An electron has a speed `3xx 10 ^(2) ms^(-1)` with uncertainty `0.07 %` what is the uncertainty in locating its position ?

Explanation

To solve the problem of determining the uncertainty in locating the position of an electron given its speed and uncertainty in speed, we will use the Heisenberg Uncertainty Principle. Here’s a step-by-step solution:

### Step 1: Understand the Heisenberg Uncertainty Principle
The Heisenberg Uncertainty Principle states that the uncertainty in position (Δx) and the uncertainty in momentum (Δp) cannot both be precisely determined at the same time. The mathematical expression is:
\[ \Delta x \cdot m \cdot \Delta v \geq \frac{h}{4\pi} \]
where:
- Δx = uncertainty in position
- m = mass of the particle
...