Question
Which of the following is a set of reducing agents? (A) HNO_(3),Fe^(2+),F_(2) (B) F,Cl^(-).MnO_(4)^(-) (C) I^(-),Na,Fe^(2+) (D) CrO_(7)^(2-)*CrO_(4)^(2-),Na . Which of the following is a redox reaction ? (A) 2CuSO_(4)+4KIlongrightarrowCu_(2)I_(2)+2K_(2)SO_(4)+I_(2) (B) SO_(2)+H_(2)OlongrightarrowH_(2)SO_(3) (C) Na_(2)SO_(4)+BaCl_(2)longrightarrowBaSO_(4)+2NaCl (D) CuSO_(4)+4NH_(3)longrightarrow[Cu(NH_(3))_(4)]SO_(4) (E) C_(12)H_(22)O_(I1)+H_(2)OlongrightarrowC_(6)H_(12)O_(6)+C_(6)H_(12)O_(6) Oxidation number of iodine in IO_(3)^(-),IO_(4)^(-),KI and I_(2) respectively are (A) -1,-1,0,+1 (B) +3,+5,+7,0 (C) +5,+7,-1,0 (D) -1,-5,-1,0 (E) -2,-5,-1,0 .
Answer
4.5
(391 Votes)
Arnold
Professional · Tutor for 6 years
Answer
1.C 2.A 3.C
Explanation
1. A reducing agent is a substance that loses electrons, causing the other substance in the reaction to be reduced. In the given options, I-, Na, and Fe2+ (option C) are known to act as reducing agents.2. A redox reaction is a type of chemical reaction that involves a transfer of electrons between two species. The reaction 2CuSO4+4KI -> Cu2I2+2 K2SO4+I2 (option A) is a redox reaction because there is a change in oxidation state of the elements involved.3. The oxidation number of iodine in IO3-, IO4-, KI, and I2 are +5, +7, -1, and 0 respectively (option C). This is determined by the rules for assigning oxidation numbers to atoms in a molecule or ion.