Verified Solution • 2025–26 Session moderate

QPages 34-37: Q1: HC Verma: Concepts of Physics - Volume 2 Kinetic Theory of Gases Pages 34-37: Q1 Solution: Calculate the volume of 1 mole of an ideal gas at STP.

⚠️ Common Exam Traps & Conceptual Pitfalls

Students frequently substitute the pressure in atmospheres ($1$ atm) directly into the ideal gas equation while using the SI value for the gas constant ($R = 8.314$ J/mol·K), leading to a result off by a factor of $10^5$. Always convert pressure to Pascals ($1.013 \times 10^5$ Pa) when using SI units for $R$.

Calculate the volume of 1 mole of an ideal gas at STP.

Step-by-Step Verified Solution

**Answer:**

V = 22.4 \times 10^{-3} \text{ m}^3 = 22.4 \text{ L}

**Step-by-Step Explanation:** At STP,

T = 273

K,

P = 1

atm

= 1.013 \times 10^5

Pa. For

n = 1

mole:

V = \frac{nRT}{P} = \frac{1 \times 8.314 \times 273}{1.013 \times 10^5} = 22.4 \times 10^{-3} \text{ m}^3 = 22.4 \text{ L}

All Questions in this Chapter

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