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Liquefaction of Gases and Critical Constants

Critical temp...

Question

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:

H_{2} O

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N H_{3}

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O_{2}

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C O_{2}

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Solution

The correct option is A $H_{2} O$
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.

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Similar questions

N H_{3}

C O_{2}

N H_{3}

C O_{2}

C O_{2}

405.5 K

304.10 K

M n O_{2} + H C l \to M n C l_{2} + C l_{2} + H_{2} O

N H_{4} C l + C a (O H)_{2} \to N H_{3} + C a C l_{2} + H_{2} O

B a C l_{2} + A l_{2} (S O_{4})_{3} \to B a S O_{4} + A l C l_{3}

N a A l O_{2} + H_{2} O + C O_{2} \to A l H_{3} + N a_{2} C O_{3}

N H_{3} + O_{2} \to N O + H_{2} O

Z n + H N O_{3} \to Z n (N O_{3})_{2} + N O_{2} + H_{2} O

H_{2} S + O_{2} \to H_{2} O + S O_{2}

P b O + C \to P b + C O_{2}

B a C l_{2} + H_{2} S O_{4} \to B a S O_{4} + H C l

C H_{4} + O_{2} \to C O_{2} + H_{2} O

A

N H_{4} C l

D

C O_{2}

B

C

+ N a O H \to N a C l + N H_{3} + H_{2} O

N H_{3} + C O_{2} + H_{2} O \to (B)

+ N a C l \to (C) + N H_{4} C l

\to N a_{2} C O_{3} + H_{2} O + (D)

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