p-Block Elements

To determine which of the given reactions of Xenon compounds is not feasible, we can analyze each option based on the chemical properties and reactivity of the substances involved :

1. Option A :
   $ \text{XeO}_3 + 6\text{HF} \to \text{XeF}_6 + 3\text{H}_2\text{O} $ This reaction involves the conversion of xenon trioxide to xenon hexafluoride. While both compounds are known, the direct conversion of XeO₃ to XeF₆ is not typically feasible due to the different oxidation states of xenon in these compounds and the reaction conditions required.

2. Option B :
   $ \text{XeF}_6 + \text{RbF} \to \text{Rb}[\text{XeF}_7] $ This reaction represents the formation of a rubidium heptafluoroxenate(VII) compound. XeF₆ can react with RbF to form Rb[XeF₇], which is a known compound. This reaction is feasible.

3. Option C :
   $ 2\text{XeF}_2 + 2\text{H}_2\text{O} \to 2\text{Xe} + 4\text{HF} + \text{O}_2 $ In this reaction, xenon difluoride is reacting with water to produce xenon, hydrofluoric acid, and oxygen. XeF₂ is known to hydrolyze in the presence of water to produce these products, making this reaction feasible.

4. Option D :
   $ 3\text{XeF}_4 + 6\text{H}_2\text{O} \to 2\text{Xe} + \text{XeO}_3 + 12\text{HF} + 1.5\text{O}_2 $ This reaction suggests that xenon tetrafluoride reacts with water to form xenon, xenon trioxide, hydrofluoric acid, and oxygen. The formation of XeO₃ and O₂ in this reaction is feasible as XeF₄ can undergo hydrolysis under certain conditions.

Given these considerations, Option A is the least feasible reaction among the ones listed. The direct conversion of XeO₃ to XeF₆ is not commonly reported or expected under normal chemical reaction conditions.

To identify the incorrect statement among the given options, let's analyze each one :

1. Option A : Ozone reacts with SO₂ to give SO₃.

   
   
   • Ozone (O₃) can react with sulfur dioxide (SO₂) to form sulfur trioxide (SO₃). This reaction is a part of the atmospheric chemistry where ozone acts as an oxidizing agent.



2. Option B : Silicon reacts with NaOH(aq) in the presence of air to give Na₂SiO₃ and H₂O.

   
   
   • Silicon reacts with sodium hydroxide (NaOH) in the presence of air (oxygen) to form sodium silicate (Na₂SiO₃) and water (H₂O). This reaction is feasible as silicon can be oxidized and dissolved by NaOH, especially in the presence of oxygen.



3. Option C : Cl₂ reacts with excess of NH₃ to give N₂ and HCl.

   
   
   • When chlorine (Cl₂) reacts with an excess of ammonia (NH₃), the main products are nitrogen (N₂) and hydrogen chloride (HCl). This reaction is a well-known example of a redox reaction where chlorine is reduced and ammonia is oxidized.



4. Option D : Br₂ reacts with hot and strong NaOH solution to give NaBr, NaBrO₄, and H₂O.

   
   
   • Bromine (Br₂) reacts with hot and concentrated sodium hydroxide (NaOH) to form sodium bromide (NaBr), sodium bromate (NaBrO₃), and water (H₂O). The formation of sodium perbromate (NaBrO₄) is not typical in this reaction under normal conditions. Usually, NaBr and NaBrO₃ are the primary products.

Based on this analysis, the incorrect statement is Option D. The expected products of the reaction between Br₂ and hot, concentrated NaOH are NaBr and NaBrO₃, not NaBr, NaBrO₄, and H₂O.

When phosphine gas (PH₃) is mixed with chlorine gas (Cl₂), the reaction between them depends on the conditions and the proportions of the reactants. Let's consider the options :

1. Option A : PCl₃ and HCl are formed and the mixture warms up.

   
   
   • When phosphine gas reacts with chlorine gas, one of the possible products is phosphorus trichloride (PCl₃) along with hydrogen chloride (HCl). This reaction is exothermic, meaning it releases heat and causes the mixture to warm up.



2. Option B : PCl₅ and HCl are formed and the mixture cools down.

   
   
   • Phosphorus pentachloride (PCl₅) can be formed if an excess of chlorine is used, but this reaction is also exothermic. The formation of PCl₅ is less likely with PH₃ as it requires a higher proportion of chlorine and controlled conditions.



3. Option C : PH₃·Cl₂ is formed with warming up.

   
   
   • There is no known stable compound like PH₃·Cl₂ formed directly from the reaction of phosphine and chlorine gas. This option does not represent a typical chemical reaction product.



4. Option D : The mixture only cools down.

   
   
   • Chemical reactions between phosphine and chlorine are exothermic, so this statement is incorrect.

Based on this analysis, the most likely and correct reaction is described in Option A : PCl₃ and HCl are formed, and the mixture warms up. This reaction is feasible and aligns with the known chemistry of phosphine and chlorine gases.