Consider the following redox reaction ((Cr2O7)2-) + (14H+) + (6I-) --> 2(Cr3+) + 3(I2) + 7(H2O) write the falf cell reactions at the cathode and anode
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Consider the following
((Cr2O7)2-) + (14H+) + (6I-) --> 2(Cr3+) + 3(I2) + 7(H2O)
write the falf cell reactions at the cathode and anode
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- ▼ Part B 2NO3(aq) +8H(aq) + 6e 3Fe(s) + 2NO3 (aq) +8H+ (aq) 3Fe(s)→→3Fe²+ (aq) + 6e →>> 2NO(g) + 4H₂0 (1) →3Fe²+ (aq) + 2NO(g) + 4H₂O(1) IVE ΑΣΦ Calculate El using the tabulated standard electrode potentials at 25 °C. cell Express your answer in volts to three significant figures. Eeell= 1.21 SWE Submit Previous Answers Request Answer 2+ X Incorrect; Try Again; 4 attempts remaining ? V stontiol buoubtrooting the electro na- Which one of the following is the correct net ionic equation for the reaction that occurs when solutions of Pb(NO3)2 and Kl are mixed?(a) NO₂(g) + N₂O(g) → 3NO(g) [NO]³ [NO₂] + [N₂O] O [NO₂] + [N₂O] [NO]³ [NO₂][N₂0] [NO]³ [NO]³ [NO₂][N₂O] (b) CaSO3(s) CaO(s) + SO₂(g) O [SO₂] [CaSO3] [CaO] + [SO] 1 [SO₂] [CaSO3] [CaO][SO] © [CaO][SO_] [CaSO3] O [CaO] + [SO] [CaSO3] (c) NICO3(s) Ni²+ (aq) + CO²(aq) O [Ni²+][co] [NiCO3] [NiCO3] [Ni²+ ][co] O [Ni²+] + [Co-] [NiCO3] [NiCO3] [Ni²+] + [co] O [Ni²+ ][co] O 2+ [Ni²+ ][co]
- L z OH 1 + ) 2,₁Ag+KNO3A certain half-reaction has a standard reduction potential E =-1.25 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 0.80 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. h Data Ag+ (aq) + e Ag (s) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a minimum. Ered = v !! Al3+ (aq) + 3e-- Al (s) -1.676 Au+ (aq) + e Au (s) 1.692 If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. Au3+ (aq) + 3e - Au (s) 1.498 O no minimum Ba2+ (ag) + 2e - Ba (s) -2.912 Brz (1) + 2e- 2Br (aq) 1.066 Ca2+ (ag) + 2e - Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? E=…Please answer questions 4a, 4b, and 4c. The questions are provided in the attached image. Thank you.9) C 10) A Please explain why these are the correct answers(a) 2N,0(g) 2N,(g) + 0,(8) (b) 6Li(s) + N2(g) (c) Ni(s) + Pb(NO3)2(aq) → 2Lİ;N(s) → Pb(s) + Ni(NO3)2(aq) → HNO,(aq) + HNO;(aq) (d) 2NO,(g) + H,0() 2. For the redox reactions above, indicate the changes in the oxidation numbers of theelements.▼ Part A Calculate AHx for the following reaction: Use the following reactions and given AH values: AHxn C7H16 (1) +1102(g) → 7CO₂(g) +8H₂O(g), -> C(s) + O2(g) → CO₂ (g), 2H₂(g) + O2(g) → 2H₂O(g), Express your answer to four significant figures in kilojoules. ▸ View Available Hint(s) VE ΑΣΦΑ Submit Previous Answers 7C(s) + 8H₂(g) → C₂H16 (1) Pearson Review I Constants I Periodic Table www ΔΗ ΔΗ ΔΗ kJ -4464.3 kJ -393.5 kJ -483.5 kJGiven (alfa)-Fe2O3 List all its: Structural properties Physical properties Chemical properties Optical properties Magnetic properties Electronic propertiesYou have a 11.5 mg sample of blood that contains various proteins. Hemoglobin is the only protein in the sample containing Fe. Hemoglobin contains 3.83% by mass of a compound called heme (C34H32FEN.O4, MW = 616.49 g/mol). You find that your 11.5 mg blood sample contains 10.9 micrograms of Fe. What is the mass percent of hemoglobin in your protein sample?SEE MORE QUESTIONS