The densities of the three gases O2 - SO2 and H2 are measured at 400 K and 1 atm- They are 0-8 g-L - 3215 g-L and 125 g-L respectively - Which of the following statements is - are correct for these gases - Use R - 112 L atm-mol K -

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Standard XII

Physics

P-T Relationship

The densities...

Question

The densities of the three gases $O_{2}, S O_{2}$ and $H_{2}$ are measured at $400 K$ and $1 a t m$ . They are $0.8 g / L, \frac{32}{15} g / L$ and $\frac{1}{25} g / L$ respectively . Which of the following statements is / are correct for these gases ? (Use $R = \frac{1}{12} L a t m / m o l K$ ) .

S O_{2}

is showing negative deviation from ideal behaviour .

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O_{2}

is more compressible than ideal gas under these conditions .

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H_{2}

is behaving ideally .

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Boyle's temperature of

O_{2}

is less than

400 K

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Solution

The correct options are
A $S O_{2}$ is showing negative deviation from ideal behaviour .
D Boyle's temperature of $O_{2}$ is less than $400 K$ .

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Similar questions

Q. Ideal gases and real gases behave in similar ways under certain conditions. However, under specific conditions, real gases deviate from ideal behaviour. Which gas deviates most from ideal behavior?

The gases which strictly follow the general equation

(P V = n R T)

are called ideal or perfect gases. Actually, there is no gas which is perfect or ideal. A real gas is one which actually exists, whether it obeys gas laws strictly or not. Under ordinary conditions, only those gases nearly behave as ideal or perfect which have very low boiling points such as nitrogen, hydrogen, etc. The most easily liquefiable and highly soluble gases such as ammonia, carbon dioxide, sulphur dioxide show large deviations.
A very convenient method of studying deviation of real gases from ideal behaviour is through a compressibility factor

(Z)

Z = \frac{P V}{n R T}

(i)

Z = 1

, for ideal gases.
(ii)

Z \neq 1

, for real gases.

The compressibility of a gas is less than unity at STP, therefore:

Q. The vander waals constant for

O_{2}

are a=1.59 atm

L^{2}

m o l^{- 2}

and b=0.0318 L

m o l^{- 1}

.Calculate the temperature at which

O^{2}

gas behaves,ideally for longer range of pressure.

O_{2}

and

S O_{2}

gases are filled in ratio of

1 : 3

by moles in a closed container of

3 L

at temperature of

27^{\circ} C

. If the partial pressure of

O_{2}

0.54 atm

, then the concentration of

S O_{2} ({in mol L}^{- 1})

would be

(R = 0.082 {L atm K}^{- 1} m o l^{- 1})

Q. The degree of dissociation is

0.4

400 K

and

1 a t m

for the gaseous reaction.

P C l_{5} ⇌ P C l_{3} + C l_{2}

. Assuming ideal behaviour of all the gases. Calculate the density of the equilibrium mixture at

400 K

and

1

atm Pressure.

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The densities of the three gases O2,SO2 and H2 are measured at 400K and 1atm. They are 0.8g/L,3215g/L and 125g/L respectively . Which of the following statements is / are correct for these gases ? (Use R=112L atm/mol K ) .

The correct options are A SO2 is showing negative deviation from ideal behaviour . D Boyle's temperature of O2 is less than 400K.

The densities of the three gases $O_{2}, S O_{2}$ and $H_{2}$ are measured at $400 K$ and $1 a t m$ . They are $0.8 g / L, \frac{32}{15} g / L$ and $\frac{1}{25} g / L$ respectively . Which of the following statements is / are correct for these gases ? (Use $R = \frac{1}{12} L a t m / m o l K$ ) .

The correct options are
A $S O_{2}$ is showing negative deviation from ideal behaviour .
D Boyle's temperature of $O_{2}$ is less than $400 K$ .