7. Balance the following reactions and identify the species that have been oxidized and the species...
For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. For each reaction below, balance the following reactions and indicate the species that has been oxidized and the species that has been reduced: Copy and paste the table below, to complete the chart. Reaction Species Oxidized Species Reduced Cl2 (g) + (aq) → 12 (s) + Cl(aq)...
3. Balance the following reactions and identify the species that have been oxidized and the species that have been reduced: Clz (g) + l'(aq) → 12 (s) + Cl(aq): - Al (s) + O2(g) → Al2O3 (s): -- 3/3 Ca (s) + H20 (1) ► H2 (9) + Ca (OH)2 (s): --- WO2 (s) + Hz (g) → W (s) + H2O (): -
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
4. (6 pts.) Oxidation-Reduction Reactions: write out two ways you can identify the species that has been oxidized in a redox reaction: b. Identify the element reduced and the element oxidized in the following oxidation- reduction reactions. Fe(s) + CuCl2(aq) FeCl2(aq) + Cu(s) Element Oxidized: Element Reduced: C(s) + O2(g) → C02(g) Element Oxidized: Element Reduced:
1. Identify the anode, the cathode, the reduced species and the oxidized species for the following electrochemical cells. Write the half reactions for the anode and cathode, the overall reaction. Calculate the total cell potential. a) Fe (8)| Fe (aq) (0.2 M) || Ni” (aq) (0.1 M) | Ni(s) b) Zn (s) | Zn? (aq) (1.0 x 10' M)||Cl(aq)(0.3 M) CI, (g) (0.100 bar) Pt (S) c) Pb (s) Pb2(aq) (1.0 x 10ʻM) || Cu (aq) (1.0 x 10M) Cu...
Identify the species oxidized, the species reduced, the oxidizing agent and the reducing agent in the following electron-transfer reaction. Mg(s) + 12(s) —— Mg2+(aq) + 21"(aq) species oxidized species reduced oxidizing agent reducing agent As the reaction proceeds, electrons are transferred from
Balance the equation and identify the species being oxidized and reduced. ___ Na (s) + __-H20 (1) ►_NaOH (aq) + _H2 (g)
For the following reactions, determine the species being oxidized or reduced, the balanced half reactions, and the balanced equation. Al(s)+Cu^2+(aq) -> Al^3+(aq)+CU(s)
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
Identify whether the reaction is a redox reaction. If it is, determine which species is oxidized and which is reduced. 2Fe^3+(aq) + 3S^2- (aq) rightarrow Fe_2S_3(s) 2FeCl_3(aq) + 3Co(s) rightarrow 2Fe(s) + 3CoCl_2(aq) 2NH_4Cl(aq) + F_2(g) rightarrow 2NH_4F(aq) + Cl_2(aq) H^+(aq) + OH^-(aq) rightarrow H_2O(I) 2HNO_3(aq) + Zn(s) rightarrow Zn(NO3)2(aq) + H_2(g) 2H_2O(I) + 2K(s) rightarrow 2KOH(aq) + H_2(g) 2.