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OLEGan [10]
3 years ago
5

In the Bohr model, which of the following electron transitions in a hydrogen atom results in the emission of the highest-energy

photon?
n = 3 to n = 2 OR n = 4 to n =3

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Chemistry
1 answer:
NISA [10]3 years ago
3 0

Answer:

n = 3 to n = 2

Explanation:

The Rydberg formula for electron transitions in the hydrogen atom is given by:

1/λ = Rh( 1/n₁² - 1/n₂² )

where

1/λ = wavelength of the transition,

Rh = Rydberg constant,

n₁ and n₂ are the principal quantum numbers of the energy levels involved in the transition with n₂ greater n₁.

The energy of the photon is given by

E = hc/λ

where

h= Planck´s constant

c= speed of light

Therefore the energy is inversely proportional to the wavelength and the term ( 1/n₁² - 1/n₂² )  will be greater  ( 1/2² - 1/3² ) than (1/3² - 1/4² )  ( 0.14 vs 0.05 ). So the transition from n= 3 to n=2 will result in the emission of the highest energy photon in this question.

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At a certain temperature the vapor pressure of pure methanol is measured to be . Suppose a solution is prepared by mixing of met
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Answer:

Partial pressure is 0.13 atm

Explanation:

CHECK THE COMPLETE QUESTION BELOW :

At a certain temperature, the vapor pressure of pure methanol is measured to be 0.43atm. Suppose a solution is prepared by mixing 88.2 g of methanol and 116.g of water. Calculate the partial pressure of methanol vapor above this solution. Be sure your answer has the correct number of significant digits. Note for advanced students: you may assume the solution is ideal.

Using Raoult´s law for ideal soultions we have

P(A) = X(A) *Pº(A)

where P(A) is the partial vapor pressure pressure of methanol,

X(A) is the mole fraction of solute (methanol) in solution,

Pº(A) is the vapor pressure of pure solute

Raoult's law states that the vapor pressure of a solution is dependent on the mole fraction of a solute added to the solution.

Raoult's law can be expressed below

Psolution = ΧsolventP0solvent.

Expressing it interns of the constituents given in the question we have

P(CH₃OH) = X(CH₃OH) x Pº(CH₃OH)

To calculate the mole fraction of CH₃OH, we make use of the formula below :

X(A) = mol (A) / ntotal

Ntotal = (sum of number of moles of A )+( moles solvent)

mol (CH₃3OH) can be calculated as :: 88.2 g/ 32 g/mol = 2.76 mol of CH₃OH

mol (H₂O) can be calculated as ::116 g/ 18 g/mol = 6.44 mol

total n = (6.44 + 2.76) mol = 9.20 mol

To calculate the partial pressure the we say;

P(CH₃OH) = (2.76 mol CH + 9.20 mol) x( 0.43 atm) = 0.13 atm

Hence, the partial pressure rounded to two significant figures is 0.13 atm

8 0
3 years ago
Which bond is formed when a fatty acid is attached to a glycerol<br> molecule?<br> 2 of 8 QU
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Explanation: Hope this helps!

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Why brain remembers picture better than words?​
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A 1-liter bag of iv solution would contain how many cubic centimeters of fluid?
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A 1-liter bag of IV solution would contain how many cubic centimeters of fluid?

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8 0
3 years ago
IF 14.07*10^26 molecules of magnesium chloride was produced in the following reaction, how many grams of magnesium reacted?
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Answer:

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Explanation:

First, we need to convert the number of molecules of magnesium chloride (MgCl2) into moles by dividing by Avagadro's number (6.02 × 10^23 molecules)

n = nA ÷ 6.02 × 10^23

n = 14.07 × 10^26 ÷ 6.02 × 10^23

n = 14.07/6.02 × 10^(26-23)

n = 2.34 × 10^3 moles of MgCl2

The balanced reaction given in the question is as follows:

Mg + 2HCl → MgCl2 + H2

If 1 mole of Mg produced 1 mole of MgCl2

Then, 2.34 × 10^3 moles of Mg will also produce 2.34 × 10^3 moles of MgCl2.

Using mole = mass ÷ molar mass (MM)

Molar mass of Mg = 24g/mol

mass = mole × MM

mass = 2.34 × 10^3 × 24

mass = 56.16 × 10^3

mass = 56160grams.

6 0
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