Single Choice

Consider the following table: Gas $$a/(k Pa dm^6 mol^{-1})$$ $$b / (dm^3 mol^{-1})$$ A 642.32 0.05196 B 155.21 0.04136 C 431.91 0.05196 D 155.21 0.4382 a and b are vander waals constant. The correct statement about the gases is:

Agas C will occupy lesser volume than gas A; gas B will be lesser compressible than gas D
Bgas C will occupy more volume than gas A; gas B will be lesser compressible than gas D
Cgas C will occupy more volume than gas A; gas B will be more compressible than gas D
Correct Answer
Dgas C will occupy lesser volume than gas A; gas B will be more compressible than gas D

Solution

Solution:- (C) Gas C will occupy more volume than gas A; gas B will be more compressible than gas D
$$\bullet$$ Gas A and C have same value of 'b' but different value of 'a' so gas having higher value of 'a' have more force of attraction so molecules will be more closer hence occupy less volume.
$$\bullet$$ Gas B and D have same value of 'a' but different value of 'b' so gas having lesser value of 'b' will be more compressible.
So option (C) is correct.

SIMILAR QUESTIONS

States of Matter - Gas and Liquid

The compressibility factor for $$H_{2}$$ and $$He$$ is usually:

States of Matter - Gas and Liquid

If $$ Z$$ is a compressibility factor, van der Waals equation at low pressure can be written as:

States of Matter - Gas and Liquid

The behaviour of a real gas is usually depicted by plotting compressibility factor Z versus P at a constant temperature. At high temperature and high pressure, Z is usually more than one. This fact can be explained by van der Waal's equation when:

States of Matter - Gas and Liquid

The compressibility factor for $$CO_2$$ at 273 $$K$$ and 100 $$atm$$ pressure is 0.2005. The volume occupied by 0.2 mole of $$CO_2$$ gas at 100 $$atm$$ and 273 $$K$$ using real gas nature is $$8.89\times 10^{-x} \:litre$$. So, value of $$x$$ is.....

States of Matter - Gas and Liquid

At low pressures, the van der Waals equation is written as $$\displaystyle \left [ P+\frac{a}{V^2} \right ]V=RT$$ The compressibility factor is then equal to :

States of Matter - Gas and Liquid

At very high pressures, the compressibility factor of one mole of a gas is given by :

States of Matter - Gas and Liquid

The compressibility factor for a real gas at high pressure is:

States of Matter - Gas and Liquid

At a moderate pressure, the van der Waal's equation is written as: $$\left[P+\dfrac{a}{V^2}\right]V=RT$$ The compressibility factor is equal to:

States of Matter - Gas and Liquid

Calculate the number of $$\alpha$$ and $$\beta$$ particles is the following change : $$U^{235}_{92}\longrightarrow \, ^{207}_{82}Pb$$

States of Matter - Gas and Liquid

For a real gas, the compressibility factor $$Z$$ has different values at different temperature and pressures. Which of the following is not correct under the given condition?

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