Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers...
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers to each, and write balanced net ionic equations.
a) Cu(s) 
Cu2+(aq) + 2e-
b) Cl2(aq) + 2e-
Cl-(aq)
c) Cu(s) + Cl2(aq)
Cu2+(aq) + 2Cl-(aq)
d) 4CuO(s) + CH4(g)
4Cu(s) + CO2(g) + 2H2O(l)
e) 2CuSO4(aq) + 4KI(aq)
2CuI (aq) + 2K2SO4(aq) +
I2(aq)
f) Cu2O(s) + Fe(SO4)3 (aq) +
H2SO4(aq)
2CuSO4(aq) + 2FeSO4(aq) +
H2O(l)
Homework Answers
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Identify the species (atoms/ elements) undergoing oxidation and
reduction in the following equations, assign oxidation numbers...
1) Making use of Table 1, write out individual redox half reactions (and their balanced sum,...
1) Making use of Table 1, write out individual redox half
reactions (and their balanced sum, including overall potential)
that describe the net chemical reactions in procedures (A-F).
A
Complexation:
CuCl2+ + 4NH3 -->
[Cu(NH3)4]Cl2
Net Ionic:
Cu2+ + 4NH3 -->
Cu(NH3)4+
B
Complexation:
CuCl2 + 2en -->
[Cu(en)2]Cl2
Net Ionic:
Cu2+ + 2en --> Cu(en)2+
C
Reduction:
2CuCl2 + 3NH4Cl -->
NH4[CuCl3] +
(NH4)2[CuCl4]
Net Ionic:
Cu2+ + 2Cl- + Cu --> 2CuCl
D
Reduction:
2CuCl2 + 4KI -->...
For the following, assign oxidation numbers. Which species is oxidized and which is reduced? Which species...
For the following, assign oxidation numbers. Which species is oxidized and which is reduced? Which species is the oxidizing agent and which is the reducing agent? (A) Zn(s) + CuCl2(aq) Cu(s) + ZnCl2 (B) MnO2 (s) + 4H+(aq) + 2Cl-(aq) Mn2+(aq) + 2H2O(l) + Cl2(g) (C)Zn(s) + 2HCl(aq)ZnCl2(aq) + H2(g)
Identify the elements listed in the table undergoing either reduction or oxidation in each of the...
Identify the elements listed in the table undergoing either reduction or oxidation in each of the following chemical equations. a.) Fe (s) + CuSO4laa) FeSO4(aq) + Cu(s) oxidation number Element oxidation or reduction before reaction after reaction Fe Select) [Select) Select] [Select) [Select) [Select ] cu a.) 2 ZnS(aq) + 3 O2(g) – 2 ZnO(s) + 6 SO2(g) Element oxidation number before reaction after reaction oxidation or reduction Select] S Select) Select [Select] O [Select] [Select)
1. Provide the oxidation number for each of the underlined elements in following compounds or ions:...
1. Provide the oxidation number for each of the underlined elements in following compounds or ions: (6) a) H3AsO3 b) d) H4P207 C202² KCIO4 N2H4 2. Which one of the following is not a oxidation-reduction reaction? (2) A) 2H2(g) + O2(g) → 2H2O(1) B) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) C) H2O(l) + NH3(g) → NH(aq) + OH(aq) D) FeSO4(aq) + K2Cr2OH(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(1) E) Cl2(g) +2KBr(aq) + Bra(l) + 2KCl(aq)...
Oxidation Numbers 1. Assign oxidation numbers to the atoms in each of the following. a) SO2...
Oxidation Numbers 1. Assign oxidation numbers to the atoms in each of the following. a) SO2 d) Mgl b) HCIO e) CaH c) Cr,0,2 f) Fe, 2. For each of the following: •assign oxidation numbers •indicate whether the equation represents a redox reaction .if redox, identify OA and RA a) Cu + 2 AgNO, 2 Ag + Cu(NO3)2 b) Pb(NO3)2 + 2 KI Pbl, + 2 KNO, c) Cl2 + 2 KI I2 + 2 KCI d) 2 NaCl 2...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to...
Using standard reduction potential in aqueous solutions at 25c Table, which substance is most likely to be oxidised by O2 (g) in acidic aqueous solution? Select one: a. Br2 (l) b. Br- (aq) c. Ni2+ (aq) d. Ag (s) e. Cu2+ (aq) Cathode (Reduction) Half-Reaction Standard Potential E° (volts) Li+(aq) + e- -> Li(s) -3.04 K+(aq) + e- -> K(s) -2.92 Ca2+(aq) + 2e- -> Ca(s) -2.76 Na+(aq) + e- -> Na(s) -2.71 Mg2+(aq) + 2e- -> Mg(s) -2.38 Al3+(aq)...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq)...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq) + 2Fe 3+ (aq) Fe2+ Cl2 OCH Fe3+
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq)...
