AP EAMCET · Chemistry · States of Matter

Which among the following statements is/are incorrect regarding real gases?
(i) Their compressibility factor is never equal to unity $(Z \neq 1)$ .
(ii) The deviations from ideal behavior are less at low pressures and high temperatures.
(iii) Intermolecular forces among gas molecules are equal to zero.
(iv) The obey Van der Waals equation, $PV = nRT$ .

A (i), (ii), (iv) only
B (ii), (iv) only
C (ii) only
D (iii), (iv) only

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Answer & Solution

Correct Answer

(D) (iii), (iv) only

Step-by-step Solution

Detailed explanation

At high pressure, the gas molecules come close to each other and the empty space between the molecules is reduced to some extent. Therefore the gas becomes less compressible at these higher pressures For the real gas equation is P+anV2V-nb = RT Thus, Intermolecular…

Apply the relevant identity from the chapter and substitute the values established in the previous step, keeping the original constraint in view.

Use the simplified expression to isolate the unknown, then plug the result back into the question setup to confirm the working is internally consistent.

Cross-check against a boundary or limiting case. Both the dimensional balance and the qualitative behaviour at the extreme should agree with the candidate answer.

Combine the steps above to identify the correct option. The remaining choices each fail at least one of the consistency, dimensional, or boundary checks.

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