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2 years ago

6

One of the wavelengths of light emitted by hydrogen atoms is 6.56 x 10-7 m. Calculate the Energy.

1 answer:

vovikov84 [41]2 years ago

3 0

The Energy of an atom of hydrogen with wavelength 6.56 × 10⁻⁷ m is
3.028 × 10⁻¹⁹ J.

I attached the working out and the answer to the question below.

Please note that C = speed of light, ν = frequency, λ= wavelength, h = Planck's Constant

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3 years ago

Hydrogen atoms absorb energy so that the electrons are excited to n=4. Calculate the wavelength, in

FromTheMoon [43]

Answer:

the wavelength, in nm, of the photon is 487.5 nm

Explanation:

Given:

n = 4 (excited)

n = 2 (relaxes)

Question: Calculate the wavelength, in nm, λ = ?

First, it is important to calculate the energy of the electron when it excited and then when it relaxes.

$E_{1} =\frac{-13.6}{n^{2} } =\frac{-13.6}{4^{2} } =-0.85eV$ (excited)

$E_{2} =\frac{-13.6}{2^{2} } =-3.4eV$ (relaxes)

The change of energy

ΔE = E₁ - E₂=-0.85 - (-3.4) = 2.55 eV = 4.08x10⁻¹⁹J

For a photon, the wavelength emitted

$\lambda =\frac{hc}{delta(E)}$

Here

h = Planck's constant = 6.63x10⁻³⁴J s

c = speed of light = 3x10⁸m/s

Substituting values:

$\lambda =\frac{6.63x10^{-34}*3x10^{8} }{4.08x10^{-19} } =4.875x10^{-7} m=487.5nm$

8 0

2 years ago

What is the molarity of a solution that contains 0.220 moles KOH in 0.350 L of solution?

Lera25 [3.4K]

Answer:

0.628 M.

Explanation:

In order to solve this problem we need to keep in mind the<em> definition of molarity</em>:

Molarity = moles / liters

We are given both the <em>number of moles and the volume of solution</em>, meaning we can now proceed to <u>calculate the molarity</u>:

Molarity = 0.220 mol / 0.350 L

Molarity = 0.628 M

5 0

2 years ago