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lisov135 [29]
3 years ago
14

Using the Rydberg formula, calculate the initial energy level when an electron in a hydrogen atom transitions into n= 2 and emit

s a photon at 410.1 nm. Note: the Rydberg constant = 1.097 x 107 m–1 .
Chemistry
2 answers:
Nina [5.8K]3 years ago
6 0

Answer:

n_1=1.459

Explanation:

Hello,

In this case, the Rydberd formula is:

\frac{1}{\lambda}=RZ^2(\frac{1}{n_1^2}-\frac{1}{n_2^2} )

Whereas \lambda is wavelength of photon,  R the Rydberg's constant,  Z the atomic number of the atom, in this case 1 as it is hydrogen,  n_1 is the initial level and n_2 is the final energy level .

In such a way, solving for n_1 one obtains:

\frac{1}{n_1^2}-\frac{1}{n_2^2} =\frac{1}{\lambda RZ^2}\\\frac{1}{n_1^2}=\frac{1}{\lambda RZ^2}+\frac{1}{n_2^2}\\\frac{1}{n_1^2}=\frac{1}{4.141x10^{-7}m*1.097x10^7m^{-1}*1^2}+\frac{1}{2^2} \\\frac{1}{n_1^2}=0.47\\n_1=\sqrt{\frac{1}{0.47}} \\n_1=1.459

Best regards.

EleoNora [17]3 years ago
3 0

Answer:

1

Explanation:

Using the Rydberg formula as:

\frac {1}{\lambda}=R_H\times Z^2\times (\frac {1}{n_{1}^2}-\frac {1}{n_{2}^2})

where,

λ is wavelength of photon

R = Rydberg's constant (1.097 × 10⁷ m⁻¹)

Z = atomic number of atom

n₁ is the initial final level and n₂ is the final energy level

For Hydrogen atom, Z= 1

n₂ = 2

Wavelength = 410.1 nm

Also,

1 nm = 10⁻⁹ m

So,

Wavelength = 410.1 × 10⁻⁹ m

Applying in the formula as:

\frac {1}{410.1\times 10^{-9}}=1.097\times 10^7\times 1^2\times (\frac {1}{n_{1}^2}-\frac {1}{2^2})

Solving for n₁ , we get

n₁ ≅ 1

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Explanation:

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Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.

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8 0
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Please help me out i will give you brainlist. 0.500 is wrong
Alik [6]
<h3>Answer:  b) 0.250 mol</h3>

============================================

Work Shown:

Using the periodic table, we see that

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These are approximations and these values are often found underneath the atomic symbol. For example, the atomic weight listed under carbon is roughly 12.011 grams. I'm rounding to 2 sig figs in those numbers listed above.

So 1 mole of CO2 is approximately 12+2*16 = 44 grams. The 2 is there since we have 2 oxygens attached to the carbon atom.

-------------------

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In short,

11.0 grams of CO2 = 0.250 mol of CO2

This is approximate.

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