Critical temperature of H2O-NH3-CO2 and O2 are 647K-405-6K-304-10K and 154-2K respectively- If the cooling starts from 500K to their temperature- the gas that liquefies first is-

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Critical Temperature of the gas in critical state- above which it cannot be liquefied-xA0- by pressure-xA0-Here- cooling starts from 500 K to critical temperature- So- H2O will liquefied first due to it-apos-s maximum critical temperature value-xA0-xA0-

Critical temperature of $H_{2} O, N H_{3}, C O_{2}$ and $O_{2}$ are $647 K, 405.6 K, 304.10 K$ and $154.2 K$ respectively. If the cooling starts from $500 K$ to their temperature, the gas that liquefies first is:

Critical Temperature of the gas in critical state, above which it cannot be liquefied by pressure.
Here, cooling starts from 500 K to critical temperature. So, $H_{2} O$ will liquefied first due to it's maximum critical temperature value.

Critical temperature of H2O,NH3,CO2 and O2 are 647K,405.6K,304.10K and 154.2K respectively. If the cooling starts from 500K to their temperature, the gas that liquefies first is:

Critical Temperature of the gas in critical state, above which it cannot be liquefied by pressure. Here, cooling starts from 500 K to critical temperature. So, H2O will liquefied first due to it's maximum critical temperature value.

Critical temperature of $H_{2} O, N H_{3}, C O_{2}$ and $O_{2}$ are $647 K, 405.6 K, 304.10 K$ and $154.2 K$ respectively. If the cooling starts from $500 K$ to their temperature, the gas that liquefies first is:

Critical Temperature of the gas in critical state, above which it cannot be liquefied by pressure.
Here, cooling starts from 500 K to critical temperature. So, $H_{2} O$ will liquefied first due to it's maximum critical temperature value.