Specifically, consider simultaneously measuring the position and momentum of an electron (it could be any particle). There is an uncertainty in position Δx that is approximately equal to the wavelength of the particle. That is, Δx ≈ λ. As discussed above, a wave is not located at one point in space.
How do you calculate the uncertainty in the position of an electron?, Therefore, the uncertainty in position (Δx) can be calculated as follows: (bigtriangleup x=frac{h}{4pi mbigtriangleup u}) (bigtriangleup x=frac{6.626times 10^{-34}times times 100}{4times 3.14times 9.1times 10^{-31}times 0.001times 300}) = 1.93 x 10–2m.
Furthermore, What is the uncertainty of an electron?, If you actually use the limiting case allowed by the uncertainty principle, Δp = hbar/2Δx, the confinement energy you get for the electron in the atom is only 0.06 eV.
Finally, What is the uncertainty in the position of electron of mass?, The uncertainty in the position of an electron (mass=9.1×10-28g) moving with a velocity of 3.0×104cms-1 accurate up to 0.001% will be. (Use h4π in the uncertainty expression, where h=6.626×10-27erg-s) Step by step solution by experts to help you in doubt clearance & scoring excellent marks in exams. Δx=1.92cm.
Frequently Asked Question:
What is the minimum uncertainty in the position of an electron moving at a speed of 4/10 6 M?
Question: What Is The Minimum Uncertainty In The Position Of An Electron Moving At A Speed Of 4 X 10^6 M / S Plus Or Minus One Percent The Mass Of The Electron Is 9.11 X 10^-31 Kg Planck’s Constant: 6.63 X 10^-34 Textbook Answer Is 1 X 10^-9 M.
What is the minimum uncertainty in the position of the electron?
Since atoms are roughly 0.1 nm in size, knowing the position of an electron to 0.0100 nm localizes it reasonably well inside the atom.
What is the minimum error in position of an electron moving with a speed?
Explanation: Since, we know from the question that the velocity of the electron is =600m/s. Also, the accuracy given is = 0.005%. So, the uncertainty in the velocity will be given as = 600 x 5 /1000.
What is the uncertainty in the position of an electron moving at with an uncertainty of?
The uncertainty in position of an electron (m = 9.1 × 10^-28gm) moving with a velocity 3 × 10^4 cm/s accurate upto 0.001.
How do you calculate the uncertainty in the position of an electron?
Therefore, the uncertainty in position (Δx) can be calculated as follows: (bigtriangleup x=frac{h}{4pi mbigtriangleup u}) (bigtriangleup x=frac{6.626times 10^{-34}times times 100}{4times 3.14times 9.1times 10^{-31}times 0.001times 300}) = 1.93 x 10–2m.
How do you find the uncertainty of an electron position?
Therefore, the uncertainty in position (Δx) can be calculated as follows: (bigtriangleup x=frac{h}{4pi mbigtriangleup u}) (bigtriangleup x=frac{6.626times 10^{-34}times times 100}{4times 3.14times 9.1times 10^{-31}times 0.001times 300}) = 1.93 x 10–2m.
What is the uncertainty of an electron?
If you actually use the limiting case allowed by the uncertainty principle, Δp = hbar/2Δx, the confinement energy you get for the electron in the atom is only 0.06 eV.
What is the uncertainty in the position of an electron moving at with an uncertainty of?
The uncertainty in position of an electron (m = 9.1 × 10^-28gm) moving with a velocity 3 × 10^4 cm/s accurate upto 0.001.
What is the minimum uncertainty in the position of an electron moving at a speed of 4/10 6 M?
Question: What Is The Minimum Uncertainty In The Position Of An Electron Moving At A Speed Of 4 X 10^6 M / S Plus Or Minus One Percent The Mass Of The Electron Is 9.11 X 10^-31 Kg Planck’s Constant: 6.63 X 10^-34 Textbook Answer Is 1 X 10^-9 M.
How do you calculate the uncertainty of an electron?
Therefore, the uncertainty in position (Δx) can be calculated as follows: (bigtriangleup x=frac{h}{4pi mbigtriangleup u}) (bigtriangleup x=frac{6.626times 10^{-34}times times 100}{4times 3.14times 9.1times 10^{-31}times 0.001times 300}) = 1.93 x 10–2m.
What is uncertain about the atom?
relativity. In the Rutherford’s model, the atom should collapse into the nucleus, because the electrons should radiate away their energy and spiral inward. … It is the uncertainty principle that explains why we can’t have any lower states, and why the negative electrons cannot exist within or on the positive nucleus.
What is the theory of uncertainty?
Introduced first in 1927 by the German physicist Werner Heisenberg, the uncertainty principle states that the more precisely the position of some particle is determined, the less precisely its momentum can be predicted from initial conditions, and vice versa.
What do you mean by Heisenberg’s uncertainty principle?
Heisenberg’s uncertainty principle is a key principle in quantum mechanics. Very roughly, it states that if we know everything about where a particle is located (the uncertainty of position is small), we know nothing about its momentum (the uncertainty of momentum is large), and vice versa.
How do you find the uncertainty of a position?
The uncertainty in position is the accuracy of the measurement, or Δx = 0.0100 nm. Thus the smallest uncertainty in momentum Δp can be calculated using ΔxΔp≥h4π Δ x Δ p ≥ h 4 π . Once the uncertainty in momentum Δp is found, the uncertainty in velocity can be found from Δp = mΔv.
What is the uncertainty of an electron?
If you actually use the limiting case allowed by the uncertainty principle, Δp = hbar/2Δx, the confinement energy you get for the electron in the atom is only 0.06 eV.
What is the formula for calculating uncertainty?
To summarize the instructions above, simply square the value of each uncertainty source. Next, add them all together to calculate the sum (i.e. the sum of squares). Then, calculate the square-root of the summed value (i.e. the root sum of squares). The result will be your combined standard uncertainty.
What is the uncertainty in the position of an electron moving at with an uncertainty of?
The uncertainty in position of an electron (m = 9.1 × 10^-28gm) moving with a velocity 3 × 10^4 cm/s accurate upto 0.001.