CHE112 Problem Set 10 Solutions
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CHE112 –
Physical Chemistry Winter 2024 Tutorial 11: Problem Set 10 (Redox Reactions and Electrochemistry) Review from High School: 1.
Determine the oxidation state of each element in the following compounds:
F
2
[answer: F = 0]
HCl [answer: H = +1, Cl = -1]
HBrO [answer: H = +1, O = -2, Br = +1]
SiC [answer: Si = +4, C = -4]
CaC
2
[answer: Ca = +2, C = -2]
FeN [answer: N = -3, Fe = +3] 2.
The Energizer battery is an alkaline zinc-magnesium dioxide cell. The overall cell reaction can be represented as: Zn (s)+ 2MnO2 (s)
ZnO (s) + Mn2O3 (s) What is the oxidation half-reaction at the anode and the reduction half-reaction at the cathode? Solution:
3.
Aluminum metal displaces zinc (II) ion from aqueous solution. Answer the following: a)
Write out the oxidation and reduction half-reactions and an overall equation for this redox reaction. b)
Write a cell diagram for a voltaic cell in which this reaction occurs. Solution: a)
Oxidation: 2 {Al(s)
Al
3+
(aq) + 3 e
-
} Reduction: 3 { Zn
2+
(aq) + 2 e
-
Zn(s)} Overall: 2 Al (s) + 3 Zn
2+
(aq)
2 Al
3+
(aq) + 3 Zn(s) b)
Al(s) is oxidized to Al
3+
(aq) in the anode half-cell (left) and Zn
2+
(aq) is reduced to Zn(s) in the cathode half-cell (right) Al(s) ǀ
Al
3+
(aq) ǁ
Zn
2+
(aq) ǀ
Zn(s) Calculation Questions: 4.
A battery system currently under study for possible use in electric vehicles is the zinc-chlorine battery. The overall reaction producing electricity in this cell is Zn (s) + Cl
2
(g)
ZnCl
2
. What is the E
o
cell
for this voltaic cell? (a
nswer: 2.121 V *note: answer may vary depending on table used
) Solution: Reduction: Cl
2
(g) + 2 e
-
2 Cl
-
(aq) Oxidation: Zn (s)
Zn
2+
(aq) + 2e
-
Overall: Zn(s) + Cl
2
(g)
Zn
2+
(aq) + 2Cl
-
(aq) E
o
cell
= E
o
(reduction half cell) –
E
o
(oxidation half cell) = 1.358 V –
(-0.738 V) = 2.121 V
Calculate E° for the reaction 2Na + 3S ⇌
Na
2
S
3
(answer: 2.00V) * Solution:
5.
Determine the standard cell potential E
cell
o
, the standard Gibbs free energy change
G
o
and the equilibrium constant for the following reaction at 25 o
C. (answer: 1.85 x 10
4
) *** The standard potential for Pb
2+
(aq) is -0.1262. (answer: E
cell
o
= +0.1262V,
G
o
= -24.35 kJ/mol, K = 1.85 x 10
4
) Solution:
Inspection of the cell reaction indicates that it comprises the following two half-reactions:
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Related Questions
Consider the following redox reaction:
Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g)
Which of the following statements are true? (Check all correct answers.)
Group of answer choices
The oxidation state of each Cl atom in FeCl2 is -2
Chlorine (Cl) is being reduced
Fe(s) is being oxidized
The oxidation state of iron in FeCl2 is +2
Hydrogen is being reduced
The oxidation state of hydrogen in H2(g) is +1
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Denitrification is an important biologically-mediated process by which nitrate is reduced. This is especially important in environments with excess inputs of nutrients. Denitrification is shown in the following (unbalanced) equation:
CH2O + NO3- + H+àH2O + N2 + CO2.
What are the oxidation states of each element in the equation? Write the number under the element in the equation.
Write the half reactions.
Label which half reaction shows oxidation and reduction.
Balance each half reaction.
Write is the full balanced equation.
Calculate the reduction potential DEo’.
Calculate the Gibbs free energy DGo’.
