Redox Reactions

In the following reaction identify the oxidizing agent and the reducing agent:   

Consider the following reaction: Cu + 2 AgNO3 → Cu(NO3)2 + 2 Ag   a. Cu is oxidized b. Ag+ is reduced c. Cu is the reducing agent d. All of the following is correct 

Which of the following is the strongest reducing agent?   A) Sn2+(aq) B) Cr3+(aq) C) Sn4+(aq) D) Cr (s) E) Sn (s)

Which of the following is the strongest reducing agent? A) Al(s) B) Zn(s) C) Mg(s) D) Al3+(aq) E) Mg2+(aq)

What is the ratio of oxidizing agent to reducing agent? Ca2+ (aq) + Al (s)   →    Ca (s) + Al 3+ (aq)   a) 2 : 3 b) 3 : 2 c) 1 : 1 d) 4 : 6 

Which one of the following is the strongest oxidizing agent? a) VO2 +              b) VO 2+               c) V 2+               d) V 3+

Which statement is true for this reaction? Fe (s) + Au(NO3)3 (aq)  → Fe(NO3)3 (aq) + Au (s) a. Metallic iron is the reducing agent b. Gold ion is oxidized c. Metallic iron is reduced d. Nitrate ion (NO3) is the oxidizing agent

In the redox reaction 2 Al + 3 CuSO 4 → 3 Cu + Al 2(SO4)3 A. Al is the reducing agent and each Al atom gains three electrons in the reaction. B. Al is the oxidizing agent and each Al atoms loses three electrons in the reaction. C. CuSO4 is the reducing agent and each Cu atom loses two electrons in the reaction. D. CuSO4 is the oxidizing agent and each Cu atoms gains two electrons in the reaction. E. Cu is the oxidizing agent and each Cu atom loses two electrons in the reaction.

Consider the following oxidation-reduction reaction: MnO2   +   4 HCl   →   Cl 2   +   2 H 2O   +   MnCl 2 What is the oxidizing agent?   1. MnO2           2. HCl           3. Cl   2           4. MnCl 2

Which of the following reactions is an oxidation-reduction reaction? 1. HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l) 2. Ca (s) + HCl (aq) → CaCl 2 (aq) + H2 (g) 3. 3 Na2S (aq) + 2 FeCl 3 (aq) → Fe2S3 (s) + 6 NaCl (aq) 4. CO2 (g) + 2 LiOH (aq) → Li 2CO3 (s) + H2O (l)

Which one of the following is the strongest oxidizing agent? a) VO2 +           b) VO 2+           c) V 2+           d) V 3+

What is the oxidizing agent in the following oxidation–reduction reaction? 2 H+ + 3 H2O + As2O3 + 2 NO3– → 2 H3AsO4  + 2 HNO2 A. H+ B. As2O3 C. NO3– D. H3AsO4 E. HNO2

Which element is oxidized and which is reduced in the following reaction: 2 Fe2O3(s) + 3 C(s) → 4 Fe(s) + 3 CO 2(g) a) O is reduced and C is oxidized b) O is oxidized and C is reduced c) Fe is oxidized and O is reduced d) Fe is reduced and C is oxidized e) Fe is oxidized and C is reduced

Consider the following unbalanced oxidation reduction reaction for the question CoO2(s) + Br2(l) → Co3+(aq) + HBrO(aq) Which compounds are involved in the reduction half reaction? (a) CoO2(s), Br2(l) (b) Co3+(aq), HBrO(aq) (c) CoO2(s), Co3+(aq) (d) Br2(l), HBrO(aq) (e) CoO2(s), HBrO(aq) (f) Br2(l), Co3+(aq)

Fill in the blanks. A reducing agent is a chemical that causes the _________ of another chemical species by __________electrons to/from the other species. In the process of doing so, the reducing agent gets __________. The answers in order are (a) oxidation, taking, reduced (b) reduction, giving, oxidized  (c) oxidation, giving, oxidized  (d) reduction, taking, reduced  (e) oxidation, taking, oxidized  (f)  reduction, giving, reduced 

Consider the chemical reaction: 2 SO2 (g) → SO(g) + SO3 (g) Determine if the sentence below is true or false The reaction is a redox reaction.

