Question

Heisenberg's uncertainty principle makes it impossible to simultaneously determine with perfect accuracy

• A. The position and color of a particle
• B. The momentum and velocity of a particle
• C. The position and momentum of a particle
• D. The energy and mass of a particle

Hint:

Always associate Heisenberg’s uncertainty with position and momentum – the more precisely one is known, the less precisely the other can be known.

Answer 1

The Correct Option is C

Heisenberg's uncertainty principle is a fundamental concept in quantum mechanics. It states that it is impossible to know both the exact position and the exact momentum (which is mass times velocity) of a particle at the same time.
Mathematically, this is expressed as: \[ \Delta x \cdot \Delta p \geq \frac{h}{4\pi} \] where \( \Delta x \) is the uncertainty in position, \( \Delta p \) is the uncertainty in momentum, and \( h \) is Planck’s constant.
This principle is not a limitation of measurement instruments but an inherent property of quantum systems. If you try to measure a particle's position very accurately, its momentum becomes more uncertain, and vice versa.
Why the other options are incorrect:

• (A) Color is not a fundamental quantum property used in Heisenberg’s principle.
• (B) Momentum includes velocity, so this option is not logically coherent.
• (D) Energy and mass are related by \(E=mc^2\), and both can be precisely known.