(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

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States of Matter

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Ideal gas equation and Related gas laws

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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

An ideal gas expands against a constant external pressure of $3 \ atm$ from $4 \ dm^3$ to $6 \ dm^3$. The work done during this process is ..... $J$.

The value of the universal gas constant $R$ is the same for all gases. What is its physical significance?

Calculate the new pressure of a gas enclosed in a cylinder when it is compressed from $5 \text{ L}$ to $2 \text{ L}$ at an initial pressure of $1 \text{ atm}$ and temperature of $300 \text{ K}$. The final temperature in this process is $500 \text{ K}$. (in $\text{ atm}$)

At a given temperature,the density of gas $x$ is twice that of gas $y$. The molar mass of $x$ is one-third of the molar mass of $y$. What is the ratio of their pressures $(P_x / P_y)$?

$100 \, mL$ of $O_2$ and $H_2$ are kept at the same temperature and pressure. Which of the following is true regarding the number of molecules?

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