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Which of the following statements is correct for the spontaneous adsorption of a gas?

1.	∆ S is negative and therefore, ∆ H should be highly positive
2.	∆ S is negative and therefore, ∆ H should be highly negative
3.	∆ S is positive and therefore, ∆ H should be negative
4.	-∆ S is positive and therefore, ∆ H should also be highly positive

Subtopic: Adsorption and Absorption |

55%

Level 3: 35%-60%

AIPMT - 2014

Hints

The Langmuir adsorption isotherm is deduced using the assumption:

1.	The adsorption takes place in multilayers
2.	The adsorption sites are equivalent in their ability to adsorb the particles
3.	The heat of adsorption varies with coverage
4.	The adsorbed molecules interact with each other

Subtopic: Adsorption and Absorption |

61%

Level 2: 60%+

AIPMT - 2007

Hints

A plot of log x/m versus log p for the adsorption of a gas on a solid gives a straight line with a slope equal to:

1. log

2. n

3. $\frac{1}{n}$

4. log 1/k

Subtopic: Adsorption and Absorption | Adsorption Isotherm |

77%

Level 2: 60%+

AIPMT - 2006

Hints