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Question
Consider the following half-reactions:
Ag+(aq) + e- Ag(s) E = +0.80 V
Cu2+(aq) + 2 e- Cu(s) E = +0.34 V
Pb2+(aq) + 2 e- Pb(s) E = -0.13 V
Fe2+(aq) + 2 e- Fe(s) E = -0.44 V
Al3+(aq) + 3 e- Al(s) E = -1.66 V
Which of the above metals or metal ions will oxidize Pb(s)?
A.Ag+(aq) and Cu2+(aq)
B.Ag(s) and Cu(s)
C.Fe2+(aq) and Al3+(aq)
D.Fe(s) and Al(s)
E.Cu2+(aq) and Fe2+(aq)
Answer
This answer is hidden. It contains 2 characters.
Related questions
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A.
B.
C.
D.
E.
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B.
C.
D.
E.
Q:
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Q:
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Q:
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Q:
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Q:
What is the half-life of a first-order reaction if it takes 4.4 10-2 seconds for the concentration to decrease from 0.50 M to 0.20 M?A.2.5 10-2 sB.3.3 10-2 sC.1.6 sD.21 sE.27 s
Q:
Hydrogen peroxide decomposes into water and oxygen in a first-order process.
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Q:
A student analyzed a first-order reaction and obtained the graph below. Unfortunately, the student forgot to label the axes. What are the correct labels for the x and y axes? A.x axis = time, y axis = ln[A]
B.x axis = ln[time], y axis = [A]
C.x axis = ln[time], y axis = [A]
D.x axis = time, y axis = 1/[A]
E.x axis = 1/time, y axis = 1/[A]