Determine the oxidation numbers of each of the elements in the following reaction, and identify which,...
See page 181 11 Question (1 point) Determine the oxidation numbers of each of the elements in the following reaction, and identify which of them, if any, are oxidized or reduced. 3NO2(s)+H,0() 2H (aq) +2NO, (aq) +NO(g) 1st attempt See Periodic Table Q See Hint Part 1 (0.2 point) NO2 N: O: Q See Hint Part 2 (0.2 point) Part 2 (0.2 point) O See Hint Но Н: O: Part 3 (0.1 point) Q See Hint H* H: Part 4...
What is the sum of the oxidation numbers of the atoms in each of the following polyatomic ions? 1st attempt Part 1 (1 point) OH- Choose one: +1 Oo 0 -1 Part 2 (1 point) NH4 Choose one: +1 oo O-1 Part 3 (1 point) SO42- Choose one: O +2 Oo 0 -2 Part 4 (1 point) PO43- Choose one: ООО
For the following reaction, (1) assign oxidation numbers for all the elements, (2) determine which one is oxidized and which one is reduced, and (3) balance the redox reaction in acidic solution. SO32–(aq) + MnO4–(aq) ® SO42–(aq) + Mn2+(aq)
The reaction of Cr2O3 with silicon metal at high temperatures will make chromium metal. $$ The reaction is begun with 134.00 g of Si and 130.00 g of Cr2O3. The reaction of Cr2O3 with silicon metal at high temperatures will make chromium metal. 2Cr203 (s) + 3Si(s) —— 4Cr(1) +3510,(s) The reaction is begun with 134.00 g of Si and 130.00 g of Cr2O3. 1st attempt Part 1 (1 point) I See Periodic Table Select the limiting reactant. Choose one...
Write the oxidation numbers UNDER all the elements in the following oxidation-reduction reaction: 5NaBiO3(s) + 2 MnCl2(aq) + 16HCl(aq) 5NaCl(aq) + 5BiCl3(aq) + 2HMnO4(aq)+7H2O(l) Identify the element being oxidized and reduced.
For each of the following balanced redox reactions, identify which elements get oxidized and reduced. Also, ldentify the oxidant and the reductant. 1) 2Cr20 (aq)+3CH,OH(aq) 16H (aq) 3HCO,H(aq)+4Cr(aq)+ 11H20 (1) 2) 2NO -(aq) + H2S(g) + 2H+(aq) →2NO2(g) + S(g) +2H2O (l)
1. Provide the oxidation number for each of the underlined elements in following compounds or ions: (6) a) H3AsO3 b) d) H4P207 C202² KCIO4 N2H4 2. Which one of the following is not a oxidation-reduction reaction? (2) A) 2H2(g) + O2(g) → 2H2O(1) B) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) C) H2O(l) + NH3(g) → NH(aq) + OH(aq) D) FeSO4(aq) + K2Cr2OH(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(1) E) Cl2(g) +2KBr(aq) + Bra(l) + 2KCl(aq)...
Enter the oxidation number of one atom of each element in each reactant and product. CH,(8) +20,() — CO2(g) + 2H,0(8) Cin CH : Hin CH :| O in : Cin CO2: o inco, H in H,O: O in H, 0: Which atom is reduced? Which atom is oxidized? Oo OH 00 OH oc oc
For the reaction KCIO4 →KCI+20, assign oxidation numbers to each element on each side of the equation. Kin KCIO, K in KCl: Cl in KCIO, Cl in KCl: O in KCIO, O in 0, Which element is oxidized? Which element is reduced? OK OK Ос oo oo
for the reaction in question 5, list those elements which have changed oxidation number during the reaction, showing the oxidation number before and after the reaction. Which element is oxidized? Which is reduced? Which is the oxidizing agent? Which is the reducing agent? How many electrons are transferred per sulfur atom? How many totally in the reaction as shown? 5. Balance the following equation: Cl2 + K2S2O3 + KOH KCI + K2SO4 + H20