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Kinetic Theory of Gases

The curve of ...

Question

The curve of pressure-volume $(P V)$ against pressure $(P)$ of the gas at a particular temperature is as shown, according to the graph which of the following is incorrect (in the low-pressure region)?

H_{2}

and

H e

show +ve deviation from ideal gas equation

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C O, C H_{4} a n d O_{2}

show negative deviation from ideal gas equation

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H_{2}

and

H e

show negative deviation while

C O_{2}, C H_{4}

and

O_{2}

show positive deviation

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H_{2}

and

H e

are less compressible than that of an ideal gas while

C O_{2}, C H_{4} a n d O_{2}

more compressible than that of ideal gas

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Solution

The correct option is C $H_{2}$ and $H e$ show negative deviation while $C O_{2}, C H_{4}$ and $O_{2}$ show positive deviation
Hydrogen and Helium show positive deviation whereas $C O_{2}, C H_{4}$ and $O_{2}$ first show negative deviation, reach through minimum value and then show positive deviation as the pressure increases.

Hence, the option $C$ is correct.

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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?

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 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}

)

For 500

K

plot value of

Z

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

a t m

to 1200

a t m

(high pressure) then the value of

\frac{b}{R T}

will be:

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
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Which of the following is correct?

Q. The gases that show positive deviation at all pressures at 273 K from ideal gas equation among the following is/are

Q. Real gases show deviations from ideal gas law because molecules interact with each other. At high pressures molecules of gases are very close to each other. At very low temperatures intermolecular forces become significant. The deviation from ideal gas behaviour can be measured in terms of compressibility factor

Z

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P V

and

n R T

(

Z = P V / n R T

) . Taking the pressure and volume corrections due to intermolecular forces vander waals corrected the ideal gas equation.
In vander waals equation of state for non ideal gases, the term that accounts for intermolecular forces

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The curve of pressure-volume (PV) against pressure (P) of the gas at a particular temperature is as shown, according to the graph which of the following is incorrect (in the low-pressure region)?

The curve of pressure-volume $(P V)$ against pressure $(P)$ of the gas at a particular temperature is as shown, according to the graph which of the following is incorrect (in the low-pressure region)?