Complete the following: XeF 4 + O 2 F 2 → XeF 2 + H 2 O →

The complete balanced reaction is: XeF 4 + O 2 F 2 → XeF 6 + O 2 Xenon-fluorine compounds: Xenon forms three binary fluorides, XeF 2 , XeF 4 and XeF 6 by the direct reaction of elements under appropriate experimental conditions. Xe ( g ) + F 2 ( g ) → 673 K , 1 bar XeF 2 ( s ) ( xenon in excess ) Xe ( g ) + 2 F 2 ( g ) → 873 K , 7 bar XeF 4 ( s ) ( 1 : 5 ratio ) Xe ( g ) + 3 F 2 ( g ) → 573 K , 60 - 70 bar XeF 6 ( s ) ( 1 : 20 ratio ) XeF 6 can also be prepared by the interaction of XeF 4 and O 2 F 2 at 143K. XeF 4 + O 2 F 2 → XeF 6 + O 2 The complete balanced reaction is: 2 XeF 2 + 2 H 2 O → 2 Xe + 4 HF + O 2 Xenon-fluorine compounds: Xenon forms three binary fluorides, XeF 2 , XeF 4 and XeF 6 which are colourless crystalline solids and sublime readily at 298 K. They are powerful fluorinating agents. They are readily hydrolysed even by traces of water. For example, XeF 2 is hydrolysed to give xenon, hydrogen fluoride and oxygen. . 2 XeF 2 ( s ) + 2 H 2 O ( l ) → 2 Xe ( g ) + 4 HF ( aq ) + O 2 ( g ) Note: In general, noble gases are the least reactive. Their inertness to chemical reactivity is attributed to the following reasons: The noble gases except helium ( 1 s 2 ) have completely filled ns 2 np 6 electronic configuration in their valence shell. They have high ionisation enthalpy and more positive electron gain enthalpy. The reactivity of noble gases has been investigated occasionally, ever since their discovery, but all attempts to force them to react to form the compounds were unsuccessful for quite a few years. In March 1962 , Neil Bartlett, then at the University of British Columbia, observed the reaction of xenon noble gas. After this discovery, a number of xenon compounds mainly with the most electronegative elements like fluorine and oxygen, have been synthesised. The compounds of krypton are fewer. Only the difluoride ( KrF 2 ) has been studied in detail. Compounds of radon have not been isolated but only identified (e.g., RnF 2 ) by radiotracer technique. No true compounds of Ar , Ne or He are yet known.

Complete the following: XeF 4 + O 2 F 2 → XeF 2 + H 2 O →

The complete balanced reaction is: XeF 4 + O 2 F 2 → XeF 6 + O 2 Xenon-fluorine compounds: Xenon forms three binary fluorides, XeF 2 , XeF 4 and XeF 6 by the direct reaction of elements under appropriate experimental conditions. Xe ( g ) + F 2 ( g ) → 673 K , 1 bar XeF 2 ( s ) ( xenon in excess ) Xe ( g ) + 2 F 2 ( g ) → 873 K , 7 bar XeF 4 ( s ) ( 1 : 5 ratio ) Xe ( g ) + 3 F 2 ( g ) → 573 K , 60 - 70 bar XeF 6 ( s ) ( 1 : 20 ratio ) XeF 6 can also be prepared by the interaction of XeF 4 and O 2 F 2 at 143K. XeF 4 + O 2 F 2 → XeF 6 + O 2 The complete balanced reaction is: 2 XeF 2 + 2 H 2 O → 2 Xe + 4 HF + O 2 Xenon-fluorine compounds: Xenon forms three binary fluorides, XeF 2 , XeF 4 and XeF 6 which are colourless crystalline solids and sublime readily at 298 K. They are powerful fluorinating agents. They are readily hydrolysed even by traces of water. For example, XeF 2 is hydrolysed to give xenon, hydrogen fluoride and oxygen. . 2 XeF 2 ( s ) + 2 H 2 O ( l ) → 2 Xe ( g ) + 4 HF ( aq ) + O 2 ( g ) Note: In general, noble gases are the least reactive. Their inertness to chemical reactivity is attributed to the following reasons: The noble gases except helium ( 1 s 2 ) have completely filled ns 2 np 6 electronic configuration in their valence shell. They have high ionisation enthalpy and more positive electron gain enthalpy. The reactivity of noble gases has been investigated occasionally, ever since their discovery, but all attempts to force them to react to form the compounds were unsuccessful for quite a few years. In March 1962 , Neil Bartlett, then at the University of British Columbia, observed the reaction of xenon noble gas. After this discovery, a number of xenon compounds mainly with the most electronegative elements like fluorine and oxygen, have been synthesised. The compounds of krypton are fewer. Only the difluoride ( KrF 2 ) has been studied in detail. Compounds of radon have not been isolated but only identified (e.g., RnF 2 ) by radiotracer technique. No true compounds of Ar , Ne or He are yet known.

Describe the manufacture of H 2 SO 4 by contact process.

Sulphuric acid is manufactured on a large scale by the contact process. It involves the following three steps: Step (I): Sulphur or sulphide ores are burnt in air to form SO 2 . Step (II): SO 2 is converted into SO 3 in the presence of V 2 O 5 as a catalyst. 2 SO 2 g + O 2 g → V 2 O 5 2 SO 3 g ∆ t H ° = - 196 . 6 kJmol - 1 Step (III): SO 3 produced in the above step is absorbed on H 2 SO 4 to give H 2 S 2 O 7 (Oleum). This oleum is then diluted to obtain H 2 SO 4 of the desired concentration. H 2 SO 4 + SO 3 → H 2 S 2 O 7 Oleum H 2 S 2 O 7 + H 2 O → 2 H 2 SO 4 Sulphuric acid The second step is the key step. It is very crucial to maximise the yield of H 2 SO 4 . The above reaction is exothermic, reversible, and the forward reaction leads to a decrease in volume. So, in accordance with Le Chatelier's principle, low temperature and high pressure are the favourable conditions for maximum yield. But the temperature should not be too low since the rate of reaction will become slow. The optimum conditions in the contact process to maximise the yield of sulphuric acid in an industrial plant is a pressure of 2 bar and temperature around 720 K .

How does chlorine react with: dry slaked lime?

Bleaching powder is produced by passing chlorine gas through dry slaked lime (calcium hydroxide). The equation for the reaction of chlorine with calcium hydroxide is: Ca ( OH ) 2 + Cl 2 → CaOCl 2 + H 2 O