An oxide of iodine(I=127) contains 25.4g of iodine for 8g of oxygen. Its formula could be:

(A)` I_2O_3`
(B)` I_2O`
(C)` I_2O_5`
(D)` I_2O_7`

I cc N_(2)O at NTP contains

XO+I_(2)O_(5)(s) to CO_(2)+I_(2)

CO+I_(2)O_(5)(s) to CO_(2)+I_(2)

5 mL solution of H_2O_2 liberates 1.27 g of iodine from an acidified KI solution. What is the molarity of H_2O_2 ?

What weight of HNO_(3) is needed to convert 5g of iodine into iodic acid according to the reaction, I_(2)+HNO_(3)rarrHIO_(3)+NO_(2)+H_(2)O

10 " mL of " H_2O_2 liberates 12.7 g of iodine form an acidic KI solution. Calculate the normality

Which of the following has the greatest affinity for water: P_(4)O_(10). Cl_(2)O_(7),I_(2)O_(5) .

12. g of an impure sample of arsenious oxide was dissolved in water containing 7.5 g of sodium bicarbonate and the resulting solution was diluted to 250 mL . 25 mL of this solution was completely oxidised by 22.4 mL of a solution of iodine. 25 mL of this iodine solution reacted with same volume of a solution containing 24.8 g of sodium thiosulphate (Na_(2)S_(2)O_(3).5H_(2)O) in one litre. Calculate teh percentage of arsenious oxide in the sample ( Atomic mass of As=74 )

Na_(2)S_(2)O_(3) is oxidized by I_(2) to give

A 5.0 mL solution of H_(2)O_(2) liberates 1.27 g of iodine from an acidified KI solution. The percentage strenth of H_(2)O_(2) is