Increases QUESTION 34 In the reaction: Mn (s) + Cu2+ (aq) --> Mn2+ (aq) + Cu...
QUESTION 4 In the following reaction, Mg(s) + + Cu2+ (aq) → Mg2+ *(aq) + Cu(3) Mg is the reducing agent and Cu is the oxidizing agent. O Cu is the reducing agent and Mg2+ is the oxidizing agent. Mg2+ is the reducing agent and Cu is the oxidizing agent. O Mg is the reducing agent and Cu2+ is the oxidizing agent. is the reducing agent and Mg is the oxidizing agent. O QUESTION 5 Which of the following diatomic...
Identify the oxidizing agent in the following redox reaction. Hg2+(aq) + Cu(s) --- ---->> Cu2+(aq) + Hg(1)
Consider the redox reaction Fe(s) + Cu2+ (aq) — Fe2+(aq) + Cu(s) Which substance gets oxidized? Which substance gets reduced? What is the reducing agent? What is the oxidizing agent?
A. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Sn2+(aq) + 2e-Sn(s) -0.140V Cr3+(aq) + 3e-Cr(s) -0.740V (1) The strongest oxidizing agent is: enter formula (2) The weakest oxidizing agent is: (3) The weakest reducing agent is: (4) The strongest reducing agent is: (5) Will Cl2(g) oxidize Cr(s) to Cr3+(aq)? (6) Which species can be oxidized by Sn2+(aq)? If none, leave box blank. B. Half-reaction E° (V) Cl2(g) + 2e-2Cl-(aq) 1.360V Cu2+(aq) + 2e-Cu(s) 0.337V Mn2+(aq) + 2e-Mn(s) -1.180V (1) The...
a Cu(s) + 2Ag+ (aq) → 2 Ag(s) + Cu2+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced b HCl(g) + NH3 (g) → NH4Cl(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced c SiCl4 (l) + 2H2O(l) → 4HCl(aq) + SiO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d C14 (1) + 2Mg(s) + 2MgCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced e Al(OH)4-(aq) → AIO2- (aq) + 2H2O(l) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced
Cu(s) + 4HNO3 --> Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Cu2+(aq) + 4NH3(aq) --> [Cu(NH3)4]2+(aq) a. For each reaction, identify the oxidation number for each of the elements on both sides of the equation. b. Which of the reactions above is a redox reaction? Explain. c. Identify the element that is being reduced and the one that is being oxidized in the redox reaction. d. Identify the strong oxidizing agent and strong reducing agent in the redox reaction.
Calculate the E°cell for the following reaction: Cu2+ (aq) + Ni (s) → Cu (s) + Ni2+ (aq) A) (-0.59 ± 0.01) V B) (-0.09 ± 0.01) V C) (0.59 ± 0.01) V D) (0.09 ± 0.01) V --------------------------------------------------------------------------------------------------------- What is the proper line notation for the following reaction? Cu (s) + 2Ag+ (aq) → Cu2+ (aq) + 2Ag (s) A) Cu2+ | Cu || Ag | Ag+ B) Ag+ | Ag || Cu | Cu2+ C) Cu |...
Question 3 For the balanced redox reaction: 3 Mn2+ (aq) + 2Al(s) →3 Mn(s) + 2 A13+ (aq) Use your previous answer to calculate Key A. 2.6 x 1034 B.5.3 x 1048 C.4.7 x 1034 D. 1.2 x 1052 E. 1.9 x 1012 ОА OB Ос OD e here to search O - FY F4 F5 F6 F7 F8 FO @ # % For the balanced redox reaction: 3 Mn2+ (aq) + 2Al(s) +3 Mn(s) + 2 A13+ (aq) Use...
Using the activity series, select all REDOX REACTIONS that should occur A) Mn(s) + Ni2+(aq) --> Ni(s) + Mn2 (aq) B) 2Ag(s)+ Fe2+(aq) --> Fe(s) + 2Ag (aq) C) Ni(s) + Mn2t(aq) --> Mn(s) + Ni2 (aq) D) Sn(s) + Fe2+(aq) --> Fe(s) + Sn2 (aq) E) Zn(s) + Cu2 (aq)-> Cu(s) + Zn2 (aq) F) Fe(s)+Sn2 (aq) --> Sn(s) + Fe2 (aq)
Consider the following half-reactions: Half-reaction F2(g) + 2e - 2H+ (aq) + 2 Mn2+ (aq) + 2e E° (V) 2F (aq) 2.870V H2(g) 0.000V Mn(s) -1.180V The strongest oxidizing agent is: enter formula / / The weakest oxidizing agent is: / The weakest reducing agent is: The strongest reducing agent is: Will Mn2+ (aq) reduce F2(g) to F"(aq)? Which species can be reduced by H2(g)? If none, leave box blank. Consider the following half-reactions: Half-reaction E° (V) Br2(1) + 2e...