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Basic Chemistry
- Many oxidationreduction reactions can be balanced by inspection. Try to balance the following reactions by inspection. In each reaction, identify the substance reduced and the substance oxidized. a. Al(s) + HCl(aq) AlCl3(aq) + H2(g) b. CH4(g) + S(s) CS2(l) + H2S(g) c. C3H8(g) + O2(g) CO2(g) + H2O(l) d. Cu(s) + Ag+(aq) Ag(s) + Cu2+(aq)arrow_forwardWhich two of the following reactions are oxidation-reduction reactions? Explain your answer briefly. Classify the remaining reaction. (a) CdC12(aq) + Na2S(aq) CdS(s) + 2 NaCl(aq) (b) 2 Ca(s) + O2(g) 2 CaO(s) (c) 4 Fe(OH)2(s) + 2 H2O() + O2(g) 4 Fe(OH)3(s)arrow_forwardFour metals, A, B, C, and D, exhibit the following properties: (a) Only A and C react with 1.0 M hydrochloric acid to give H2(g). (b) When C is added to solutions of the ions of the other metals, metallic B, D, and A are formed. (c) Metal D reduces Bn+ to give metallic B and Dn+. Based on this information, arrange the four metals in order of increasing ability to act as reducing agents.arrow_forward
- 4. Identify the complete redox reaction for a FelFe3+||Cu2+ Cu cell. A. 2 Fe (s) + 3 Cu (s) →2 Fe³+ (aq) + 3 Cu²+ (aq) B. 2 Fe (s) + 3 Cu²+ (aq) → 2 Fe³+ (aq) + 3 Cu (s) c. 2 Fe³+ (aq) + 3 Cu (s) →→→ 2 Fe(s) + 3 Cu²+ (aq) D. Fe (s) + 2 Cu²+ (aq) →→→ Fe³+ (aq) + 2 Cu (s) s) 5. Identify the complete redox reaction for a Fe Fe3+AgAg cell. D A Fe(s) + Ag(s) →→→ Fe¹¹ (aq) + Ag' (aq) B. Fe(s) 1 Ag (aq) —> Fe' (aq) | Ag(s) + c. Fe (aq) + Ag (s) Fe(s) + Ag (aq) +arrow_forward8 H+(aq) + Cr2O72-(aq) + 3 H2S (aq)----> 2 Cr+3 (aq) + 7 H2O (l) + 3 S (s)a. Assign oxidation numbers to each element in each substance.b. What is the oxidizing AGENT? What is the reducing agent?arrow_forwardPART 1: Write the half - reaction of each redox reaction and determine the oxidizing and reducing agent. 1. H2 + F2 → 2HF 2. CO2 + H2O → CaH12Os + O2 3. MnO2 + Al → Mn +Al2O3 4. Fe203 + 3CO → 2Fe + 3CO2 5. NH3 + OCI -→ N2H4 + H2O + CHarrow_forward
- In this reaction, identify the: 2+ Fe(s) + 2 Agg) → 2 Ag(s) + Fe²+ < being oxidized reducing agen h oxidizing agent being reduced 1. Fe + 2. Ag 3. Ag 4. Fe²+arrow_forward4. For the following reactions: Balance each equation using half-reactions in the given conditions, and find the reduced and Oxidized reactants. a. Al + NO3 → Al(OH)4 + NH3 (basic conditions) b. Zn(s) + NO3(aq) → Zn+²(aq) + NH4 +(aq) (acidic conditions) C. PbO2 (s) + 12(s) → Pb²+ (aq) +103- (aq) (acidic conditions) 2- d. MnO4 + Sn(OH)4²→→ Sn(OH)²- + MnO₂ (basic conditions) e. CN- (aq) + CrO4)2(aq) →CNO- (aq) + Cr(OH)3 (s) (basic conditions)arrow_forwardIdentify the reducing agent, oxidizing agent, the atom or ion that is oxidized, and the atom or ion that is reduced. 1. C2O4-2 → CO2 2. CrO4-2 → Cr+3 3. Cu + HNO3 → Cu+2 (NO3)2 + NO + H2Oarrow_forward
- 4511/take/9/ MULTIPLE CHOICE Question 11 Which half-reaction correctly represents oxidation? → Fe +2 +2e= A Fe(s) (aq) B Fe +2 (aq) → Fe() + 2e- CFe + 2e¯ → Fe*2 (s) (aq) D Fe +2 → +2e Fe (aq) Fe (s) ర ర ర ర ó ó ó ó Ó00000000 Total Questions Answered All Changes Saved ☆ QL ✩ < * Continuearrow_forward= 2 AgNO3(aq) + Cu(s) 2 Ag(s) + Cu(NO3)2(aq) → a. What is element is oxidized? b. What element is reduced? c. What is the oxidizing agent? nd Jau d. What is the reducing agent? daun 1081100 zinotaufani eri aj pidigel sow azalnu sibens aviso91 2on llw AW A WOJOR OMA GA3R 32A319 od p112 bra zjinu tio #2010 2nologi Brun Ismisab er noe rigib S vem bns hobnuation exad ad bas alinu nistmooarrow_forwardreaction between nickel and copper(II) chlorideis shown below.Ni(s) + CuC l 2 (aq) → Cu(s) + NiC l 2 (aq)What are the half-reactions for this redox reaction?A. Ni → N i 2 + + 2 e - , C l 2 → 2C l - + 2 e -B. Ni → N i 2+ + e - , C u + + e - → CuC. Ni → N i 2+ + 2 e - , C u 2 + + 2 e - → CuD. Ni → N i 2+ + 2 e - , 2C u + + 2 e - → Cuarrow_forward
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