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Question 22 (5 points) Given the following half reactions: PbO2 + 4H+ + SO42- + 2e...
Question 20 (5 points) Using the following standard reduction potentials: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = +1.69 V PbO2 + 4H+ + 2e → Pb2+ + 2H20 E° = +1.46 V The standard cell voltage for the reaction PbSO4(s) Pb2+ + SO42- is V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.
Question 20 (5 points) Using the following standard reduction potentials: PbO2 + 4H+ + SO42- + 2e → PbSO4(s) + 2H20 E° = +1.69 V PbO2 + 4H+ + 2e Pb2+ + 2H20 E° = +1.46 V is The standard cell voltage for the reaction PbSO4(s) → Pb2+ + SO42- V. Please enter your answer in decimal form, such as 2.5, and keep the correct number of significant figures.
Question 22 (5 points) Given the following half reactions: - AgBr(s) + e- Ag+ (aq) + e- Ag(s) + Br- (aq) E° = 0.07V → Ag (s) E° = 0.80V - Calculate the Ksp for PbSO4 at 25 degrees C. Please enter your answer in scientific notation, such as 1.2E10 or 1.2E-10 and keep two significant figures.
You want to make a battery using the following reactions: PbO2 + 4H+ + SO42- + 2e ---> PbSO4(s) + 2H20 Ni2+ + 2e ---> Ni ° = +1.69 E° = -0.25 Which is being reduced? Which is being oxidized? Which is the anode? Which is the cathode? What is the formula to calculate Eºcell? What is Eºcell?
5. A lead storage battery involves the following two half-reactions: PbSO4(s) + 2e → Pb(s) + SO42- (aq); E = -0.36 V PbO2(s) + 4H*(aq) + SO42 (aq) + 2e → PbSO4(s) + 2H2O(1); E° = 1.69 V In the lead battery during the discharge reaction: A) PbSO4 is the cathode. B) PbSO4 is the anode. C) Pb is the anode. D) PbO, is the anode. E) H2SO4 is the cathode.
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
Given the following standard half-cell potentials: MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l) E° = 1.23 V NO3 – (aq) + 4H+ (aq) + 3e– → NO(g) + 2H2O(l) E° = 0.96 V N2(g) + 5H+ (aq) + 4e– → N2H5 + (aq) E° = –0.23 V Which of the following reactions is nonspontaneous under standard state conditions?
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.26 M )+2e- Red: MnO-4(aq, 1.50 M )+4H+(aq, 2.7 M )+3e-→MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C.
An electrochemical cell is based on the following two half-reactions: Ox: Pb(s)→Pb2+(aq, 0.18 M )+2e− Red: MnO−4(aq, 1.65 M )+4H+(aq, 1.9 M )+3e−→ MnO2(s)+2H2O(l) Compute the cell potential at 25 ∘C.