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H(2) gas is adsorbed on activated charco...

`H_(2)` gas is adsorbed on activated charcoal to a very little extent in comparison to easily liquefiable gases due to ……. .

A

very strong van der Waals' interaction

B

very weak van der Waals' forces

C

very low critical temperature

D

very high critical temperature

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To solve the question regarding the adsorption of \( H_2 \) gas on activated charcoal, we can break it down into the following steps: ### Step 1: Understand the Concept of Adsorption Adsorption is the process by which atoms, ions, or molecules from a gas, liquid, or dissolved solid adhere to a surface. The extent of adsorption depends on various factors, including the nature of the adsorbate (the substance being adsorbed) and the adsorbent (the surface on which adsorption occurs). ### Step 2: Identify the Nature of \( H_2 \) Gas \( H_2 \) gas is a diatomic molecule that is non-polar and has a very low molecular weight. Due to its small size and non-polar nature, the intermolecular forces acting on \( H_2 \) are weak Van der Waals forces. ### Step 3: Compare with Easily Liquefiable Gases Easily liquefiable gases (like \( SO_2 \) and \( NH_3 \)) have higher critical temperatures. A high critical temperature indicates that the gas can be easily condensed into a liquid state, which correlates with stronger intermolecular forces (like dipole-dipole interactions or stronger Van der Waals forces). ### Step 4: Relate Critical Temperature to Adsorption The extent of adsorption is directly proportional to the critical temperature of the gas. Gases with higher critical temperatures are more likely to be adsorbed because they can interact more strongly with the adsorbent due to their stronger intermolecular forces. ### Step 5: Conclusion Since \( H_2 \) has a very low critical temperature and weak Van der Waals forces, it is adsorbed to a much lesser extent on activated charcoal compared to easily liquefiable gases. ### Final Answer The reason \( H_2 \) gas is adsorbed on activated charcoal to a very little extent in comparison to easily liquefiable gases is due to: - Very weak Van der Waals forces of attraction. - Very low critical temperature.
To solve the question regarding the adsorption of \( H_2 \) gas on activated charcoal, we can break it down into the following steps: ### Step 1: Understand the Concept of Adsorption Adsorption is the process by which atoms, ions, or molecules from a gas, liquid, or dissolved solid adhere to a surface. The extent of adsorption depends on various factors, including the nature of the adsorbate (the substance being adsorbed) and the adsorbent (the surface on which adsorption occurs). ### Step 2: Identify the Nature of \( H_2 \) Gas \( H_2 \) gas is a diatomic molecule that is non-polar and has a very low molecular weight. Due to its small size and non-polar nature, the intermolecular forces acting on \( H_2 \) are weak Van der Waals forces. ...
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