Home
Class 11
CHEMISTRY
A measurment establishes position of a p...

A measurment establishes position of a proton with an accuracy of` pm ``10^(-10)m`. Find the mininum uncretainty in proton 's position 1 second later .

Text Solution

AI Generated Solution

To solve the problem, we will use the Heisenberg Uncertainty Principle, which states that the uncertainty in position (Δx) and the uncertainty in momentum (Δp) are related by the equation: \[ \Delta x \cdot \Delta p \geq \frac{h}{4\pi} \] Where: - \( \Delta x \) = uncertainty in position ...
Promotional Banner

Topper's Solved these Questions

  • ATOMIC STRUCTURE

    BANSAL|Exercise Exercise.1|48 Videos
  • ATOMIC STRUCTURE

    BANSAL|Exercise Exercise.2|21 Videos
  • ATOMIC STRUCTURE

    BANSAL|Exercise Solved Examples|17 Videos
  • GENERAL ORGANIC CHEMISTRY

    BANSAL|Exercise Exercise 3|9 Videos

Similar Questions

Explore conceptually related problems

If the uncertainity in the position of proton is 6xx10^(8)m , then the minimum uncertainity in its speed is

A proton (m_(p) = 1.673 xx 10^(-27) kg) and an electron (m = 9.109 xx 10^(-31) kg) are confined such that the position x of each is known within 1.50 xx 10^(-10) m . What is the ratio of the minimum uncertainty in the x component of the velocity of the electron to that of the proton, Deltav_(e)// Deltav_(p) ?

In an atom , an electron is moving with a speed of 600 m/s with an accuracy of 0.05% . The certainty with which the position of the electron can be located is (h = 6.6 xx 10^(-34) kgm^(2)s^(-1) , mass of electron , e_(m) = 9.1 xx 10^(-31) kg ):

The speed fo this dust particle ("mass" =n 10^(-3) g) is measured with the uncertainty of (3.313)/(pi) xx10^(-3) m//s. The minimum uncertainty in position of the dust particle ("in order of"10^(-26) m) is :

A ball has a mass of "10g" and speed of "20m/s" . If the speed can be measured with the accuracy of 1%, then the uncertainty in its position is

An e^- moving with a velocity of 2xx10^6m//s . If the speed can be measured with an accuracy of 0.02%. Calculaate the uncertainty in its position is 1.45xx10^(-x) . The value of x: