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What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq)...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+(aq) — 2CH(aq) + 2Fe3+(aq) O Fe2+ O Cl2 OCH O Fe3+
Consider the following cell diagram: Pt(s) | Fe3+(aq) , Fe2+(aq) || Cl–(aq) | Cl2(g) | Pt(s) The reaction utilized by this cell is Question 8 options: Fe2+(aq) + 2Cl–(aq) --> Fe(s) + Cl2(g) Fe(s) + Cl2(g) --> Fe2+(aq) + 2Cl–(aq) 2Fe3+(aq) + 2Cl–(aq) --> 2Fe2+(aq) + Cl2(g) Fe3+(aq) + Cl–(aq) --> Fe2+(aq) + 1/2Cl2(g) 2Fe2+(aq) + Cl2(g) --> 2Fe3+(aq) + 2Cl–(aq)
Given the cell reaction: 2Cl–(aq) + Fe3+(aq) → Cl2(aq) + Fe2+(aq): (unbalanced) a) As written, is the cell galvanic or electrolytic? b) Calculate ε°cell. c) Calculate ΔG°.
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers to each, and write balanced net ionic equations. a) Cu(s) Cu2+(aq) + 2e- b) Cl2(aq) + 2e- Cl-(aq) c) Cu(s) + Cl2(aq) Cu2+(aq) + 2Cl-(aq) d) 4CuO(s) + CH4(g) 4Cu(s) + CO2(g) + 2H2O(l) e) 2CuSO4(aq) + 4KI(aq) 2CuI (aq) + 2K2SO4(aq) + I2(aq) f) Cu2O(s) + Fe(SO4)3 (aq) + H2SO4(aq) 2CuSO4(aq) + 2FeSO4(aq) + H2O(l)
1. For the following electron-transfer reaction: Cl2(g) + Hg(l) 2Cl-(aq) + Hg2+(aq) The oxidation half-reaction is: (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g) The reduction half-reaction is: (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g) 2. For the following electron-transfer reaction: 3Br2(l) + 2Al(s) 6Br-(aq) + 2Al3+(aq) The oxidation half-reaction is: (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g) The reduction half-reaction is: (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g)
Choose the correct QUESTION 19 According to the following cell notation, the species that is undergoing oxidation is answer from the options below (a through e). Zn(s) Zn2+ (aq) || Mn2+(aq)|MnO2(3)| Pt() a. Mn2+ (aq) b. Zn2+ (aq) c. MnO2(3) d. Zn(s) e. Pt(s) Choose the correct answer from the In the following electrochemical cell, the cathode half reaction is options below (a through e). Mn(s) Mn2+ (aq) || Fe3+ (aq), F ), Fe2+ (aq)| Pt() 4. Fe3+(aq) + 6...
A voltaic cell utilizes the following reaction: 2Fe3+(aq)+H2(g)→2Fe2+(aq)+2H+(aq). emf of this cell under standard conditions E∘ = 0.771 V What is the emf for this cell when [Fe3+]= 3.70 M , PH2= 0.95 atm , [Fe2+]= 1.0×10−3 M , and the pH in both compartments is 3.95? Express your answer using two significant figures.
Assign the correct oxidation number to each species in the redox reaction below. PbSO4(s) + H*(aq) + 2Cl(aq) = Pb(s) + H$04" (aq) + Cl2(g)
2Fe3+ (aq) + 2I-(aq) → 2Fe2+ (aq) + I2(aq) What would be the cathode in this reaction? Question options: a. Fe3+ (aq) b. Fe2+ (aq) c. I2(aq) d. I-(aq)
What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2O2 (g) -> CO2(g) + 2H2O (g) 1. H 2. O 3. C