NH 3 can be liquefied at ordinary temperature without the application of pressure- but O 2 cannot- becauseA- its T C is higher than that of NH 3B- its T C is very lowC- its T C is very moderateD- its T C is very high

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Standard XII

Chemistry

Types of Hydrogen Bonding

NH 3 can be l...

Question

$N H_{3}$ can be liquefied at ordinary temperature without the application of pressure, but $O_{2}$ cannot, because

its T_C is very high

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its T_C is very low

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its T_C is very moderate

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its T_C is higher than that of NH₃

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Solution

The correct option is B
its T_C is very low

Oxygen has a lower critical temperature than ammonia. Lower the critical temperature, lower the extent of liquifaction of a gas.

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Similar questions

N H_{3}

can be liquefied at ordinary temperature without the application of pressure. But

O_{2}

cannot, because:

State True or False.

A gas above its

T_{c}

or its critical temperature can be liquefied.

The essential conditions for liquefaction of gases were discovered by Andrews in

1869

as a result of his study of pressure-volume-temperature relationship for

C O_{2}

. It was found that above a certain temperature, it was impossible to liquefy a gas whatever the pressure was applied. The temperature below which the gas can be liquefied by the application of pressure alone is called critical temperature

(T_{c})

. The pressure required to liquefy a gas at this temperature is called the critical pressure

(P_{c)}

. The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der Waals' constant as follows:

V_{c} = 3 b, P_{c} = \frac{a}{27 b^{2}}, T_{c} = \frac{8 a}{27 R b}

The relationship between

P_{C}, V_{C}

and

T_{C}

The critical temperature $(T_{c})$ and critical pressure $p_{c})$ of $C O_{2}$ are ${30.98}^{\circ} C$ and 73 atm respectively.Can $C O_{2}$ (g) be liquefied at $32^{\circ} C$ and 80 atm pressure?

The essential conditions for liquefaction of gases were discovered by Andrews in

1869

as a result of his study of pressure-volume-temperature relationship for

C O_{2}

(T_{c})

. The pressure required to liquefy a gas at this temperature is called the critical pressure

(P_{c)}

. The volume occupied by one mole of the substance at the critical temperature and pressure is called critical volume. Critical constants are related with van der Waals' constant as follows:

V_{c} = 3 b, P_{c} = \frac{a}{27 b^{2}}, T_{c} = \frac{8 a}{27 R b}

Which of the following parameters is three times the van der Waals' constant

^{'} b^{'}

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NH3 can be liquefied at ordinary temperature without the application of pressure, but O2 cannot, because

The correct option is B its TC is very low Oxygen has a lower critical temperature than ammonia. Lower the critical temperature, lower the extent of liquifaction of a gas.

$N H_{3}$ can be liquefied at ordinary temperature without the application of pressure, but $O_{2}$ cannot, because

The correct option is B
its T_C is very low

Oxygen has a lower critical temperature than ammonia. Lower the critical temperature, lower the extent of liquifaction of a gas.