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19. Determine which of the following...
1. which of the following is the strongest oxidizing agent? (in an acidic solution) (pick one)...
1. which of the following is the strongest oxidizing agent? (in an acidic solution) (pick one) PbO2(s) Mg(s) Ba2+(aq) NO3-(aq) MnO2(s) 2. what element is being oxidized in the following redox reaction? Co2+(aq)+NH4+(aq)=Co(s)+NO3-(aq) Choices are: O,N,Co,Xe, or H 3. which of the following reactant pairs would result in a spontaneous redox reaction? (pick one) Al(s)+Pb2+(aq) Pb(s)+Mn2+(aq) Ni(s)+Zn2+(aq) Ag(s)+Ni2+(aq)
help me to solve worksheet like an example sheet i am posting it for second time....
help me to solve worksheet like an example sheet i am posting
it for second time. help me
CHEM 200 CHAP 7: Classifying Chemical Reactions Dr. Bancroft ZnCl2 (aq) + (NH)2SO4 (aq) → _ZnSO4 (aq) + 2NH.CI (aq) Total Ionic: Circle one: • Redox: Combination • Redox: Decomposition • Redox: Single Replacement • DD: Precipitation • DD: Acid-Base • No Reaction Occurs Net lonic: 2 H2 (g) + 2 H20 (1) Total Ionic: Circle one: • Redox: Combination • Redox:...
19. a. Balance the following redox reaction if it occurs in acidic solution. How many electrons...
19. a. Balance the following redox reaction if it occurs in acidic solution. How many electrons are transferred, and what are the half reaction potentials? Fe 2+(aq) + MnO4 ?(aq) ? Fe 3+(aq) + Mn 2+(aq) b. What element is being oxidized, and what is the oxidizing agent in the given redox reaction? Mg2+(aq) + NH4 +(aq) ? Mg(s) + NO3 ?(aq)
Determine which of the following pairs of reactants will result in a spontaneous Pb2+(aq) + 2...
Determine which of the following pairs of reactants will result in a spontaneous Pb2+(aq) + 2 e- - Pb(s) Eº = -0.13 V Cu+(aq) + e- - Cu(s) E = 0.52 V Ag+ (aq) + e Ag(s) Eº = 0.80 V Br2(+2 e 2 Br-(s) E° = 1.09 V reaction at 25°C. Li+(aq) + e- - Li(s) E° = -3.04 V A13+(aq) + 3 e- → Al(s) E° = -1.66 V Fe3+(aq) + 3 e" -> Fe(s) E° = -0.036...
Balance the following redox reaction if it occurs in acidic solution. Your answer should indicate the...
Balance the following redox reaction if it occurs in acidic solution. Your answer should indicate the phases of all reactants and products. Sn(s) + Ag+(aq) → Ag(s) + Sn2+(aq) HTML Editor Keyboard Shortcuts
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C....
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Pb2+(aq) + Ag(s) Fe3+(aq) +Cd(s) Ag+(aq) + Br-(aq) Li+(aq) + Al(s) None of the above pairs will react.
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C....
Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Determine which of the following pairs of reactants will result in a spontaneous reaction at 25°C. Fe3+(aq) +Al(s) Pb2+(aq) + Au(s) Na+(aq) + Cr(s) Ag+(aq) + Br−(aq) None of the above pairs will react.
use the example to answer 8,9,10&11 Here's an example: Balance the following redox reaction, which occurs...
use the example to answer
8,9,10&11
Here's an example: Balance the following redox reaction, which occurs in acidic solution: Fe (aq)+ MnO4'(aq) -Fe (aq) + Mn (aq) Solution: +2 +7 +3 Step 1) +2 Fe2 (aq)+ MnOa (aq) Fe(aq) + Mn2 (aq) Fe (aq) MnO4 (aq) Mn2 (aq) 1 Fe on each side; 1 Mn on each side; no adjustment necessary Fe2 (aq) Fe 3'(aq) + e 5 e + MnO4(aq) Fe (aq) Fe (aq) + e (2+ on each...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the...
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
please show and explain all answers Relative Half-Cell Potentials Assuming standard conditions, answer the following questions....
please show and explain all answers
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed. Is Sn2+ (aq) capable of oxidizing Fe2+ (aq)? Is Sn metal capable of reducing Fe3+ (aq) to Fe2+ (aq)? Is VO2+ (aq) capable of oxidizing Fe2+ (aq)? Is Cr metal capable...
help me to solve worksheet like an example sheet i am posting
it for second time. help me
CHEM 200 CHAP 7: Classifying Chemical Reactions Dr. Bancroft ZnCl2 (aq) + (NH)2SO4 (aq) → _ZnSO4 (aq) + 2NH.CI (aq) Total Ionic: Circle one: • Redox: Combination • Redox: Decomposition • Redox: Single Replacement • DD: Precipitation • DD: Acid-Base • No Reaction Occurs Net lonic: 2 H2 (g) + 2 H20 (1) Total Ionic: Circle one: • Redox: Combination • Redox:...
Determine which of the following pairs of reactants will result in a spontaneous Pb2+(aq) + 2 e- - Pb(s) Eº = -0.13 V Cu+(aq) + e- - Cu(s) E = 0.52 V Ag+ (aq) + e Ag(s) Eº = 0.80 V Br2(+2 e 2 Br-(s) E° = 1.09 V reaction at 25°C. Li+(aq) + e- - Li(s) E° = -3.04 V A13+(aq) + 3 e- → Al(s) E° = -1.66 V Fe3+(aq) + 3 e" -> Fe(s) E° = -0.036...
use the example to answer
8,9,10&11
Here's an example: Balance the following redox reaction, which occurs in acidic solution: Fe (aq)+ MnO4'(aq) -Fe (aq) + Mn (aq) Solution: +2 +7 +3 Step 1) +2 Fe2 (aq)+ MnOa (aq) Fe(aq) + Mn2 (aq) Fe (aq) MnO4 (aq) Mn2 (aq) 1 Fe on each side; 1 Mn on each side; no adjustment necessary Fe2 (aq) Fe 3'(aq) + e 5 e + MnO4(aq) Fe (aq) Fe (aq) + e (2+ on each...
please show and explain all answers
Relative Half-Cell Potentials Assuming standard conditions, answer the following questions. (Use the table of Standard Reduction Potentials for common Half-reactions from your text. If hydrogen is one of the reagents, assume acidic solution.) cf Table 11.1 on p 403 of Zumdahl 8th ed. Is Sn2+ (aq) capable of oxidizing Fe2+ (aq)? Is Sn metal capable of reducing Fe3+ (aq) to Fe2+ (aq)? Is VO2+ (aq) capable of oxidizing Fe2+ (aq)? Is Cr metal capable...
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