Question

Assertion :$S{O}_2$ gases is easily liquefied while $H_2$ is not. Reason: $S{O}_2$ has low critical temperature while $H_2$ has high critical temperature.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Both Assertion and Reason are incorrect

Answer 1

The correct option is C Assertion is correct but Reason is incorrect

Assertion
$S{O}_2$ gases is easily liquefied while $H_2$ is not.
Reason
$S{O}_2$ has high critical temperature while $H_2$ has low critical temperature.
Assertion is correct but Reason is incorrect
Note: Permanent gases (such as $H_2$) have very low critical temperature.
Temporary gases (such as $S{O}_2$) have critical temperature very near to ordinary temperature.
$S{O}_2$ is a polar molecule with strong intermolecular forces of attraction and high value of the Van der Waals' constant 'a'.
$H_2$ is a no-polar molecule with weak Van der Waals' forces of attraction and low value of the Van der Waals' constant 'a'.