estimate number of impacts number of imapcts air molecule make with palm of your hand assuming all air is nitrogen molar mass =.0028
How to get velocity=functionof temperature
What are the answer of this equation
Well, I have to admit, it's quite difficult to count the number of impacts air molecules make with the palm of your hand. It's like trying to count the number of ants at a picnic - they're just too tiny and numerous!
But fret not, I am here to give you an estimate! Let's approach this question with a touch of humor:
Since there are roughly 2.5 x 10^19 molecules in a single cubic centimeter of air, and assuming your palm covers an area of about 100 square centimeters, we can use some clown math to estimate the impacts.
Now, if we consider that the average molecule in the air moves at a speed of around 500 meters per second, and let's say your hand is in contact with the air for about 1 second, then by dividing the area of your hand by the volume of a single molecule, we get...
Ah, who am I kidding? The number is simply too astronomical for my clown brain to comprehend! Let's just say you'll have a plethora of air molecules bouncing off your hand, enough to make a clown's head spin!
So, while I may not have a specific number for you, rest assured that there are a whole lot of impacts happening between your hand and those jovial nitrogen molecules. Enjoy your atmospheric high-fives!
To estimate the number of impacts air molecules make with the palm of your hand, we can make some reasonable assumptions and calculations.
First, let's consider the volume of air that the palm of your hand comes into contact with. On average, the surface area of an adult's palm is about 90 square centimeters (cm²). Assuming a typical distance from the surface of your hand to the first layer of air molecules of around 0.1 centimeters (cm), we can estimate the volume of air in contact with your hand.
Volume = Surface Area * Distance = 90 cm² * 0.1 cm = 9 cm³
Next, let's calculate the number of air molecules in this volume using the ideal gas law. The ideal gas law equation is PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the ideal gas constant, and T is temperature. Since we are assuming a constant pressure and temperature, we can simplify the equation to n = PV / RT.
Assuming a standard temperature of 25 degrees Celsius (or 298 Kelvin) and a pressure of 1 atmosphere (or 101.325 kilopascals), we can plug in the values to calculate the number of moles of air molecules.
R = 0.0821 L·atm/(mol·K) (ideal gas constant)
n = (1 atm * 9 cm³) / (0.0821 L·atm/(mol·K) * 298 K) = 0.037 moles
Now, we can use Avogadro's number, which states that there are approximately 6.022 × 10^23 molecules in one mole, to calculate the number of air molecules.
Number of molecules = n * Avogadro's number
Number of molecules = 0.037 moles * (6.022 × 10^23 molecules/mole) ≈ 2.221 × 10^22 molecules
Therefore, we estimate that approximately 2.221 × 10^22 air molecules would make impacts with the palm of your hand.
A0932944201B
pressure*areaofHand=force=Numberhits*mass*velocity change
numberhits=air pressure*areaofhand/massN2*velocitychagne
but the change of velocity=2*Velocity (assumeing rebounds).
and velocity=function of temperature
so is this enough for you ? watch your units here.