Consider the following chemical equation,             2 Al3+(aq) + 2 Fe(s)  →  2 Al(s) + 3 Fe2+(aq) identify the reducing agent.   A) Al3+ B) Fe C) Al D) Fe2+ E) This is not an oxidation-reduction reaction.

What is the ratio of oxidizing agent to reducing agent? _______ Ca2+ (aq) + _______ Al (s) → _______ Ca (s) + _______ Al  3+ (aq)   a) 2 : 3              b) 3 : 2              c) 1: 1              d) 4 : 6 

Which species is reduced in the reaction below?        2Al(s) + NO2–(aq) + H2O(l)  + OH-(aq) → 2AlO2–(aq) + NH3(g) a. Al b. NO2– c. H2O(l) d. OH– e. None of the above - this is not an oxidation-reduction reaction.    

Consider the reaction2 Fe3+ (aq) + 2 I– (aq)   ⇌   2 Fe2+ (aq) + I2 (aq)Which statement for the reaction is true? A. Fe3+ is oxidizedB. Fe3+ increases in oxidation numberC. Fe3+ is reducedD. I– is reduced 

In the chemical reaction, Zn (s) + CuSO4 (aq)   ⇌   ZnSO4 (aq) + Cu (s), A. Metallic zinc is the reducing agentB. Metallic zinc is reducedC. Copper ion is oxidizedD. Sulfate ion is the oxidizing agent 

The following three questions are based on the following reaction:2 Cr + 3 ClO2 – + 3 H2O → 2 Cr(OH)3 + 3 ClO –The reducing agent is:a) Crb) ClO2c) H2Od) Cr(OH)3e) ClO The oxidizing agent is:a) Crb) ClO2c) H2Od) Cr(OH)3e) ClO The oxidation number of chromium on the right hand side of the equation is:a) 2b) -2c) 3d) 4e) 6

In the following reaction identify the oxidizing agent and the reducing agent:32 H+ + 14 MnO4 – + 5 N2H4 → 14 Mn2+ + 26 H2O + 10 NO 3 –

The activity series are listed in order from most reactive to least reactive. Answer each of the following questions based on the following half reactions:HALF REACTIONSClO2 (g) + e–→ 2 ClO2– (aq)Cu+ (aq) + e– → Cu (s)Fe3+ (aq) + 3 e– → Fe (s)K+ (aq) + e– → K (s)a) Which is the strongest oxidizing agent?    b) Which is the strongest reducing agent?    c) Could the following reaction occur: Fe3+ (aq) + Cu (s) → Fe (s) + Cu+ (aq)    

What is the ratio of oxidizing agent to reducing agent?_______ Ca2+ (aq) + _______ Al (s) → _______ Ca (s) + _______ Al  3+ (aq) a) 2 : 3              b) 3 : 2              c) 1: 1              d) 4 : 6 

Identify which has been oxidized and reduced. Then identify the oxidizing agent in the following:2 NH3 + OCl - → N2H4 + H2O + Cl -Oxidized: ______________                     Reduced: ____________Oxidizing Agent: ____________              Reducing Agent: _____________

Which statement about this redox reaction is correct? Fe(s) + Cu2+ (aq) → Cu(s) + Fe2+ (aq) A. Cu2+ is oxidized B. Cu2+ gains in oxidation number C. Cu2+ is reduced D. Fe is reduced

Identify the oxidation and reduction steps in the following reaction:4Fe +3O2 → 2Fe2O3A.  Oxidize: O2 → 2 O2− + 2 e−                  Reduced: Fe → Fe  3+ + 3 e−B.  Oxidize: Fe → Fe2+ + 2 e−                    Reduced: O2 → 2 O2− + 4 e−C.  Oxidize: Fe → Fe3+ + 3 e−                    Reduced: 4 e− + O2 → 2 O2− D.  Oxidize: Fe → Fe3+ + 3 e−                      Reduced: O2 → 2 O2− + 4 e−E.  Oxidize: O2 → 2 O2− + 4 e−                  Reduced: Fe → Fe3+ + 3 e− 

