3.4 moles of an ideal gas occupies volume of 68 mL at 300 K . What would be the pressure of gas?…

3.4 moles of an ideal gas occupies volume of 68 mL at 300 K . What would be the pressure of gas? $\left(\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$
  1. $1.247 \times 10^2 \mathrm{kPa}$
  2. $2.431 \times 10^3 \mathrm{kPa}$
  3. $1.031 \times 10^5 \mathrm{kPa}$
  4. $3.247 \times 10^5 \mathrm{kPa}$

Solution

$\begin{aligned} & \mathrm{n}=3.4 \mathrm{~mol}, \mathrm{~T}=300 \mathrm{~K} \\ & \mathrm{~V}=68 \mathrm{~mL}=0.068 \mathrm{~L}, \mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1} \end{aligned}$
According to ideal gas equation, $\mathrm{PV}=\mathrm{nRT}$ $\begin{aligned} \therefore \quad \mathrm{P}=\frac{\mathrm{nRT}}{\mathrm{~V}} & =\frac{3.4 \mathrm{~mol} \times 8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \times 300 \mathrm{~K}}{0.068 \mathrm{dm}^3} \\ & =124710 \mathrm{kPa} \end{aligned}$

Asked in: MHT CET 2024 (15 May Shift 2)

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