In each of the following reactions, identify which el- ement(s) are being oxidized and which are...
4. In each of the following reactions, identify the elements being oxidized or reduced, a) 4 Fe (s) + 3 O2(g) 2 FeO3 (5) (Oxygen is in its natural state.) Element being oxidized: Element being reduced: b) CuCl2 (aq) + Zn (s) → ZnCl2 (aq) + Cu (s) (Zinc and Copper are in their natural states.) Element being oxidized: Element being reduced: 21
a In the following reaction, identify which element is oxidized and which is reduced by assigning oxidation numbers: Ba(s)S(s)BaS (s) barium is reduced; sulfur is reduced barium is reduced; sulfur is oxidized barium is oxidized; sulfur is oxidized barium is oxidized; sulfur is reduced Submit b In the following reaction, identify which element is oxidized and which is reduced by assigning oxidation number 2Sr(s)02(g)> 2SrO(s) strontium is reduced; oxygen is reduced strontium is oxidized; oxygen is reduced strontium is oxidized;...
Identify which element is being reduced and oxidized in the following reaction. (For full credit, please give the oxidation states of each clement or ion below.) 4 Fe (s) + 3 O_2(g) rightarrow 2Fe_2Q_3 (s)
1. Identify the species being oxidized and reduced in each of the following reactions, and determine the number of electrons (in mol) involved in the reaction: a. Crt + Sn4+ -> Cr3+ + Sn2+ b. 3 Hg2+ + 2 Fe (s) -> 3 Hg2+ 2 Fe3+ c. 2 As (s) + 3 Cl2 (8) 2 AsCl3
3. In the following reactions, identify which of the elements are oxidized and which are reduced and enter the name of the element on the line. (3 points for each equation, 9 points total) a. 2Ca(s) + O2(g) - Cal is oxidized is reduced b. MnO2 (aq) + 4 HBr(aq) -Bra(l) + MnBr2 (aq) + 2 H2O(0) is oxidized is reduced C. Cl2(g) +2 NaBr(ag) 2NaCl(aq) + Br2 () (Here Cl is chlorine) is oxidized is reduced
In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: (its multiple choice) Number 1: Br2(g)+2KI(aq)→2KBr(aq)+I2(s) I− (in KI) loses electrons and is oxidized. Br2 gains electrons and is reduced. Br2 gains electrons and is oxidized. I− (in KI) loses electrons and is reduced. I− (in KI) gains electrons and is oxidized. Br2 loses electrons and is reduced. Br2 loses electrons and is oxidized. I− (in KI) gains electrons and is reduced....
Identify which substance is reduced and which is oxidized in each of the following reactions. (aq)3 Mg? (aq) + 2 Au (s) 2. 3 Mg (s)+ 2 Au a. 2 Na (s)+ 2 H2O (I)->2 NaOH (aq) + H2 (g) b.
Please, in the following reactions, show Half Reactions to decide which reactant is oxidized and which is reduced. Designate the oxidizing agent and reducing agent. Assign oxidation numbers to each atom. 1.a) Si (s) + 2Cl2 (g) ----> SiCl4 (l) 1.b) C2H4 (g) + 3O2 (g) ----> 2CO2 (g) + 2H2O (l) Thank You!
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)
Problem 2: Below are several chemical equations. For each equation, identify which atoms are oxidized and which atoms are reduced. It is possible to have a type of atom that is both oxidized and reduced in the same chemical process. (How? Assign oxidation numbers to each element on both sides of the equation. If the number goes up, the atom is oxidized. If the number goes down, it's reduced.) a. N2(g) + 2 O2(g) → 2 NO2(g) b. CH4(g) +...