(A) Using the combined gas law,$\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$,we can express the ratio of volumes as $\frac{V_2}{V_1} = \frac{P_1 T_2}{P_

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Volume will become greater by a factor of $1.6$.

(A) Using the combined gas law,$\frac{P_1 V_1}{T_1} = \frac{P_2 V_2}{T_2}$,we can express the ratio of volumes as $\frac{V_2}{V_1} = \frac{P_1 T_2}{P_2 T_1}$.Given initial conditions: $T_1 = 15 + 273 = 288 \ K$ and $P_1 = 1.5 \ bar$.Given final conditions: $T_2 = 25 + 273 = 298 \ K$ and $P_2 = 1.0 \ bar$.Substituting the values: $\frac{V_2}{V_1} = \frac{1.5 \times 298}{1.0 \times 288} = \frac{447}{288} \approx 1.552$.Rounding to one decimal place,the volume increases by a factor of $1.6$.

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

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$A$ bubble of air is underwater at temperature $15^\circ C$ and the pressure $1.5 \ bar$. If the bubble rises to the surface where the temperature is $25^\circ C$ and the pressure is $1.0 \ bar$,what will happen to the volume of the bubble?

AIPMT 2011 All AIPMT

A
Volume will become greater by a factor of $1.6$.
B
Volume will become greater by a factor of $1.1$.
C
Volume will become smaller by a factor of $0.70$.
D
Volume will become greater by a factor of $2.5$.

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Ideal gas equation and Related gas laws

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At $0\, ^\circ C$ and $1\, atm$ pressure,a gas occupies $100\, cc$. If the pressure is increased to $1.5$-times and temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be .............. $cc$.

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$A$ bubble of air is underwater at temperature $15^\circ C$ and the pressure $1.5 \ bar$. If the bubble rises to the surface where the temperature is $25^\circ C$ and the pressure is $1.0 \ bar$,what will happen to the volume of the bubble?

Similar Questions

At $0\, ^\circ C$ and $1\, atm$ pressure,a gas occupies $100\, cc$. If the pressure is increased to $1.5$-times and temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be .............. $cc$.

The density of oxygen gas at $1.0 \, atm$ pressure and $27 \, ^oC$ temperature is ............. $g/L$.

For $1 \ mol$ of an ideal gas at a constant temperature $T,$ the plot of $(\log \ P)$ against $(\log \ V)$ is a ($P :$ Pressure,$V:$ Volume)

Densities of a gas at different conditions are in the ratio $1:2$ and their temperatures are in the ratio $2:1$,then the ratio of their respective pressure is :-

The densities of two gases are in the ratio $1:2$ and their temperatures are in the ratio $2:1$. What is the ratio of their corresponding pressures?

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