15. Which of the following reactions is/are redox reactions?(1) K2CrO4 + BaCl2 → BaCrO4 + 2KCl(2) Ag+ + Br− → AgBr(3) Cu + S → CuS      A) only reaction (1)     B) only reaction (2)     C) only reaction (3)             D) both reactions (1) and (3)            E) both reactions (2) and (3)

In which group can each substance act as an oxidizing agent?A. Cl2, MnO2, CuB. Cl2, MnO4–, Cu2+C. Cl-, MnO4–, Cu+D. Cl2, Mn, Cu2+

Which of the following describe oxidation?A. Increase in oxidation numberB. Loss of electronsC. Loss of neutronsD. Gain of protonsE. Both A and B

Which one of the following is  not a redox reaction?a) 2H2O2(aq) → 2H2O(l) + O2(g) b) C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)c) Na6FeCl8(s) + 2Na(l) → 8NaCl(s) + Fe(s)d) Al(OH)4-(aq) + 4H+(aq) → Al3+(aq) + 4H2O(l)e) CO2(g) + H2(g) → CO(g) + H2O(g)               

Consider the following balanced redox reaction: 3CuO(s) + 2NH3(aq) → N2(g) + 3H2O(l) + 3Cu(s)Which of the following statements is true?a) CuO(s) is the oxidizing agent and copper is oxidized.b) CuO(s) is the oxidizing agent and copper is reduced.c) CuO(s) is the reducing agent and copper is oxidized.d) CuO(s) is the reducing agent and copper is reduced.e) CuO(s) is the oxidizing agent and N2(g) is the reducing agent.

Using the table below, which substance can oxidize I – (aq) to I2 (s)?a) Br2 (l)b) Ni2+ (aq)c) Ag (s)d) Cu2+ (aq)e) More than one of the above

Which substance serves as the reducing agent in the following unbalanced reaction that occurs in acid:Cr2O72– (aq) + Ni (s) → Ni 2+ (aq) + 2 Cr 3+ (aq) (acidic solution) a) H+ (aq)b) Cr2O72– (aq)c) Ni (s)d) Ni2+ (aq)e) H2O (l) 

Is the following reaction an example of a redox reaction?Cr2O72– (aq) + H2O (l) ⇄ 2 CrO 42– (aq) + 2 H+ (aq) a) Yes, Cr is oxidized and oxygen is reducedb) Yes, Cr is oxidized and hydrogen is reducedc) Yes, oxygen is oxidized and Cr is reducedd) Yes, hydrogen is oxidized and Cr is reducede) No, neither hydrogen, oxygen, nor Cr are oxidized or reduced

Which statement is most true of the reaction:Bi2S3 (s) + 3 H+ (aq) → 2 Bi3+ (aq)+ 3 H2S (aq)a) This is a redox reaction because Bi2S3 serves as the oxidizing agent and H+ as the reducing agentb) This is a redox reaction because Bi2S3 serves as the reducing agent and H+ as the oxidizing agentc) This is a redox reaction because Bi is oxidized and H is reducedd) Both a and c are truee) None of the above are true because the reaction is not a redox reaction  

Which of the following are redox reactions?I. CuSO4 + 2NaOH → Cu(OH) 2 + Na 2SO4 II. 2Al + 3MgSO4 → 3Mg + Al 2(SO4)3 III. 2(NH4)3PO4 + 3Ba(NO3)2 → Ba 3(PO4)2 + 6NH4NO3 IV. 2HNO3 + 3H3AsO3 → 2NO + 3H 3AsO4 + H2O

Which statement is true for this reaction?Zn (s) + CuSO4 (aq)  → Cu (s) + ZnSO4 (aq)a) Copper ion is oxidized. b) Sulfate ion is the oxidizing agent. c) Metallic zinc is reduced. d) Metallic zinc is the reducing agent. 

