(A) From the ideal gas equation,$PV = nRT = \frac{m}{M} RT$. Since density $d = \frac{m}{V}$,we have $P = \frac{dRT}{M}$,which implies $d = \frac{PM}{

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$d_2 = d_1 \left( \frac{T_1 P_2}{T_2 P_1} \right)$

(A) From the ideal gas equation,$PV = nRT = \frac{m}{M} RT$. Since density $d = \frac{m}{V}$,we have $P = \frac{dRT}{M}$,which implies $d = \frac{PM}{RT}$. For a constant mass of gas,$\frac{d_1 T_1}{P_1} = \frac{d_2 T_2}{P_2}$. Rearranging for $d_2$,we get $d_2 = d_1 \left( \frac{T_1 P_2}{T_2 P_1} \right)$.

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

Medium

Which of the following represents the correct relationship between the change in density of an ideal gas and the change in temperature?

A
$d_2 = d_1 \left( \frac{T_1 P_2}{T_2 P_1} \right)$
B
$d_2 = d_1 \left( \frac{T_1 T_2}{P_2 P_1} \right)$
C
$d_2 = d_1 \left( \frac{T_1 P_1}{P_2 T_2} \right)$
D
$d_2 = d_1 \left( \frac{T_2 P_2}{P_1 T_1} \right)$

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Ideal gas equation and Related gas laws

By what other name is the ideal gas equation known? Why?

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At constant temperature, a gas occupies a volume of $200 \text{ mL}$ at a pressure of $500 \text{ mm Hg}$. What will be its volume at $800 \text{ mm Hg}$ pressure (in $\text{ mL}$)?

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Explain: Gay-Lussac's Law.

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Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

MediumNEET 2021

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At $0\, ^\circ C$,$4\, g$ of $O_2$ and $2\, g$ of $H_2$ are filled in a $1\, L$ bulb. What will be the total pressure of the mixture (in $, atm$)?

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Which of the following represents the correct relationship between the change in density of an ideal gas and the change in temperature?

Similar Questions

By what other name is the ideal gas equation known? Why?

At constant temperature, a gas occupies a volume of $200 \text{ mL}$ at a pressure of $500 \text{ mm Hg}$. What will be its volume at $800 \text{ mm Hg}$ pressure (in $\text{ mL}$)?

Explain: Gay-Lussac's Law.

Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

At $0\, ^\circ C$,$4\, g$ of $O_2$ and $2\, g$ of $H_2$ are filled in a $1\, L$ bulb. What will be the total pressure of the mixture (in $, atm$)?

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Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$