A large flask contains air at 27 , ^{circ}C. | vedclass

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(B) For a gas in a flask, the pressure $P$ and volume $V$ remain constant as air is expelled.According to the ideal gas equation, $PV = \mu RT$, where

Vedclass · Accepted Answer

$327$

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(B) For a gas in a flask, the pressure $P$ and volume $V$ remain constant as air is expelled.According to the ideal gas equation, $PV = \mu RT$, where $\mu$ is the number of moles (proportional to mass) and $T$ is the absolute temperature in Kelvin.Since $P$ and $V$ are constant, we have $\mu T = 	ext{constant}$.Let the initial mass be $m$ (moles $\mu_1 = \mu$) at temperature $T_1 = 27 + 273 = 300 \, K$.After heating, half the mass is expelled, so the remaining mass is $m/2$ (moles $\mu_2 = \mu/2$) at temperature $T_2$.Using the relation $\mu_1 T_1 = \mu_2 T_2$:$\mu 	imes 300 = (\mu/2) 	imes T_2$$300 = T_2 / 2$$T_2 = 600 \, K$.Converting to Celsius: $T_2 = 600 - 273 = 327 \, ^{\circ}C$.

$A$ large flask contains air at $27 \, ^{\circ}C$. In order to expel half the mass of air from the flask, the flask should be heated up to what temperature in $^{\circ}C$?

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