In this reaction, which substance behaves as the oxidizing agent?Pb (s) + PbO2 (s) + 2 H2SO4 → 2 PbSO4 (s) + 2 H2O (l)(A)  PbSO4(B) PbO2(C) Pb(D) H2SO4

Which experimental evidence clearly illustrates the oxidizing property of chlorine, Cl2?(A) the use of chlorides as oxidizing agents in the manufacture of matches(B) the reaction of chlorine with sodium bromide solution, resulting in the displacement of bromine(C) its moderate solubility in aqueous solution(D)  its liberation at the anode during the electrolytic of sodium chloride solution

Which statement about this redox reaction is correct?2 ZnS(s) + 3 O2(g) → 2 ZnO(s) + 2SO2(g)A. oxygen is reducedB. Sulfur gains electronsC. Oxygen is the reducing agentD. Sulfur is the oxidizing agent

Define oxidation and reduction in terms of (a) electron transfer

Which circled region of the periodic table shown here contains the most readily oxidized elements? Which contains the least readily oxidized?

Which element is oxidized and which is reduced in the following reactions?(a) N2 (g) + 3 H2 (g) → 2 NH3 (g) 

Which element is oxidized and which is reduced in the following reactions?(b) 3 Fe(NO3)2 (aq) + 2 Al (s) → 3 Fe (s) + 2 Al(NO 3)3 (aq)

Which element is oxidized and which is reduced in the following reactions?(c) Cl2 (aq) + 2 NaI (aq) → I 2 (aq) + 2 NaCl (aq)

Which element is oxidized and which is reduced in the following reactions?(d) PbS (s) + 4 H2O2 (aq) → PbSO4 (s) + 4 H2O (l) 

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or acid-base reactions.(c) Sr(NO3)2(aq) + H2SO4(aq) → SrSO4(s) + 2 HNO3(aq)

Which of the following are redox reactions? For those that are, indicate which element is oxidized and which is reduced. For those that are not, indicate whether they are precipitation or acid-base reactions.(d) 4 Zn(s) + 10 H+(aq) + 2 NO3-(aq) → 4 Zn2+(aq) + N2O(g) + 5 H2O(I) 

Specify which of the following equations represent oxidation–reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced.a. CH4(g) + H2O(g) → CO(g) + 3H2(g)

Specify which of the following equations represent oxidation–reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced.b. 2AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + 2Ag(s) 

Specify which of the following equations represent oxidation–reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced.c. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) 

Specify which of the following equations represent oxidation–reduction reactions, and indicate the oxidizing agent, the reducing agent, the species being oxidized, and the species being reduced.d. 2H+(aq) + 2CrO42-(aq) → Cr2O72-(aq) + H2O(l) 

Consider the following reaction equations. Which is/are redox reactions?i. Cr(C2H3O2)2 (aq) + 2 NaOH (aq) → 2 NaC 2H3O2 (aq) + Cr(OH)2 (s)ii. Fe (s) + 4 HNO3 (aq) → Fe(NO3)2 (aq) + 2 NO2 (g) + 2 H2O (l)iii. B2O3 (s) + 6 KOH (aq) → 2 K 3BO3 (aq) + H2O (l) A. i onlyB. ii onlyC. iii onlyD. i and iiE. ii and iii

What is the oxidizing agent in the (unbalanced) reaction?Cu(s) + H+(aq) + NO3-(aq) → NO(g) + H2O(l) + Cu2+(aq)A) CuB) H+C) NO3-D) NOE) Cu2+

Which of the following is True?A) reduction results in a decrease in the oxidation numberB) reduction is the loss of electronsC) reduction occurs at the cathodeD) an increase in the oxidation number occurs only at the cathodeE) both A and C

What element is being oxidized in the following redox reaction? Cr2O72-(aq) + Mn2O3(s) → Cr3+(aq) + MnO2(aq)A) OB) CrC) MnD) ClE) both Mn and Cl

Reduction involves which of the following?A) decrease in oxidation numberB) loss of electronsC) gain of electronsD) increase in oxidation numberE) both A and C

