If the energy of a photon is 1.32 × 10^-18 J, what is its wavelength in nm (c = 3.00 × 10⁸m/s; h = 6.63 × 10^-34 J • s)? A) 1.51 × 10^-7 nm B) 151 nm C) 1.99 × 10¹⁵ nm D) 1.99 × 10²⁴ nm E) None of these choices is correct.

Question

Quizplus · Accepted Answer

The wavelength of a photon can be calculated using the formula λ = hc/E, where λ is the wavelength, h is Planck's constant (6.63 × 10^-34 J•s), c is the speed of light (3.00 × 10^8 m/s), and E is the energy of the photon (1.32 × 10^-18 J). Substituting the given values, λ = (6.63 × 10^-34 J•s * 3.00 × 10^8 m/s) / (1.32 × 10^-18 J) = 1.51 × 10^-7 m. Converting meters to nanometers (1 m = 10^9 nm), λ = 1.51 × 10^-7 m * 10^9 nm/m = 151 nm.

If the Energy of a Photon Is 1