(C) According to Charles's Law,at constant pressure,$V \propto T$,so $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.Given: $V_1 = 300 \; cm^{3}$,$T_1 = 27 + 273

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(C) According to Charles's Law,at constant pressure,$V \propto T$,so $\frac{V_1}{T_1} = \frac{V_2}{T_2}$.Given: $V_1 = 300 \; cm^{3}$,$T_1 = 27 + 273 = 300 \; K$,$T_2 = 37 + 273 = 310 \; K$.Calculating $V_2$: $V_2 = V_1 \times \frac{T_2}{T_1} = 300 \; cm^{3} \times \frac{310 \; K}{300 \; K} = 310 \; cm^{3}$.The volume of air expelled is $\Delta V = V_2 - V_1 = 310 \; cm^{3} - 300 \; cm^{3} = 10 \; cm^{3}$.

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

Medium

Volume of the air that will be expelled from a vessel of $300 \; cm^{3}$ when it is heated from $27 \; ^{\circ}C$ to $37 \; ^{\circ}C$ at the same pressure will be ........... $cm^{3}$

A
$310$
B
$290$
C
$10$
D
$37$

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Ideal gas equation and Related gas laws

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Volume of the air that will be expelled from a vessel of $300 \; cm^{3}$ when it is heated from $27 \; ^{\circ}C$ to $37 \; ^{\circ}C$ at the same pressure will be ........... $cm^{3}$

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What is the density of $CO_2$ at $100\,^oC$ and $800\,mm\,Hg$ pressure in $g/L$?

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The pressure exerted by $6.0 \ g$ of methane gas in a $0.03 \ m^3$ vessel at $129 \ ^oC$ is : (Atomic masses of $C = 12.01, H = 1.01$ and $R = 8.314 \ J K^{-1} mol^{-1}$) :- ................ $Pa$

If $4 \ g$ of $O_2$ and $2 \ g$ of $H_2$ are filled in a $1 \ L$ bulb at $0 \ ^oC$,the total pressure of the mixture will be...... (in $atm$)

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