What element is being oxidized in the following redox reaction?Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq)A) OB) CrC) HD) Cl 

What element is being oxidized in the following redox reaction?H2O2(l) + ClO2(aq) → ClO21-(aq) + O2(g)A) HB) OC) CD) ClE) This is not a Redox Rxn

Which is the reducing agent in the (unbalanced) reaction?S2O32-(aq) +  I2(aq) +  H+(aq)  →  I1-(aq)  + S4O62-(aq)            A)  S2O32-    B)  H+    C) I 2      D)  S4O62-  E)  I1- 

Solve the following problem:Consider the reaction,Fe(s) + Cu2+(aq) → Cu(s) + Fe2+(aq), which statement is true for the reaction? Select one:

Solve the following problem:Which change requires an oxidizing agent to produce the indicated product?A. S2O32- → S4O62- B. Zn2+ → Zn C. ClO- → Cl- D. SO3 → SO42-

Consider the redox equation shown below and determine which of the statements(s) that follow is/are correct.SeO32-(aq) + Cl2(aq) → SeO42-(s) + Cl-(aq)i.  SeO42- is the reducing agent.ii. Cl2 is the oxidizing agent.iii. Cl- is the oxidizing agent.A. i onlyB. ii onlyC. iii onlyD. i and iiiE. ii and iii

What element is undergoing oxidation (if any) in the following reaction?CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)a) Ob) Hc) Cd) both C and He) None of the elements is undergoing oxidation 

In the two reactions below, which atom is oxidized?Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)H2O2 + CaS → CaSO4 + H2O (not balanced)a. Zn and Sb. H and Sc. Zn and Hd. S and Se. none of these

Which of the following statement(s) is/are correct regarding the following reaction?      SO42- + Br2 → S2O32- + BrO3- i. SO42- is the oxidizing agent ii. The oxidation number of Br in BrO3- is +6 iii. BrO3- is the reducing agent A) i only B) ii only C) iii only D) ii and iii E) i and iii

Aluminum metal reacts with oxygen gas (O2) to form aluminum oxide according to the equation4Al + 3O2   → 2Al2O3Aluminum is reduceda) Trueb) False

Which of the following is an oxidation-reduction reaction? Ba(C2H3O2)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaC2H3O2 (aq)H2CO3 (aq) + Ca(NO3)2 (aq) → 2HNO3 (aq) + CaCO3 (s)Cu (s) + 2AgNO3 (aq) → 2Ag (s) + Cu(NO3)2 (aq)AgNO3 (aq) + HCl (aq) → AgCl (s) + HNO3 (aq)HCl (aq) + NaOH (aq) → H2O (l) + NaCl (aq)

Which element is oxidized in this reaction?2CuO + C → 2Cu + CO 2Enter the chemical symbol of the element.

Which one of the following is not a redox reaction?a. Al(OH)4-(aq) + 4H +(aq) → Al 3+(aq) + 4H 2O(l)b. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)c. Na 6FeCl8(s) + 2Na(l) → 8NaCl(s) + Fe(s)d. 2H2O2(aq) → 2H2O(l) + O2(g)e. CO2(g) + H2(g) → CO(g) + H3O(g)

Which element is reduced in this reaction?16H+ + 2Cr2O72- + C2H5OH → 4Cr3+ + 11H2O + 2CO2 

Which element is reduced in this reaction?16H+ + 2Cr2O72- + C2H5OH → 4Cr3+ + 11H2O + 2CO2

Which element is reduced in this reaction?2KMnO4 + 3Na2SO3 + H2O → 2MnO2 + 3Na2SO4 + 2KOHEnter the chemical symbol of the element.

Which one of the following is not a redox reaction?a. 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)b. H2(g) + Cl2(g) → 2 HCl(g)c. 2 H2O2(aq) → 2 H2O(l) + O2(g)d. Fe2O3(s) + 3 H2SO4(aq) → Fe2(SO4)3(aq) + 3 H2O(l)e. 2 KMnO4(aq) + 10 FeSO4(aq) + 8 H2SO4(aq) → K2SO4(aq) + 2 MnSO4(aq) + 5 Fe2(SO4)3(aq) + 8 H2O(l)

Choose the appropriate labels to their respective targets. Indicate whether a reactant is a reducing agent or an oxidizing agent. 

