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andreyandreev [35.5K]
3 years ago
14

Use the Rydberg equation to calculate the wavelength (in Å) of the photon absorbed when a hydrogen atom undergoes a transition f

rom n = 1 to n = 3.
Chemistry
1 answer:
ivolga24 [154]3 years ago
7 0

Answer:

1024Å

Explanation:

The Rydberg equation is an empirical relationship equation expressed by Balmer and Rydberg which is given as:

1/λ = R_{H} (\frac{1}{n_{f} ^{2} }-\frac{1}{n_{i} ^{2} }  ).............................(1)

where R_{H} is the Rydberg constant given as 1.09 x 10^{7}m^{-1}, n is the transition level and the subscript f and i show the final and initial level numbers respectively. λ is the wavelength.

n_{f}= 1

n_{i} = 3

Using equation (1), we have

1/λ = 1.097 x 10^{7}(\frac{1}{3^{2} }- \frac{1}{1^{2} })

    = 1.097 x 10^{7} (\frac{1}{9} -\frac{1}{1} )

      = 1.097 x 10^{7}(0.11-1)

       = 1.097 x 10^{7} (-0.89)

       = - 9763300

λ = -\frac{1}{9763300}

   = -1.024x 10^{-7}m

We should note that the negative sign we have is as a result of photon absorption whereby the hydrogen atom gains energy to undergo a transition from the lower energy level to a higher one. Wavelength does not have a negative value.

To convert to Å, we have

λ = \frac{1.024 x 10^{-7} }{10^{-10} } = 1024Å  

Therefore the wavelength of the photon in Å  is 1024Å

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A solution was prepared by dissolving 0.800 g of sulfur S8, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and
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<u>Answer:</u> The freezing point of solution is 16.5°C and the boiling point of solution is 118.2°C

<u>Explanation:</u>

To calculate the molality of solution, we use the equation:

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Where,

m_{solute} = Given mass of solute (S_8) = 0.800 g

M_{solute} = Molar mass of solute (S-8) = 256.52 g/mol

W_{solvent} = Mass of solvent (acetic acid) = 100.0 g

Putting values in above equation, we get:

\text{Molality of solution}=\frac{0.800\times 1000}{256.52\times 100.0}\\\\\text{Molality of solution}=0.0312m

  • <u>Calculation for freezing point of solution:</u>

Depression in freezing point is defined as the difference in the freezing point of water and freezing point of solution.

\Delta T_f=\text{freezing point of acetic acid}-\text{Freezing point of solution}

To calculate the depression in freezing point, we use the equation:

\Delta T_f=iK_fm

or,

\text{Freezing point of acetic acid}-\text{Freezing point of solution}=iK_fm

where,

Freezing point of acetic acid = 16.6°C

i = Vant hoff factor = 1 (for non-electrolyte)

K_f = molal freezing point depression constant = 3.59°C/m

m = molality of solution = 0.0312 m

Putting values in above equation, we get:

16.6^oC-\text{freezing point of solution}=1\times 3.59^oC/m\times 0.0312m\\\\\text{Freezing point of solution}=16.5^oC

Hence, the freezing point of solution is 16.5°C

  • <u>Calculation for boiling point of solution:</u>

Elevation in boiling point is defined as the difference in the boiling point of solution and freezing point of pure solution.

The equation used to calculate elevation in boiling point follows:

\Delta T_b=\text{Boiling point of solution}-\text{Boiling point of acetic acid}

To calculate the elevation in boiling point, we use the equation:

\Delta T_b=iK_bm

or,

\text{Boiling point of solution}-\text{Boiling point of acetic acid}=iK_fm

where,

Boiling point of acetic acid = 118.1°C

i = Vant hoff factor = 1 (for non-electrolyte)

K_f = molal boiling point elevation constant = 3.08°C/m

m = molality of solution = 0.0312 m

Putting values in above equation, we get:

\text{Boiling point of solution}-118.1^oC=1\times 3.08^oC/m\times 0.0312m\\\\\text{Boiling point of solution}=118.2^oC

Hence, the boiling point of solution is 118.2°C

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