benzoic
Pachacha [2.7K]

Answer:

The percent yield is 116.6 %

Explanation:

Step 1: Data given

Mass of benzoic anhydride = 2.1 grams

Mass of sodium borohydride = 0.15 grams

Molar mass of benzoic anhydride = 226.23 g/mol

Molar mass of NaBH4 = 37.83 g/mol

Mass of benzyl alcohol produced = 0.5 grams

Step 2: The balanced equation

C14H10O3 + NaBH4 → C7H6O2 + C7H8O + NaB

Step 3: Calculate moles of C14H10O3

Moles C14H10O3 = Mass / molar mass

Moles C14H10O3 = 2.10 grams / 226.23 g/mol

Moles C14H10O3 = 0.00928 moles

Step 4: Calculate moles NaBH4

Moles NaBH4 = 0.150 grams / 37.83 g/mol

Moles NaBH4 = 0.00397 moles

Step 5: Calculate limiting reactant

For 1 mol of C14H10O3 we need 1 mol of NaBH4 to produce 1 mol of C7H8O

NaBH4 is the limiting reactant. It will completely be consumed ( 0.00397 moles).

C14H10O3 is in excess. There will react 0.00397 moles.

There will remain 0.00928 - 0.00397 = 0.00531 moles

Step 6: Calculate moles of C7H8O

For 1 mol of C14H10O3 we need 1 mol of NaBH4 to produce 1 mol of C7H8O

For 0.00397 of C14H10O3 we need 0.00397 mol of NaBH4 to produce 0.00397 mol of C7H8O

Step 7: Calculate mass of C7H8O

Mass of C7H8O = Moles * molar mass

Mass of C7H8O = 0.00397 moles * 108.14 g/mol

Mass of C7H8O = 0.429 grams = theoretical yield

Step 8: Calculate % yield

% yield = (actual yield/ theoretical yield) * 100%

% yield = 0.5/0.429) *100 %

% yield = 116.6 %

The percent yield is 116.6 %

3 0
4 years ago
Whoever answers my question correctly I'll give 50 points​
Jet001 [13]

Answer:

okii is it on your page

Explanation:

4 0
3 years ago
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