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq) 1.36 O2(g)+4H+(aq)+4e? ?2H2O(l) 1.23 Br2(l)+2e? ?2Br?(aq) 1.09 NO3?(aq)+4H+(aq)+3e? ?NO(g)+2H2O(l) 0.96 Ag+(aq)+e? ?Ag(s) 0.80 I2(s)+2e? ?2I?(aq) 0.54 Cu2+(aq)+2e? ?Cu(s) 0.16 2H+(aq)+2e? ?H2(g) 0 Cr3+(aq)+3e? ?Cr(s) -0.73 2H2O(l)+2e? ?H2(g)+2OH?(aq) -0.83 Mn2+(aq)+2e? ?Mn(s) -1.18 How can the table be used to predict whether or not a metal will dissolve in HCl? In HNO3? Drag the terms on the left to the appropriate blanks on the right to...
Part A Identify each of the following as an oxidation or a reduction. Drag the appropriate...
Part A Identify each of the following as an oxidation or a reduction. Drag the appropriate items to their respective bins. Ag(s)—Ag+ (aq) +e- | Be2+ (aq) + 2e →Be(s) Cd(s) +Cd2+ (aq) + 2e Cu2+ (aq) + e +Cu+ (aq) Oxidation Reduction
3) Convert the following equations below to a net ionic equation and write it in the...
3) Convert the following equations below to a net ionic equation and write it in the space provided. H2SO4 (aq.) + NaOH(aq.) → Na2SO4(aq.) + 2H2O(1) 4) Label the oxidation, reduction processes and oxidizing and reducin agents in the reaction given below a) Fe(s) + O2(g) → Fe2O3 (8) 3) Convert the following equations below to a net ionic equation and write it in the space provided. H2SO4 (aq.) + NaOH(aq.) → Na2SO4(aq.) + 2H2O(1) 4) Label the oxidation, reduction...
1) Making use of Table 1, write out individual redox half
reactions (and their balanced sum, including overall potential)
that describe the net chemical reactions in procedures (A-F).
A
Complexation:
CuCl2+ + 4NH3 -->
[Cu(NH3)4]Cl2
Net Ionic:
Cu2+ + 4NH3 -->
Cu(NH3)4+
B
Complexation:
CuCl2 + 2en -->
[Cu(en)2]Cl2
Net Ionic:
Cu2+ + 2en --> Cu(en)2+
C
Reduction:
2CuCl2 + 3NH4Cl -->
NH4[CuCl3] +
(NH4)2[CuCl4]
Net Ionic:
Cu2+ + 2Cl- + Cu --> 2CuCl
D
Reduction:
2CuCl2 + 4KI -->...
Identify the elements listed in the table undergoing either reduction or oxidation in each of the following chemical equations. a.) Fe (s) + CuSO4laa) FeSO4(aq) + Cu(s) oxidation number Element oxidation or reduction before reaction after reaction Fe Select) [Select) Select] [Select) [Select) [Select ] cu a.) 2 ZnS(aq) + 3 O2(g) – 2 ZnO(s) + 6 SO2(g) Element oxidation number before reaction after reaction oxidation or reduction Select] S Select) Select [Select] O [Select] [Select)
1. Provide the oxidation number for each of the underlined elements in following compounds or ions: (6) a) H3AsO3 b) d) H4P207 C202² KCIO4 N2H4 2. Which one of the following is not a oxidation-reduction reaction? (2) A) 2H2(g) + O2(g) → 2H2O(1) B) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) C) H2O(l) + NH3(g) → NH(aq) + OH(aq) D) FeSO4(aq) + K2Cr2OH(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(1) E) Cl2(g) +2KBr(aq) + Bra(l) + 2KCl(aq)...
Oxidation Numbers 1. Assign oxidation numbers to the atoms in each of the following. a) SO2 d) Mgl b) HCIO e) CaH c) Cr,0,2 f) Fe, 2. For each of the following: •assign oxidation numbers •indicate whether the equation represents a redox reaction .if redox, identify OA and RA a) Cu + 2 AgNO, 2 Ag + Cu(NO3)2 b) Pb(NO3)2 + 2 KI Pbl, + 2 KNO, c) Cl2 + 2 KI I2 + 2 KCI d) 2 NaCl 2...
What species is undergoing oxidation (if any) in the following reaction? Cl2(g) + 2Fe2+ (aq) 2Cl"(aq) + 2Fe 3+ (aq) Fe2+ Cl2 OCH Fe3+
Part A Identify each of the following as an oxidation or a reduction. Drag the appropriate items to their respective bins. Ag(s)—Ag+ (aq) +e- | Be2+ (aq) + 2e →Be(s) Cd(s) +Cd2+ (aq) + 2e Cu2+ (aq) + e +Cu+ (aq) Oxidation Reduction
3) Convert the following equations below to a net ionic equation and write it in the space provided. H2SO4 (aq.) + NaOH(aq.) → Na2SO4(aq.) + 2H2O(1) 4) Label the oxidation, reduction processes and oxidizing and reducin agents in the reaction given below a) Fe(s) + O2(g) → Fe2O3 (8) 3) Convert the following equations below to a net ionic equation and write it in the space provided. H2SO4 (aq.) + NaOH(aq.) → Na2SO4(aq.) + 2H2O(1) 4) Label the oxidation, reduction...
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