Related InterviewSolutions

• The reaction of white phosphorus with aqueous `NaOH` gives phosphine along with another phosphorus containing compound. The reacation type, the oxidation states of phosphorus in phosphine and the other product are respectvely:A. redox reaction, -3 and -5B. redox reaction, +3 and +5C. disproportion reaction, -4 and +5D. disproportion reaction, -3 and +5
• Explain why `HNO_(3)` acts only as oxidising agent while `HNO_(2)` can act both as a reducing agent and an oxiding agent?
• Which ordering of Compounds is according to the decreasing order of the oxidation state of nitrogen?A. `HNO_(3), NO,NH_(4)Cl,N_(2)`B. `HNO_(3), NO,N_(2),NH_(4)Cl`C. `HNO_(3),NH_(4)Cl,NO,N_(2)`D. `NO,HNO_(3),NH_(4)Cl,N_(2)`
• The oxidation number of nitrogen atom in `NH_(4)NO_(3)` are:A. `+3,+3`B. `+3,-3`C. `-3,+5`D. `-5,+3`
• Balance the following equation by oxidation number method `NaIO_(3)+NaHSO_(3)to Na_(2)SO_(4)+NaHSO_(4)+I_(2)+H_(2)O`
• The oxidation state of iodine in `IPO_(4)` isA. `+1`B. `+3`C. `+5`D. `+7`
• Arrange the following in the order of (a) Increasing oxidation number of iodine. `I_(2), HI, HIO_(4),ICI` (b) Increasing oxidation number of cholorine `Cl_(2)O_(7),Cl_(2)O,HCl,CIF_(3),Cl_(2)` (c ) increasing oxidation number of nitrogen. `NH_(3),N_(3)H,N_(2)O,NO,N_(2)O_(5)`
• In alkaline medium `CIO_(2)` oxidises to `H_(2)O_(2)` and `O_(2)` and itself gets reduced to `Cl^(-)`. How many moles of `H_(2)O_(2)` are oxidised by 1 mole of `ClO_(2)`? Hint: The balanced chemical equation is:A. 1B. 1.5C. 2.5D. 3.5
• Calculate the oxidation state of underlined (a) `Ba_(2)XeO_(2)` (b). `BaCl_(2)` (c ).`C_(12)H_(22)O_(11)` (d) `IF_(7)` (e ) `Na[Fe(CN)_(5)NO]` (f) `RuO_(4)` (g) `K_(2)TaF_(7)` (h) `Na_(2)MO_(4)` `U_(2)O_(7)^(4-)` (j) C is diamond.
• Write the following ionic equation in the molecular form if the reactants are chlorides. `2Fe^(3+)+Sn^(2+) to 2Fe^(2+)+Sn^(4+)`