Identify the oxidizing agent and the reducing agent for the following reaction.N2 + 6Li → 2Li 3Na. N2 is the oxidizing agent and Li is the reducing agent.b. Li is the oxidizing agent and N 2 is the reducing agent.

Identify the oxidizing agent and the reducing agent for the following reaction.2H2S + SO2 → 3S + 2H 2Oa. H2S is the oxidizing agent and SO2 is the reducing agent.b. SO2 is the oxidizing agent and H2S is the reducing agent. 

Identify the oxidizing agent and the reducing agent for the following reaction.C3H4 + 2H2 → C3H8a. C3H4 is the oxidizing agent and H2 is the reducing agent.b. H2 is the oxidizing agent and C3H4 is the reducing agent.

Identify the oxidizing agent and the reducing agent for the following reaction.Ag+ + Ti 3+ → Ag + Ti 4+a. Ag+ is the oxidizing agent and Ti 3+ is the reducing agent.b. Ti 3+ is the oxidizing agent and Ag+ is the reducing agent.

Which element is reduced in this reaction?2KMnO4 + 3Na2SO3 + H2O → 2MnO2 + 3NaSO4 + 2KOH

Which one of the following is NOT a redox reaction?a. 2H2O2(aq) → 2H2O(l) + O2(g)b. 2 Al(s) + Fe2O3(s)→ Al2O3(s) + 2Fe(s)c. BaCl2(aq) +K2CrO4(aq) →BaCrO4(aq) + 2 KCl(aq)d. 2 H2O(g) → 2H2(g) + O2(g)e. N2(g) + 3 H2(g) → 2NH3(g)

Which of the following reactions would be classified as oxidation-reduction?a. 2Na(s) + Cl 2(g) → 2NaCl(s)b. Na(s) + CuCl(aq) → NaCl(aq) + Cu(s)c. NaCN(aq) + CuCl(aq) → NaCl(aq) + CuCN(s)

Which one of the following reactions is not an oxidation-reduction reaction?a. N2(g) + 3H2(g) → 2NH3(g)b. NH4NO2(s) → N2(g) + 2H2O(l)c. Cu(s) + 2Ag+(aq) → Cu2+(aq) + 2Ag(s)d. C2H4(g) + H2(g) → C2H6(g)e. 2CrO42-(aq) + 2H+(aq) → Cr2O72-(aq) + H2O(l)

Which is reduced in the following reaction?Fe2O3 + 3 H2 → 2 Fe + 3 H2Oa. Fe2O3b. H2Oc. Fed. H2e. None of the above 

Which element is reduced in this reaction?Cr2O72− + 3HNO2 + 5H+ → 2Cr3+ + 3NO3−+4H2OEnter the chemical symbol of the element.

Which element is most likely to react with oxygen?a. aluminumb. argonc. magnesiumd. nitrogene. silicon

Which element is oxidized and which is reduced in the following reaction?N2(g) + 3H2(g) → 2NH3(g)

Which element is oxidized and which is reduced in the following reaction?3Fe(NO3)2(aq) + 2Al(s) → 3Fe(s) + 2Al(NO 3)3(aq)

Which element is oxidized and which is reduced in the following reaction?Cl2(aq) + 2 NaI(aq) → I2(aq) + 2 NaCl(aq)

Which element is oxidized and which is reduced in the following reaction?PbS(s) + 4H2O2(aq) → PbSO4(s) + 4H2O(l)

Which element is oxidized and which is reduced in the following reaction? N2(g) + 3H2(g) → 2NH3(g) Express your answer as chemical symbols separated by a comma.

Which element is oxidized and which is reduced in the following reaction? 3Fe(NO3)2(aq) + 2AI(s) → 3Fe(s) + 2AI(NO 3)3(aq)Express your answer as chemical symbols separated by a comma.

