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 overpressure range in the low pressure region- Boyle-s temperature T b - a - Rb- If a plot i 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 pressureregion-Which of the following is correct- a-b-0-4 kcalmol -1B- 1 kcalmol -1-1-2-2 kcalmol -1a-b-1 kcalmol -D- a-b-0-2 kcalmol -1

The correct option is B 1 kcalmol^ 1 lt; 12 lt; 2 kcalmol^ 1From graph, 500K lt; aRb lt; 1000 K and R ∼ 2 Cal/mol/K ∴ 500R lt; ab lt; 1000R ∴ 1kc ...

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Byju's Answer

Standard XII

Chemistry

Compressibility Factor

The sketch sh...

Question

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?

\frac{a}{b} < 0.4 k c a l m o l^{- 1}

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1 k c a l m o l^{- 1} < \frac{1}{2} < 2 k c a l m o l^{- 1}

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\frac{a}{b} < 0.2 k c a l m o l^{- 1}

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\frac{a}{b} = 1 k c a l m o l^{- 1}

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Solution

The correct option is B $1 k c a l m o l^{- 1} < \frac{1}{2} < 2 k c a l m o l^{- 1}$
From graph, $500 K < \frac{a}{R b} < 1000 K$
and $R \sim 2 C a l / m o l / K$
$∴ 500 R < \frac{a}{b} < 1000 R$
$∴ 1 k c a l / m o l < \frac{a}{b} < 2 k c a l / m o l$

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Similar questions

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. 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}

500 K, Z

changes from 2 to 2.2 as the pressure varies from 1000 atm to

1200 atm

(high pressure). 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}

500 K, Z

changes from 2 to 2.2 as the pressure varies from 1000 atm to

1200 atm

(high pressure). The value of

\frac{b}{R T}

will be:

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:

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The correct option is B 1 kcalmol−1<12<2 kcalmol−1From graph, 500K<aRb<1000K and R∼2 Cal/mol/K ∴500R<ab<1000R ∴1kcal/mol<ab<2kcal/mol

The correct option is B $1 k c a l m o l^{- 1} < \frac{1}{2} < 2 k c a l m o l^{- 1}$
From graph, $500 K < \frac{a}{R b} < 1000 K$
and $R \sim 2 C a l / m o l / K$
$∴ 500 R < \frac{a}{b} < 1000 R$
$∴ 1 k c a l / m o l < \frac{a}{b} < 2 k c a l / m o l$