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Lesson: Energy and Wavelength

Worksheet • 8 Questions

Q1:

In a flame test, bismuth atoms emit photons with an energy of 4.042 eV.

Calculate the wavelength of the emitted photons.

Calculate the energy per mole of emitted photons.

Q2:

Heated barium ions emit photons with an energy of 2.722 eV.

Calculate the wavelength of the emitted photons.

Calculate the energy per mole of emitted photons.

Q3:

Mercury atoms in a high-pressure lamp emit photons with an energy of 6.705 eV.

Calculate the wavelength of the emitted photons.

Calculate the energy per mole of emitted photons.

Q4:

The atomic emission spectrum of nitrogen contains a strong line corresponding to photons with an energy of 1 . 6 5 6 × 1 0 1 8 J.

Calculate the wavelength of the emitted photons.

Calculate the energy per mole of emitted photons.

Q5:

Atomic emission spectra of the hydrogen atom show a red line at a wavelength of 656 nm. Given that the speed of light is 3 . 0 0 × 1 0 / 8 m s and Planck’s constant is 6 . 6 2 6 × 1 0 3 4 J s , what is the energy possessed by one photon at this wavelength?

  • A 3 . 0 3 0 × 1 0 1 9 J
  • B 3 . 3 0 0 × 1 0 1 8 J
  • C 4 . 5 7 3 × 1 0 1 4 J
  • D 1 . 0 1 0 × 1 0 2 7 J

Q6:

The atomic emission spectrum of the hydrogen atom shows a violet line at a wavelength of 434.0 nm. Calculate the energy of one photon at this wavelength. Use a value of 2 . 9 9 8 × 1 0 / 8 m s for the speed of light and 6 . 6 2 6 × 1 0 3 4 J s for Planck’s constant.

  • A 4 . 5 7 7 × 1 0 1 9 J
  • B 6 . 9 1 2 × 1 0 1 4 J
  • C 2 . 1 8 0 × 1 0 1 8 J
  • D 1 . 5 2 6 × 1 0 2 7 J

Q7:

How many infrared photons with a wavelength of 1 . 3 0 × 1 0 6 m must be absorbed by 190 g of water to increase the temperature from 25.0 to 3 5 . 0 C ? The specific heat capacity of water is 4.184 J/g⋅K.

  • A 86.4 mmol
  • B 77.7 mmol
  • C 82.4 mmol
  • D 83.0 mmol
  • E 90.9 mmol

Q8:

Heated thallium ions emit photons with an energy of 8 . 6 4 4 × 1 0 1 9 J.

Calculate the wavelength of the emitted photons.

Calculate the energy per mole of emitted photons.

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