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Q2.22(e):
Just as precise measurements are necessary in science, it is equally important to be able to make rough estimates of quantities using rudimentary ideas and common observations. Think of ways by which you can estimate the following (where an estimate is difficult to obtain, try to get an upper bound on the quantity) : (e) the number of air molecules in your classroom.

Solution :

Step 1: Establishing Physical Parameters and Assumptions

To estimate the number of air molecules in a classroom, we must define the macroscopic volume of the space and apply the Ideal Gas Law. We assume standard ambient conditions at Room Temperature ($T \approx 300 \, K$) and Atmospheric Pressure ($P \approx 1.013 \times 10^5 \, Pa$).

Let the classroom dimensions be:

  • Length ($l$) = $10 \, m$
  • Width ($w$) = $8 \, m$
  • Height ($h$) = $3 \, m$

Total Volume ($V$) = $l \times w \times h = 10 \times 8 \times 3 = 240 \, m^3$.

Step 2: Theoretical Foundation

We utilize the Ideal Gas Equation: $PV = nRT$, where:

  • $P$: Pressure in Pascals ($Pa$)
  • $V$: Volume in cubic meters ($m^3$)
  • $n$: Number of moles
  • $R$: Universal Gas Constant ($8.314 \, J \cdot mol^{-1} \cdot K^{-1}$)
  • $T$: Temperature in Kelvin ($K$)

[By the Ideal Gas Law derivation, $n = \frac{PV}{RT}$]

Step 3: Calculating Molar Quantity

Substitute the assumed values into the equation:

$n = \frac{(1.013 \times 10^5 \, Pa) \times (240 \, m^3)}{(8.314 \, J \cdot mol^{-1} \cdot K^{-1}) \times (300 \, K)}$

$n = \frac{2.4312 \times 10^7}{2494.2} \approx 9747.4 \, \text{moles}$

Step 4: Determining Total Molecular Count

To find the total number of molecules ($N$), we multiply the number of moles ($n$) by Avogadro’s Constant ($N_A \approx 6.022 \times 10^{23} \, \text{molecules/mol}$):

$N = n \times N_A$ [Per Avogadro's hypothesis regarding molecular count per mole]

$N = 9747.4 \times 6.022 \times 10^{23}$

$N \approx 5.87 \times 10^{27} \, \text{molecules}$

Step 5: Visual Representation of Room Volume

Room Volume (V) = 240 m³ h = 3m

Analytical Summary

Variable Value
Classroom Volume ($V$) $240 \, m^3$
Pressure ($P$) $1.013 \times 10^5 \, Pa$
Temperature ($T$) $300 \, K$
Total Molecules ($N$) $\approx 5.9 \times 10^{27}$

Final Solution: The estimated number of air molecules in a classroom of volume $240 \, m^3$ is approximately $6 \times 10^{27}$ molecules.


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