Will this reaction produce energy for bacterial growth?
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2. KMNO4 + NagC204 + H2SO4 K2SO4 + MNSO4 + NagSO4 + CO2+ H20
Balanced equation:
Oxidizing agent:
Reducing agent:
Criteria for each item
Solution following the 5-step process
Balanced equation
Oxidizing agent
Reducing agent
10 points
3 points
1 point
1 point
Total points or each item: 15points
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4. Consider the following redox equation (balanced)
32 H+ + 4
4 Cr₂0²
+ 3 S²- → 8 Cr³+ + 3 SO² + 16 H₂O
a.
b.
C.
Calculate the Molarity of a solution prepared by dissolving 0.624 g of Na2S in enough
water to give 250 mL of solution.
How many mL of this solution will be required to react with 0.512 g of Al2(Cr2O7)3?
Suppose that 24.86 mL of this Na2S solution was required to react with 0.377 g of a
dichromate salt. Which one of the following could be this salt?
Fe2(Cr2O7)3 CaCr2O7
PbCr2O7
BaCr2O7
Bi2(Cr2O7)3.
d. How many mL of the Na2S solution would be required to react with 50.00 mL of 0.300 M K2Cr2O7
solution?
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What is the oxidation number for each of the following elements?
(e.n.'s: C = 2.5, O = 3.5, H = 2.1)
1.
Co in Co (NO:)a
а.
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Consider the two-step process for the formation of tellurous acid described by the following equations:
???2+ 2??−⟶ ???3 2− + ?2? ???3 2− + 2?+⟶ ?2???3 What mass of H2TeO3 is formed from 74.2 g of TeO2, assuming 100% yield?
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50.00 grams of chromium (III) sulfate is dissolved in enough water to prepare 250.0 ml of solution. • What is the chemical formula for chromium (III) sulfate? • What is the molecular weight of chromium (III) sulfate grams per mole? • What is the concentration of chromium (III) sulfate in the solution above in moles per liter? • What is the concentration of Cr+3 ions in the solution above in moles per liter? Answer M • What is the concentration of SO4−2 ions in the solution above in moles per liter? • How many milliliters of the solution above are required to supply 0.100 moles of chromium (III) sulfate? • How many milliliters of the solution above are required to supply 0.275 moles of SO4−2 ions? • How many milliliters of the solution above are required to supply 0.120 moles of Cr+3 ions
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Which element in the compounds below has an oxidation number (state) of +2?
N in NH4Br
Ba in Ba(OH)2
Cr in CrO3
V in VO2+
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When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown?Cl- + NiO2 Ni(OH)2 + Cl2 Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is oxidized?
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Adding an oxidation state to each element in each reaction and use the change in oxidation state to determine which element is being oxidized and which is being reduced.
a) CH4(g) + 2H2S(g) = CS2(g) + 4 H2(g)
b) 2 H2S(g) = 2 H2(g) + S2(g)
c) C6H12O6(s) + 6 O2(g) = 6 CO2(g) + 6 H2O(g)
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Decide whether each chemical reaction in the table below is an oxidation-reduction ("redox") reaction. If the reaction is a redox reaction, write down the
formula of the reducing agent and the formula of the oxidizing agent.
redox reaction?
yes
no
2Na(s) + Cl, (8)
2NACI (s)
reducing
agent:
?
oxidizing
agent:
redox reaction?
yes
no
C(s) + 0, (g) → co,(g)
reducing
agent:
oxidizing
agent:
redox reaction?
yes
no
+
co, (g) + 2H,0(1) → H,0" (aq) + HCO,(aq)
reducing
agent:
oxidizing
agont:
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Use the rules (in order) to assign oxidation numbers to each of the elements in the compounds below.
bismuth hydroxide
H
Bi
O
Bi(OH)3
bromine trifluoride
Br
F
BrF3
periodic acid
H
I
O
HIO4
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Identify the oxidation numbers to all the elements in each of the compound or ions
H2SO3
O a.
H2 =+2; S=+2; O3 =-2
O b.
