Heisenberg's uncertainty principle states that there is a fundamental limit to the precision with which certain pairs of physical properties of a particle, such as position and momentum, can be simultaneously known. This principle applies to subatomic particles and has implications for the measurement and determination of their properties.
When it comes to measuring the position of a subatomic particle, the more precisely you measure its position, the less precisely you can know its momentum (and vice versa). This means that the more precisely you determine the position of a particle, the more uncertain its momentum becomes, making it difficult to determine its average velocity accurately. In other words, the more precisely you measure the position of a particle, the less meaningful the concept of average velocity becomes due to the inherent uncertainty in momentum.
Similarly, if you were to measure the position of a subatomic particle multiple times, the uncertainty in its momentum would increase with each measurement. This would make it challenging to accurately determine its acceleration since acceleration is related to changes in momentum over time.
Heisenberg's uncertainty principle fundamentally limits the simultaneous measurement and precise determination of certain pairs of properties, such as position and momentum or position and velocity. Therefore, attempting to determine average velocity or acceleration with high precision for a subatomic particle becomes problematic due to the inherent uncertainty associated with such measurements.