Which element is oxidized and which is reduced in the following reactions? Express your answers as chemical symbols separated by a comma. Enter the oxidized element first.a. N2(g) + 3H2(g) → 2NH3(g)b. Cl2(aq) + 2NaI(aq) → I2(aq) + 2NaCl(aq)c. PbS(s) + 4H2O2(aq) → PbSO4(s) + 4H2O(l)

Which element is oxidized and which is reduced in the following reaction? PbS(s) + 4H2O2(aq) → PbSO4(s) + 4H2O(l)Express your answer as chemical symbols separated by a comma.

Consider the reaction:Zn(s) + Fe2+(aq) → Zn2+(aq) + Fe(s)What is being reduced?

Which substance is the oxidizing agent in this reaction?Fe2O3 + 3 CO → 2 Fe + 3 CO2Express your answer as a chemical formula.Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. Oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. In general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number.An oxidizing agent is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction.A reducing agent is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction.As a summary, keep in mind the following:Oxidation means an increase in oxidation state and a loss of electrons and involves a reducing agent.Reduction means a decrease in oxidation state and a gain of electrons and involves an oxidizing agent.

Which element is oxidized in this reaction?Fe2O3 + 3 CO → 2 Fe + 3 CO2Enter the chemical symbol of the element.Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. Oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. In general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number.An oxidizing agent is an element or compound in a redox reaction that oxidizes another species and itself gets reduced and is therefore the electron acceptor in the reaction.A reducing agent is an element or compound in a redox reaction that reduces another species and itself gets oxidized and is therefore the electron donor in the reaction.As a summary, keep in mind the following:Oxidation means an increase in oxidation state and a loss of electrons and involves a reducing agent.Reduction means a decrease in oxidation state and a gain of electrons and involves an oxidizing agent.

Identify the oxidizing agent and the reducing agent for4Li(s) + O2(g) → 2Li2O (s)Mg(s) + Fe2+(aq) → Mg2+(aq) + Fe(s)

Which element is the oxidizing agent in this reaction?ZnO+C→Zn+COEnter the chemical symbol of the element. 

Which substance is the reducing agent in this reaction?2 Cr(OH)3 + 3 OCl− + 4 OH− → 2 CrO4−2 + 3 Cl−+ 5 H2OExpress your answer as a chemical formula.

In the following reactions, identify what is oxidized and what is reduced. 2Li(s) + F2(g) → 2LiF(s)a. both Li and F are oxidizedb. both Li and F are reducedc. Li is oxidized, F is reducedd. F is oxidized, Li is reduced Cl2(g) + 2KI(aq) → 2KCl(aq) + I 2(s)a. Cl is oxidized, K is reducedb. K is oxidized, Cl is reducedc. I is oxidized, Cl is reducedd. Cl is oxidized, I is reduced Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)a. both Cu2+ and Zn are reducedb. both Cu2+ and Zn are oxidizedc. Cu2+ is oxidized, Zn is reducedd. Zn is oxidized, Cu2+ is reduced

Which of the following is an oxidation-reduction reaction?a) Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g)b) Pb(C2H3O2)2(aq) + 2NaCl(aq) → PbCl2(s) + 2NaC2H3O2(aq)c) NaI(aq) + AgNO3(aq) → AgI(s) + NaNO3(aq)d) HCl(aq) + LiOH(aq) → LiCl(aq) + H2O(l)e) All of the above are oxidation-reduction reactions.

Classify each of the following as a redox reaction or a non-redox reaction.Zn + CuCl2 → ZnCl2 + CuSO3 + H2O → H2SO4HCl + NaOH → H2O + NaCl2CO + O2 → 2CO2

In the following reaction, what is reduced? 2 Al3+(aq) + 2 Fe(s) → 2 Al(s) + 3 Fe2+(aq)a. Feb. Al3+c. Ald. Fe2+ Which of the following is the oxidizing agent? 

Which element is oxidized in this reaction? ZnO + C → Zn + CO 

Which element is oxidized in this reaction?ZnO + C → Zn + CO

Which element is oxidized in this reaction?2CuO + C → 2Cu + CO 2