Consider the equation Z - pVRT which of the following statement is correct-

The correct options are C When Z = 1, gases get compressed easily. D When Z gt; 1, real gases are difficult to compress than ideal gases.Ideal gases can not ...

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Standard XII

Chemistry

Ideal Gas Equation

Consider the ...

Question

Consider the equation $Z = \frac{pV}{RT}$ which of the following statement is correct?

When Z > 1, real gases are easier to compress than the ideal gas.

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When Z = 1, gases get compressed easily.

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When Z > 1, real gases are difficult to compress than ideal gases.

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When Z = 1, real gases are difficult to compress:

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Solution

The correct options are
C When Z = 1, gases get compressed easily.
D When Z > 1, real gases are difficult to compress than ideal gases.
Ideal gases can not be compressed at all due to the absence of any interactions between the particles of gases.

Z = 1 is for an ideal gas, if a real gas achieves Z=1, then it behaves as an ideal gas but it can be compressed but it is difficult to compress.

When Z > 1 or Z<1, real gases are easier to compress than the ideal gas.

Hence, Option "B" & "C" are correct answers.

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Similar questions

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. Assertion :Compressibility factor Z according to van der Waal's equation may be written as

Z = \frac{1}{1 - (\frac{n b}{V})} - \frac{a n}{R T V}

. Reason: For real gases

Z >< 1

Q. Assertion :Compressibility factor

(Z)

for non ideal gases is always greater than 1. Reason: Non-ideal gases always exert higher pressure than expected.

The given graph in Fig represents the variation of Z $(c o m p r e s s i b i l i t y f a c t o r = \frac{p V}{n R T}$ ) vs.P , for the three real gases A,B and C.identify the only incorrect statement
$1 - \frac{p b}{R T}$

Q. The given graph represent the variations of

Z

(compressibility factor

(Z) = \frac{p V}{n R T})

versus

P

, for three real gases

A, B

and

C

. Identify the only incorrect statement.

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Consider the equation Z=pVRT which of the following statement is correct?

Consider the equation $Z = \frac{pV}{RT}$ which of the following statement is correct?