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Introduction

Which of the ...

Question

Which of the following statement(s) is/are correct for a real gas at a temperature below its critical temperature?

A

The gas can be liquified on applying pressure at constant temperature

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B

The compression curve of the gas (P vs V isotherm) has negative slope only

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C

For each gas, in very high pressure region, Z is always greater than one

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D

In low pressure region, Z can be greater than one for a gas

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Solution

The correct options are
B The gas can be liquified on applying pressure at constant temperature
C In low pressure region, Z can be greater than one for a gas
D For each gas, in very high pressure region, Z is always greater than one
The critical temperature is the highest temperature at which the gas starts condensing in a liquid. When the temperature of a gas is below its critical temperature, and pressure is applied at a constant temperature, the gas is liquified.
The compressibility factor $z = \frac{P V}{n R T}$ . It is always greater than one for any gas in the very high-pressure region. This is because the pressure term appears in the numerator. In the low-pressure region, it can be greater than one for gas. This is possible at low temperature and high volume.

Hence, the correct answer is options $A, C and D$ .

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Similar questions

Q. The sketch shows the plot of Z v/s P for a hypothetical gas for one mole at three distinct temperature . Boyle's temperature is the temperature at which a gas shows ideal behavior over a pressure range in the low-pressure region .Boyle's temperature

(T_{b})

\frac{a}{R b}

.If a plot is obtained at temperatures well below Boyle's temperature then the curve will show negative deviation,in low-pressure region and positive deviation in the high-pressure region.Near critical temperature, the curve is more likely as

C O_{2}

and the temperature well above critical temperature curve is more like

H_{2}

O^{0}

C as shown above.At high pressure suppose all the constant temperature curve varies linearly with pressure according to the following equation

Z = 1 + \frac{P b}{R T} (R = 2 c a l m o l^{- 1} K^{- 1}

Which of the following is correct?

Q. Assertion (A): Real gases tend to behave as ideal gas at low pressure and high Temperature.
Reason (R): At temperature more than critical temperature, a gas can’t be liquefied just by increasing the pressure. Which of the followings is correct?

The sketch shows the plot of

Z

P

for a hypothetical gas for one mole at three distinct temperature. Boyle's temperature is the temperature at which a gas shows ideal behavior over a pressure range in the low-pressure region. Boyle's temperature

(T_{b})

\frac{a}{R b}

.If a plot is obtained at temperatures well below Boyle's temperature then the curve will show negative deviation, in the low-pressure region and positive deviation in the high-pressure region. Near critical temperature, the curve is more likely as

C O_{2}

and the temperature well above critical temperature curve is more like

H_{2}

O^{o} C

as shown above.At high pressure suppose all the constant temperature curve varies linearly with pressure according to the following equation

Z = 1 + \frac{P b}{R T} (R = 2 c a l m o l^{- 1} K^{- 1}

)

K

Z

changes from 2 to 2.2 ,if pressure is varied from 1000

a t m

a t m

(high pressure) then the value of

\frac{b}{R T}

Q. The sketch shows the plot of Z vs P for 1 mole of a hypothetical gas at three distinct
temperatures:

Boyle's temperature is the temperature at which a gas shows ideal behaviour over a
pressure range in the low pressure region. Boyle's temperature

(T_{b}) = \frac{a}{R b}

. If a plot is
obtained at temperatures well below Boyle's temperature, then the curve will show a negative deviation in the low pressure region and a positive deviation in the high pressure
region.

Which of the following is correct?

Q. A gas can be liquified by pressure alone only, when its temperature is ___________ its critical temperature.

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