Question

Calculate uncertainty in velocity, an electron has 0.1nm uncertainty in position​

Answer 1

Answer:

Explanation:

We apply Hiesenberg's uncertainty principle here.

∆x*∆p≥{h/4π}

where ∆x is uncertainty in position, ∆p is uncertainty in momentum.

∆p=m∆v,where ∆v is uncertainty in velocity.

So,∆v=h/(4πm*∆x), where h is Planck's constant and m is mass of electron.

Substituting values and changing to appropriate units,we get:-

Uncertainty in velocity (∆v)=5.8*10^5 m/s

Answer 2

Answer:

We apply Hiesenberg's uncertainty principle here.

∆x*∆p≥{h/4π}

where ∆x is uncertainty in position, ∆p is uncertainty in momentum.

∆p=m∆v,where ∆v is uncertainty in velocity.

So,∆v=h/(4πm*∆x), where h is Planck's constant and m is mass of electron.

Substituting values and changing to appropriate units,we get:-

Uncertainty in velocity (∆v)=5.8*10^5 m/s