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The chapter sections to review are shown in parentheses at the end of each problem.
15.48 Which of the following are
a.
b.
c.
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- (10) * Which reaction is an example of both a precipitation and a neutralization? (A) H3PO4(aq) + 3 KOH(aq) –→ K3PO4(aq) + 3 H2O(1) (B) FeC13(aq) + 3 KOH(aq) → Fe(OH)3(s) + 3 KCI(aq) (C) (NH4)2CO3(s) → 2 NH3(g) + CO2(g) + H20(1) (D) H2SO4(aq) + Ba(OH)2(aq) → BaSO4(s) + 2 H2O(1) (E) 2 C(s) + 02(g) → 2 CO(g) (11) * All of the statements regarding redox reactions are true except (A) a reducing agent causes another substance to be reduced. (B) halogens usually behave as oxidizing agents because they readily gain electrons. (C) metal ions are produced when pure metals are oxidized. (D) when a substance is oxidized its charge (or oxidation number) decreases. (E) alkali metals often behave as reducing agents because they readily lose electrons. (12) In a typical oxidation-reduction reaction the electrons are transferred (A) from the oxidizing agent to the reducing agent. (B) from what is being oxidized to the substance being reduced. (C) from what is being reduced to the substance being…arrow_forwardFill in the blanks: (7.1b. continued) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. b) Mn*2(ag) + BiO3 (aq) Bi*3. Bi* (aq) Mn04 (aq) Analysis: Previous page. Final Balanced equation: Mn* (aq) BiO3 (aq) H* - Mn04 (aq) Bi (aq) H20 Important: Check that number of atoms & charges are balanced.arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*taq) + NO2(g Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu(aq) * e Reduction-Half reation: Balancing 0 & H and charges: H* + NO3 (aq) + e - NO2(g) H20 Balancing electrons lost & gained and balancing the equation: Cus) NO3 (aq) * H* - Cu(aq) NO2(g) H20arrow_forward
- Question 16 of 40 Balance the following chemical equation (if necessary): C3H,O2(g) + O2(g) → H2O(g) + CO2(g) H2O (g) + CO2 (g) 3C2 2- Reset 1. 2. 4 6. 8. 9. ) (s) (1) (g) (aq) LO 3.arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (aq) - Cro, (aq) + Clug Analysis: Balancing under acidic condition first (adding H30 & H*) Oxidation-Half reation: Balancing atoms & charges: Cr(OH)) * H20 - Cro, ug) + Reduction-Half reation: Balancing atoms and charges: e Clap H20 Balancing electrons lost & galned Multiply oxidation-half reaction by e's Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forwardConsider the unbalanced reaction below occurring in acidic solution: PbO₂ (s) + (aq) Pb2+ (aq) + 1₂(5) Which of the following reactions is the properly balanced net redox reaction? O PbO₂(s) + 21-(aq) + 4H*(aq) O PbO₂(s) +41-(aq) + 4H*(aq) O PbO₂(s) +1-(aq) + 2H*(aq) - O PbO₂(s) + 21-(aq) - 1 Pb2+ (aq) + 12(s) + 2H₂O() Pb2+ (aq) +212(s) + 2H₂O() Pb2+ (aq) + 1₂(s) + H₂O() Pb2+ (aq) + 1₂(s) + O₂(g)arrow_forward
- (7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + CIO (nq) - Cro, (aq) Analysis: Balancing under acidic condition first (adding H30 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)x) * H20 - Cro, ug * H' + Reduction-Half reation: Balancing atoms and charges: 10 taq H20 Balancing electrons lost & gained Multiply oxidation-half reaction by Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forward(7.1a) Complete and balance the following by ion-electron method. Reactions are taking place in acidic solution. a) Cu(s) + NO3 (aq) - Cu*2(aq) + NO2(g) + NO29) Analysis: Oxidation-Half reation: Balancing atoms & charges: Cu(s) Cu*2, (aq) e Reduction-Half reation: Balancing O & H and charges: H* + NO3 (aq) e NO2(g) + 1 H20 Balancing electrons lost & gained and balancing the equation: Cu(s) NO3 (aq) + H* - Cu*(aq) NO2(g) H20arrow_forward4. 5. OH + HCI I strong acid catalystarrow_forward
- part 2arrow_forward(7.2b) Complete and balance the following by ion-electron method. Reactions are taking place in alkaline solution. b) Cr(OH)a) + Clo (aq) - Cro, 2(aq) • Clzup Analysis: Balancing under acidic condition first (adding Hy0 & H") Oxidation-Half reation: Balancing atoms & charges: Cr(OH)y) * H20 - Cro, ng) + H' Reduction-Half reation: Balancing atoms and charges: CIo (aq) e Clp H20 Balancing electrons lost & gained Multiply oxidation-half reaction by e's Multiply reduction-half reaction by e's Final balanced equation: Continue next page.arrow_forwardNeutralizationarrow_forward
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