Question

A photon of light produced by a surgical laser has an energy of 3.027 × 10^−19 J. Calculate the frequency and wavelength of the photon. What is the total energy in 1 mole of photons? What is the color of the emitted light?

a) Frequency: 4.97 × 10^14 Hz; Wavelength: 6.03 × 10^−7 m; Total energy in 1 mole: 181.5 kJ; Color: Yellow
b) Frequency: 6.03 × 10^14 Hz; Wavelength: 4.97 × 10^−7 m; Total energy in 1 mole: 181.5 kJ; Color: Yellow
c) Frequency: 4.97 × 10^14 Hz; Wavelength: 6.03 × 10^−7 m; Total energy in 1 mole: 126.9 kJ; Color: Green
d) Frequency: 6.03 × 10^14 Hz; Wavelength: 4.97 × 10^−7 m; Total energy in 1 mole: 126.9 kJ; Color: Green

Answer 1

The frequency of the photon is approximately 4.97 × 10¹⁴ Hz and the wavelength is approximately 6.03 × 10⁻⁷ m. The total energy in 1 mole of photons is approximately 181.5 kJ. The emitted light is yellow.

Step-by-step explanation:

The frequency of a photon can be calculated using the formula:

f = E / h

Where f is the frequency, E is the energy of the photon, and h is Planck's constant (6.626 × 10⁻³⁴ J·s).

The wavelength of a photon can be calculated using the formula:

λ = c / f

Where λ is the wavelength, c is the speed of light (3 × 10⁸ m/s), and f is the frequency.

The total energy in 1 mole of photons can be calculated by multiplying the energy of one photon by Avogadro's number (6.022 × 10²³).

Based on the given energy of the photon (3.027 × 10⁻¹⁹ J), the frequency of the photon is approximately 4.97 × 10¹⁴ Hz and the wavelength is approximately 6.03 × 10⁻⁷ m.

The total energy in 1 mole of photons is approximately 181.5 kJ.

The color of the emitted light is yellow.