Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I ) s u l f a t e ( a q ) c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I I ) s u l f a t e ( a q ) You place 87.7 mL of a 0.500- M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.
Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I ) s u l f a t e ( a q ) c o p p e r ( I I ) s u l f a t e ( a q ) + i r o n ( s ) → c o p p e r ( s ) + i r o n ( I I I ) s u l f a t e ( a q ) You place 87.7 mL of a 0.500- M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.
Solution Summary: The author explains the reaction that produces a better yield of copper by taking the products of molar mass of the compound to the given mass.
Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations.
c
o
p
p
e
r
(
I
I
)
s
u
l
f
a
t
e
(
a
q
)
+
i
r
o
n
(
s
)
→
c
o
p
p
e
r
(
s
)
+
i
r
o
n
(
I
I
)
s
u
l
f
a
t
e
(
a
q
)
c
o
p
p
e
r
(
I
I
)
s
u
l
f
a
t
e
(
a
q
)
+
i
r
o
n
(
s
)
→
c
o
p
p
e
r
(
s
)
+
i
r
o
n
(
I
I
I
)
s
u
l
f
a
t
e
(
a
q
)
You place 87.7 mL of a 0.500-M solution of copper(II) sulfate in a beaker. You then add 2.00 g of iron filings tu the copper(II) sulfate solution. After one of the above reactions occurs, you isolate 2.27 g of copper. Which equation above describes the reaction that occurred? Support your answer.
My question is whether HI adds to both double bonds, and if it doesn't, why not?
Strain Energy for Alkanes
Interaction / Compound kJ/mol kcal/mol
H: H eclipsing
4.0
1.0
H: CH3 eclipsing
5.8
1.4
CH3 CH3 eclipsing
11.0
2.6
gauche butane
3.8
0.9
cyclopropane
115
27.5
cyclobutane
110
26.3
cyclopentane
26.0
6.2
cycloheptane
26.2
6.3
cyclooctane
40.5
9.7
(Calculate your answer to the nearest 0.1 energy unit, and be sure to specify units, kJ/mol or kcal/mol. The answer is case
sensitive.)
H.
H
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A certain half-reaction has a standard reduction potential Ered +1.26 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that
must provide at least 1.10 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 anode of the cell.
Is there a minimum standard reduction
potential that the half-reaction used at
the cathode of this cell can have?
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..
Is there a maximum standard reduction
potential that the half-reaction used at
the cathode of this cell can have?
If so, check the "yes" box and calculate
the maximum. Round your answer to 2
decimal places. If there is no upper
limit, check the "no" box.
yes, there is a minimum.
1
red
Πν
no minimum
Oyes, there is a maximum.
0
E
red
Dv
By using the information in the ALEKS…
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