(A) : CO2 cannot be liquified above 304K, critical temperature of CO2(R) : At a certain temperature, volume ∝1pressure

CO2 has a critical temperature of 304.2 K (31.0 °C) and a critical pressure of 73.8 atm. Above the critical temperature, CO2 cannot be liquefied by increasing the pressure alone. This is because, at or above the critical temperature, the intermolecular forces between CO2 molecules become weak, and the gas behaves more like a supercritical fluid, which has properties intermediate between those of a gas and a liquid.In order to liquefy CO2 above its critical temperature, it must be cooled below its critical temperature while simultaneously increasing the pressure. This requires specialized equipment such as high-pressure pumps and refrigeration systems. However, if the temperature remains above the critical temperature, no amount of pressure can liquefy CO2.At a constant temperature and with a fixed number of moles of gas, the volume of a gas is inversely proportional to its pressure.This is known as Boyle's law, which states that PV = K, where P is the pressure, V is the volume, and K is a constant. Therefore, if the pressure is increased, the volume of the gas will decrease, and vice versa, as long as the temperature and number of moles of gas remain constant.So, both (A) and (R) are correct but, (R) is not the correct explanation of (A).

(A) : CO2 cannot be liquified above 304K, critical temperature of CO2(R) : At a certain temperature, volume ∝1pressure

CO2 has a critical temperature of 304.2 K (31.0 °C) and a critical pressure of 73.8 atm. Above the critical temperature, CO2 cannot be liquefied by increasing the pressure alone. This is because, at or above the critical temperature, the intermolecular forces between CO2 molecules become weak, and the gas behaves more like a supercritical fluid, which has properties intermediate between those of a gas and a liquid.In order to liquefy CO2 above its critical temperature, it must be cooled below its critical temperature while simultaneously increasing the pressure. This requires specialized equipment such as high-pressure pumps and refrigeration systems. However, if the temperature remains above the critical temperature, no amount of pressure can liquefy CO2.At a constant temperature and with a fixed number of moles of gas, the volume of a gas is inversely proportional to its pressure.This is known as Boyle's law, which states that PV = K, where P is the pressure, V is the volume, and K is a constant. Therefore, if the pressure is increased, the volume of the gas will decrease, and vice versa, as long as the temperature and number of moles of gas remain constant.So, both (A) and (R) are correct but, (R) is not the correct explanation of (A).

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(A) : CO₂ cannot be liquified above 304K, critical temperature of CO₂
(R) : At a certain temperature, volume $\propto \frac{1}{pressure}$

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(A) is true but (R) is false

Both (A) and (R) are correct and (R) is the correct explanation of (A)

Both (A) and (R) are false

Both (A) and (R) are correct but (R) is not the correct explanation of (A)

answer is B.

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Detailed Solution

CO₂ has a critical temperature of 304.2 K (31.0 °C) and a critical pressure of 73.8 atm.
Above the critical temperature, CO₂ cannot be liquefied by increasing the pressure alone.
This is because, at or above the critical temperature, the intermolecular forces between CO₂ molecules become weak, and the gas behaves more like a supercritical fluid, which has properties intermediate between those of a gas and a liquid.
In order to liquefy CO₂ above its critical temperature, it must be cooled below its critical temperature while simultaneously increasing the pressure.
This requires specialized equipment such as high-pressure pumps and refrigeration systems. However, if the temperature remains above the critical temperature, no amount of pressure can liquefy CO₂.
At a constant temperature and with a fixed number of moles of gas, the volume of a gas is inversely proportional to its pressure.
This is known as Boyle's law, which states that PV = K, where P is the pressure, V is the volume, and K is a constant.
Therefore, if the pressure is increased, the volume of the gas will decrease, and vice versa, as long as the temperature and number of moles of gas remain constant.
So, both (A) and (R) are correct but, (R) is not the correct explanation of (A).

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