(C) The critical temperature of $CO_2$ is $30.98 \, ^\circ C$. Above this temperature,$CO_2$ exists only as a gas and cannot be liquefied by pressure

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It becomes a gas at higher temperatures and a liquid at lower temperatures.

(C) The critical temperature of $CO_2$ is $30.98 \, ^\circ C$. Above this temperature,$CO_2$ exists only as a gas and cannot be liquefied by pressure alone. Below this temperature,$CO_2$ can exist as a liquid or a gas-liquid equilibrium mixture depending on the pressure applied.

Class 11 Chemistry States of Matter Critical state and Liquefaction of gases

Easy

What happens when the temperature of $CO_2$ at its critical temperature of $30.98 \, ^\circ C$ is increased or decreased?

A
It remains a gas at all temperatures.
B
It liquefies at higher temperatures.
C
It becomes a gas at higher temperatures and a liquid at lower temperatures.
D
It remains a liquid at all temperatures.

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States of Matter

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Critical state and Liquefaction of gases

Explain the relationship between the fluid state,liquid-gas state,critical temperature,and the vapour form of substances.

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Critical constants for a real gas are given as:
$T_C = 180 \ K$; $V_C = 0.123 \ L \ mol^{-1}$
$P_C = 45 \ atm$; $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$
Which of the following statements is correct for this real gas?

Medium

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Critical temperature for carbon dioxide and methane are $31.1^{\circ} C$ and $-81.9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?

Easy

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The temperature and pressure at which ice,liquid water,and water vapour can exist together are:

Medium

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Critical temperatures for $A$,$B$,$C$ and $D$ gases are $25\,^{\circ}C$,$10\,^{\circ}C$,$-80\,^{\circ}C$ and $15\,^{\circ}C$ respectively. Which gas will be liquefied more easily?

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What happens when the temperature of $CO_2$ at its critical temperature of $30.98 \, ^\circ C$ is increased or decreased?

Similar Questions

Explain the relationship between the fluid state,liquid-gas state,critical temperature,and the vapour form of substances.

Critical constants for a real gas are given as:$T_C = 180 \ K$; $V_C = 0.123 \ L \ mol^{-1}$$P_C = 45 \ atm$; $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$Which of the following statements is correct for this real gas?

Critical temperature for carbon dioxide and methane are $31.1^{\circ} C$ and $-81.9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?

The temperature and pressure at which ice,liquid water,and water vapour can exist together are:

Critical temperatures for $A$,$B$,$C$ and $D$ gases are $25\,^{\circ}C$,$10\,^{\circ}C$,$-80\,^{\circ}C$ and $15\,^{\circ}C$ respectively. Which gas will be liquefied more easily?

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Critical constants for a real gas are given as:
$T_C = 180 \ K$; $V_C = 0.123 \ L \ mol^{-1}$
$P_C = 45 \ atm$; $R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}$
Which of the following statements is correct for this real gas?