H2 =+1; S=+3; 03 =-2
H2 =+2; S=+4; O3 =-2
d.
H2 =+1; S=+4; O3 =-2
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Given the type of the reaction, complete and balance each of the following
reactions:
a)
b)
Na(s) + CuSO4(aq) →
- Single replacement.
K(s) + N₂(g) →
- combination.
Edit View Insert Format Tools Table
12pt ✓ Paragraph
BIU AT²V
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VII. Write the balanced chemical equation for the given reactions.
1. Fe(s) + Cl: –→ FeCl:(s)
2. N:(g) + H:(g) → NH:(g)
3. CeH.COOH(ag) + O:(g) → CO:(g) + H:O(I)
4. AGNO:(ag) + Cu(s) -
5. HCN(ag) + CUSO:(ag)
Cu(NO:)-(ag) + Ag(s)
H.SO:(ag) + Cu(CN)(ag)
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Combustion reactions (burning of fuels) are another example of redox. Coal is nearly pure carbon and has been burned as a fuel for centuries. The reaction of coal with oxygen in the air is illustrated by the balanced equation:
C + O2 → CO2
What is the change in oxidation state for the carbon in this reaction?
Group of answer choices
+2
-4
+4
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Rank the following according to oxidation number on chlorine. (#1 lowest)
HOCl, Cl2, AlCl3, ClO2
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What numbers belong in the
blank spaces to fully balance the
following reaction?
_ Fe (s) + Cl2 (g) → FeCl3
(s)
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Listen
What is the balanced chemical equation that represents the following reaction?
80
goo go
6H + 2N – 2HN3
->
O 2N + 2H3 - 2H3N
O 6H + 2N
· 2NH3
→
->
6H + 2N – 2N3H
3H2 + N2 - 2NH3
V Saved
Question 40 (1 point)
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G c3h6 m
G no2 mo
G nh3 mo
O Poelt
W Wordle
* Ground G co3 - G b Answer
G co2 mo
O Caffein
G molar
b Answer
Gk
Question 11 of 28
Complete the balanced molecular chemical equation for the reaction below.
If no reaction occurs, write NR after the reaction arrow.
K:SO:(aq) + FeCls(aq) →
12+ 3+ 4+
1
3
4
6.
7
8
9.
口2
Do
14
(s)
(1)
(g) (aq)
K
CI
NR
Fe
•x H2O
Delete
Reset
PgUp
PgDn
Home
F9
End
F10
F1
PrtScn
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For each of the reactions below, determine the initial and final oxidation states (OS) of each of the atoms as well as the
oxidizing and reducing agents.
a) Mg(s) + NiCl₂ (aq) → MgCl₂ (aq) + Ni (s)
->
Element
Mg
Ni
CI
Oxidizing Agent
1
OM O NiCly
Reducing Agent
O ME O NiCl₂
b) C₂H (g) + 30₂ (g) 2 CO₂ (g) + 2 H₂O(g)
Element
Initial OS
C
H
0
Oxidizing Agent
O Cylla O 0₂
Reducing Agent
Tab
Caps
Shift
Esc
!
1
Initial OS
A
@
2
21
Q
x
Z
F2
W
S
I
#
3
X
F3
E
D
L Q Search
»
$
4
Final OS
Final OS
F4
R
C
DII
TI
F
F5
%
5
T
V
*
G
F6
^
6
*
Y
B
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80°F
Sunny
The oxidation number of an element can vary.
O True
Search
F8
6725
F9
O False
- « Οι
F10
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Some chemical reactants are listed in the table below. Complete the table by filling in the oxidation state of the highlighted atom.
oxidation state of
highlighted atom
0
0
species
FeSO4(s)
VO(s)
Fe₂O3(s)
KMnO4(s)
X
0
0
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When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown?
NiO2 +
Sno,2- →
Ni(OH)2 +
Sno32-
(Enter 0
Water appears in the balanced equation as a
for neither.)
(reactant, product, neither) with a coefficient of
Which species is the reducing agent?
