MHTCET 14 May 2023 Shift 1 Solved Paper

To find the temperature of an ideal gas, we can use the ideal gas equation:$P V = n R T$where:$P$ is the pressure in atmospheres,$V$ is the volume in liters $(\mathrm{dm}^3)$,$n$ is the number of moles,$R$ is the gas constant $(0.0821\ \mathrm{dm}^3\ \mathrm{atm}\ \mathrm{K}^{-1}\ \mathrm{mol}^{-1})$, and $T$ is the temperature in Kelvin.Given: We can rearrange the ideal gas equation to solve for $T$ :$T = \frac{P V}{n R}$Plugging in the given values: $T = \frac{(4.926\ \mathrm{atm})(20\ \mathrm{dm}^3)}{(2\ \mathrm{mol})(0.0821\ \mathrm{dm}^3\ \mathrm{atm}\ \mathrm{K}^{-1}\ \mathrm{mol}^{-1})}$$T = \frac{98.52\ \mathrm{atm} \cdot \mathrm{dm}^3}{0.1642\ \mathrm{dm}^3\ \mathrm{atm}\ \mathrm{mol}^{-1}}$$T = 600\ \mathrm{K}$To convert the temperature from Kelvin to Celsius, use the conversion formula:$\text{Celsius} = \text{Kelvin} - 273.15$For our calculation:$\text{Celsius} = 600\ \mathrm{K} - 273.15$$\text{Celsius} = 326.85 \approx 327^{\circ}\ \mathrm{C}$Therefore, the temperature of the gas in degree Celsius is closest to Option B: 327 .