(B) Using the ideal gas equation: $PV = nRT = \frac{m}{M} RT$ $\therefore m = \frac{PVM}{RT}$ Since both containers contain the same gas $(CO_2)$, the

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(B) Using the ideal gas equation: $PV = nRT = \frac{m}{M} RT$ $\therefore m = \frac{PVM}{RT}$ Since both containers contain the same gas $(CO_2)$, the molar mass $(M)$ is constant. Therefore, $\frac{m_A}{m_B} = \frac{P_A V_A}{P_B V_B} \times \frac{T_B}{T_A}$ Given: $P_A = 4P_B$, $V_A = 4V_B$, $T_A = 4T_B$, and $m_B = x \ g$. Substituting these values: $\frac{m_A}{x} = \frac{(4P_B)(4V_B)}{P_B V_B} \times \frac{T_B}{4T_B}$ $\frac{m_A}{x} = 16 \times \frac{1}{4} = 4$ $m_A = 4x \ g$

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

Medium

Two containers $A$ and $B$ contain $CO_2$ gas. Pressure, volume, and absolute temperature of the gas in $A$ are $4$ times more compared to that in $B$. If the mass of the gas in $B$ is $x \ g$, then the mass of the gas in $A$ will be:

TS EAMCET 2023 All TS EAMCET

A
$\frac{x}{2} \ g$
B
$4x \ g$
C
$2x \ g$
D
$16x \ g$

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

States of Matter

Subtopic

Ideal gas equation and Related gas laws

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At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

Medium

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The graph of $V$ versus $T$ for an ideal gas at constant pressures $P_1$ and $P_2$ is shown below. Which of the following is correct?

Easy

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If the volume of a gas is $V \ L$ at $P \ atm$ pressure and $27 \ ^oC$ temperature,what will be the volume of the gas at $-173 \ ^oC$ temperature and $P \ atm$ pressure if the amount of gas is doubled?

Difficult

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Keeping temperature constant,the pressure of $11.2 \ dm^3$ of a gas was increased from $105 \ kPa$ to $420 \ kPa$. What is the new volume of the gas (in $dm^3$)?

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What is the value of $R$ in the ideal gas equation $pV = nRT$ in units of $bar \ L \ mol^{-1} \ K^{-1}$? Calculate it.

Medium

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Two containers $A$ and $B$ contain $CO_2$ gas. Pressure, volume, and absolute temperature of the gas in $A$ are $4$ times more compared to that in $B$. If the mass of the gas in $B$ is $x \ g$, then the mass of the gas in $A$ will be:

Similar Questions

At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

The graph of $V$ versus $T$ for an ideal gas at constant pressures $P_1$ and $P_2$ is shown below. Which of the following is correct?

If the volume of a gas is $V \ L$ at $P \ atm$ pressure and $27 \ ^oC$ temperature,what will be the volume of the gas at $-173 \ ^oC$ temperature and $P \ atm$ pressure if the amount of gas is doubled?

Keeping temperature constant,the pressure of $11.2 \ dm^3$ of a gas was increased from $105 \ kPa$ to $420 \ kPa$. What is the new volume of the gas (in $dm^3$)?

What is the value of $R$ in the ideal gas equation $pV = nRT$ in units of $bar \ L \ mol^{-1} \ K^{-1}$? Calculate it.

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