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ter 8: EOC
t
Calculate the number of grams of solute in each of the following solutions.
(a) 3.63 L of a 3.23 M HCI solution
(b) 36.3 mL of a 14.6 M HNO3 solution
(c) 37.3 mL of a 10.4 M AgNO3 solution
(d) 1.57 L of a 3.2x10-³ M Na₂SO4 solution
Submit Answer
Try Another Version
[References
grams of HCI
grams of HNO3
grams of AgNO3
grams of Na2SO4
5 item attempts remaining
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Would you use an oxidizing agent(OA) or reducing agent(RA)
in order for the following reactions to occur?
NH3 ==> NO2
Choose...
As
==> As+3
Choose...
MnO2
==> Mn2O3
Choose...
P205 ==> P4H10
Choose...
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When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown?Cl- + Br2ClO3- + Br-Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is reduced?
Part B:
When the following equation is balanced properly under basic conditions, what are the coefficients of the species shown? Cl- + I2 I- + Cl2Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is oxidized?
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Item 5
Write a balanced chemical equation for the reaction that occurs when Ca(s) reacts with Cl2(g)..
Express your answer as a balanced chemical equation including phases.
ΑΣΦΑ
Submit
A chemical reaction does not occur for this question.
Part B
Request Answer
Ć
ΑΣΦ
?
Write a balanced chemical equation for the reaction that occurs when calcium carbonate decomposes into calcium oxide and carbon dioxide gas
when heated.
Express your answer as a balanced chemical equation including phases.
*****
5 of 30
2
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- Consider the following redox reaction: Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g) Which of the following statements are true? (Check all correct answers.) Group of answer choices The oxidation state of each Cl atom in FeCl2 is -2 Chlorine (Cl) is being reduced Fe(s) is being oxidized The oxidation state of iron in FeCl2 is +2 Hydrogen is being reduced The oxidation state of hydrogen in H2(g) is +1arrow_forwardDenitrification is an important biologically-mediated process by which nitrate is reduced. This is especially important in environments with excess inputs of nutrients. Denitrification is shown in the following (unbalanced) equation: CH2O + NO3- + H+àH2O + N2 + CO2. What are the oxidation states of each element in the equation? Write the number under the element in the equation. Write the half reactions. Label which half reaction shows oxidation and reduction. Balance each half reaction. Write is the full balanced equation. Calculate the reduction potential DEo’. Calculate the Gibbs free energy DGo’. Will this reaction produce energy for bacterial growth?arrow_forward2. KMNO4 + NagC204 + H2SO4 K2SO4 + MNSO4 + NagSO4 + CO2+ H20 Balanced equation: Oxidizing agent: Reducing agent: Criteria for each item Solution following the 5-step process Balanced equation Oxidizing agent Reducing agent 10 points 3 points 1 point 1 point Total points or each item: 15pointsarrow_forward
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- 50.00 grams of chromium (III) sulfate is dissolved in enough water to prepare 250.0 ml of solution. • What is the chemical formula for chromium (III) sulfate? • What is the molecular weight of chromium (III) sulfate grams per mole? • What is the concentration of chromium (III) sulfate in the solution above in moles per liter? • What is the concentration of Cr+3 ions in the solution above in moles per liter? Answer M • What is the concentration of SO4−2 ions in the solution above in moles per liter? • How many milliliters of the solution above are required to supply 0.100 moles of chromium (III) sulfate? • How many milliliters of the solution above are required to supply 0.275 moles of SO4−2 ions? • How many milliliters of the solution above are required to supply 0.120 moles of Cr+3 ionsarrow_forwardWhich element in the compounds below has an oxidation number (state) of +2? N in NH4Br Ba in Ba(OH)2 Cr in CrO3 V in VO2+arrow_forwardWhen the following equation is balanced properly under basic conditions, what are the coefficients of the species shown?Cl- + NiO2 Ni(OH)2 + Cl2 Water appears in the balanced equation as a fill in the blank 5 (reactant, product, neither) with a coefficient of . (Enter 0 for neither.)Which element is oxidized?arrow_forward
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