An open-mouthed container is filled with air | vedclass

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(D) For an open container,the pressure $P$ and volume $V$ remain constant.Using the ideal gas law $PV = nRT$,where $n$ is the number of moles,we have

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$171$

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(D) For an open container,the pressure $P$ and volume $V$ remain constant.Using the ideal gas law $PV = nRT$,where $n$ is the number of moles,we have $n \propto 1/T$.Therefore,$n_1 T_1 = n_2 T_2$.Initial temperature $T_1 = 60 + 273 = 333 \ K$.Let the initial number of moles be $n_1 = n$.Since $1/4$ of the air escapes,the remaining moles $n_2 = n - (1/4)n = (3/4)n$.Substituting the values: $n 	imes 333 = (3/4)n 	imes T_2$.$T_2 = 333 	imes (4/3) = 444 \ K$.Converting back to Celsius: $T = 444 - 273 = 171^{\circ}C$.

An open-mouthed container is filled with air at $60^{\circ}C$. The container is heated to a temperature $T$ such that $1/4$ of the air escapes. The value of $T$ is ........ $^{\circ}C$.

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