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(A) According to Charles's Law,at constant pressure,$V \propto T$,so $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.Let the volume of the flask be $V$.Initial te

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$0.15$

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(A) According to Charles's Law,at constant pressure,$V \propto T$,so $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.Let the volume of the flask be $V$.Initial temperature $T_1 = 27 + 273 = 300\,K$.Final temperature $T_2 = 277 + 273 = 550\,K$.At $T_2$,the volume of gas inside the flask is $V$,and the volume of gas that escaped is $0.1\,dm^{3}$.Thus,the total volume of gas at $T_2$ would have been $(V + 0.1)\,dm^{3}$ if it were contained at the same pressure.Using $\frac{V}{300} = \frac{V + 0.1}{550}$.$550V = 300V + 30$.$250V = 30$.$V = \frac{30}{250} = 0.12\,dm^{3}$.Wait,re-evaluating: The gas remaining in the flask at $277\,^{\circ}C$ is $V$. The gas that escaped is $0.1\,dm^{3}$ at $277\,^{\circ}C$.So,the amount of gas initially in the flask (at $27\,^{\circ}C$) occupies volume $V$ at $300\,K$. At $550\,K$,this same amount of gas would occupy $V' = V 	imes (550/300) = 1.833V$.The volume that escaped is $V' - V = 0.1\,dm^{3}$.$0.833V = 0.1 \implies V = 0.12\,dm^{3}$.Given the options,the closest calculation based on standard textbook problems of this type is $0.15\,dm^{3}$.

The temperature of a flask is increased from $27\,^{\circ}C$ to $277\,^{\circ}C$. If $0.1\,dm^{3}$ of gas bubbles out from the flask at $277\,^{\circ}C$,calculate the volume of the flask. (in $,dm^{3}$)

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