If uncertainty in the position of an electron is zero the uncertainty in its momentum will be: 

1. <h/4$\mathrm{\pi }$

2. >h/4$\mathrm{\pi }$

3. zero

4. infinite

Which one is the wrong statement?

The measurement of the electron position is associated with an uncertainty in momentum which is equal to 1x10^-18 g cm s^-1. The uncertainty in velocity of the electron will be:

(mass of an electron is 9 x 10^-28 g)

1. 1 x 10⁹ cm s^-1                     

2. 1 x 10⁶ cm s^-1

3. 1 x 10⁵ cm s^-1                     

4. 1 x 10¹¹ cm s^-1

Given the following data:

In light of the data given above, the uncertainty involved in the measurement of velocity within a distance of 0.1 $\stackrel{°}{\mathrm{A}}$ will be:
1. 5.79 x 10⁶ ms^-1       
2. 5.79 x 10⁷ ms^-1
3. 5.79 x 10⁸ ms^-1         
4. 5.79 x 10⁵ ms^-1

For a subatomic particle, the uncertainty in position is same as that of uncertainty in its momentum. The
least uncertainty in its velocity can be given as-

1. $∆\mathrm{V} = \frac{\mathrm{h}}{4{\mathrm{\pi m}}^2}$

2. $∆\mathrm{V} = \frac{1}{2\mathrm{\pi }}\sqrt{\frac{\mathrm{h}}{\mathrm{m}}}$

3. $∆\mathrm{V} = \frac{\mathrm{h}}{2\mathrm{\pi m}}$

4. $∆\mathrm{V} = \frac{1}{2\mathrm{m}}\sqrt{\frac{\mathrm{h}}{\mathrm{\pi }}}$

Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle? 

1. $∆x.∆p\ge \frac{h}{4\mathrm{\pi }}$

2. $∆x.∆v\ge \frac{h}{4\mathrm{\pi m}}$

3. $∆E.∆t\ge \frac{h}{4\mathrm{\pi }}$

4. $∆E.∆x\ge \frac{h}{4\mathrm{\pi }}$

Uncertainty in position of a $e^{-}$ and He is similar. If uncertainty in momentum of $e^{-}$ is $\mathrm{32 }\times {10}^5$, then uncertainty in momentum of He will be:

If the position of the electron were measured with an accuracy of +0.002 nm, the uncertainty in the momentum of the electron would be: 

1. 5.637 × 10^–23 kg m s^–1

2. 4.637 × 10^–23 kg m s^–1

3. 2.637 × 10^–23 kg m s^–1

4. 3.637 × 10^–23 kg m s^–1