According to the Heisenberg uncertainty principle, if the uncertainty in the speed of an electron is 3.5 *10³ m/s, the uncertainty in its position (in m) is at least: A) 1.7 * 10¯⁸ m B) 6.6 * 10¯⁸ m C) 17 m D) 66 m E) None of these choices is correct.

Question

Quizplus · Accepted Answer

The Heisenberg uncertainty principle states that Δx * Δp ≥ ħ/2, where Δx is the uncertainty in position, Δp is the uncertainty in momentum, and ħ is the reduced Planck's constant (approximately 1.0545718 × 10^-34 Js). Given the uncertainty in speed (Δv) is 3.5 * 10^3 m/s, and using the electron's mass (approximately 9.10938356 × 10^-31 kg), we can calculate Δp = m * Δv. Solving for Δx gives approximately 1.7 * 10^-8 m.

According to the Heisenberg Uncertainty Principle, If the Uncertainty in the Speed