The van der Waals constant '' for helium gas is experimentally determined to be . Knowing that '' is — States of Matter and Gaseous State Chemistry Question
Question
The van der Waals constant '$b$' for helium gas is experimentally determined to be $2.4 \times 10^{-2}\text{ L mol}^{-1}$. Knowing that '$b$' is theoretically $4$ times the actual total volume occupied by one mole of the gas atoms, calculate the actual volume of $1\text{ mole}$ of helium atoms in $\text{mL}$.
Answer: 6
💡 Solution & Explanation
By definition, the excluded volume $b = 4 \times V_{actual\_per\_mole}$. Therefore, $V_{actual\_per\_mole} = b / 4$. $V_{actual} = 2.4 \times 10^{-2}\text{ L} / 4 = 0.6 \times 10^{-2}\text{ L} = 6 \times 10^{-3}\text{ L}$. Converting to millilitres ($\text{mL}$): $6 \times 10^{-3}\text{ L} \times 1000\text{ mL/L} = 6\text{ mL}$.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes