For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. 4 Al(s) + 3 O2(g) ® 2 Al2O3
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issue 2
For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank.
4 Al(s) + 3 O2(g) ® 2 Al2O3
| Element | # oxy initial | # oxy final | e- lost or won | oxidized or reduced |
Oxidizing agent or Reducing agent |
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| → | ||||||
| → |
Step by step
Solved in 4 steps with 4 images
- issue 7For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. CH4 + O2 → CO2 + H2O Element # oxy initial # oxy final e- lost or win Oxidized or Reduced Oxidizing Agent or Reducing agent: C → H → O →issue 1Question 1 options:In the reaction below, identify the reducing agents and the agentsoxidants, as well as reduced and oxidized substances. 2 Au3+(aq) + 6 I−(aq) ⇌ 2 Au(s) + 3 I2(s) Oxidizing Agent:Reducing agent:Reduced substance:Oxidized substance: issue 2In the reaction below, identify the reducing agents and the agentsoxidants, as well as reduced and oxidized substances. 2 NO2(g) + 7 H2(g) ⇌ 2 NH3(g) + 4 H2O(l) Oxidizing Agent:Reducing agent:Reduced substance:Oxidized substance:2Cl- + SS2- + Cl2 In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent.
- issue 3For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. 2 Fe (s) + 3 SnCl2 (aq) → 2 FeCl3 (aq) + 3 Sn (s) Element # oxy initial # oxy final e- lost or won oxidized or reduced Oxidizing agent or Reducing agent → → →Identify the oxidizing agent, element oxidized, reducing agent and element reduced from the following line notation. Fe(s)|FeBr2(aq)||NaBr(aq)|Br2(l)|Pt(s) Group of answer choices Fe is the reducing agent, Fe is oxidized, Br2 is the oxidizing agent, Br2 is reduced. FeBr2 is the reducing agent, Fe+2 is reduced, NaBr is the oxidizing agent, Br-1 is oxidized. Fe is the oxidizing agent, Fe is oxidized, Br2 is the reducing agent, Br2 is reduced. FeBr2 is the oxidizing agent, Fe+2 is reduced, NaBr is the reducing agent, Br-1 is oxidized. FeBr2 is the reducing agent, Fe+2 is oxidized, NaBr is the oxidizing agent, Br-1 is reduced. FeBr2 is the oxidizing agent, Fe+2 is oxidized, NaBr is the reducing agent, Br-1 is reduced. Fe is the reducing agent, Fe is reduced, Br2 is the oxidizing agent, Br2 is oxidized. Fe is the oxidizing agent, Fe is reduced, Br2 is the reducing agent, Br2 is oxidized.issue 8For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. Na(s) + Br2(l) → NaBr(s) Element # oxy initial # oxy final e- lost or win oxidized or reduced Oxidizing agent or Reducing agent Na → Br → issue 13Balance the reaction equation below using the half-reaction method. Step 1: Write the two balanced half-reactions removing the spectator ions, if any. Step 2: Balance the electrons. Step 3: Add half-reactions by replacing spectator ions and/or recombining compounds. Na + Br2 → NaBr issue 14Compare the two reactions below by calculating their potential difference. Which is a spontaneous reaction? Use the table: Half-reaction potential. 2 Al(s) + 3 Zn2+(aq) → 2 Al3+(aq) + 3 Zn(s) 2 Al3+(aq) + 3 Cu(s) → 2 Al(s) + 3 Cu2+(aq) issue 15The reaction below takes place in a galvanic cell. 2 Fe(s) + 6H+(aq) → 2 Fe3+(aq) + 3 H2(g) E° = 0.04 V You want to maximize the…
- Consider the following unbalanced reaction: MnO4-(aq) + C2O42-(aq) → MnO2(s) + CO32-(aq) 1.Enter the oxidation number of Mn in the compound MnO4- 2.Balance the overall reaction in basic media. 3.Identify the species being oxidized and reduced. Identify the species being oxidized and reduced.Choose one of the following -.Mn is oxidized and C is reduced -.C is oxidized and Mn is reduced -O is both oxidized and reducedWhich is the balanced chemical equation for the following redox reaction in an acidic medium? Cr2O72- + C2O42- → Cr3+ + CO2 Cr2O72- + C2O42- + 14H+ → 2Cr3+ + 2CO2 + 7H2O Cr2O72- + C2O42- → Cr3+ + CO2 Cr2O72- + 3C2O42- + 14H+ → 2Cr3+ + 6CO2 + 7H2O 3Cr2O72- + C2O42- + 14H+ → 6Cr3+ + 2CO2 + 7H2O10 Which of the following is the strongest oxidizing agent? Br2(l) Au3+(aq) Br-(aq) Au(s) Ag(s)
- Unit 2: Balance the chemical equation for the following redox reaction under acidic aqueous conditions with the smallest whole-number coefficients possible using the half-reaction method. What is the coefficient of C2H5OH? Enter your answer as a number, not in words. Cr2O72-(aq) + C2H5OH(aq) → Cr3+ (aq) + CO2(g)Determine whether the underlined element is oxidized or reduced in a given partial equation and state if it is an oxidizing agent or a reducing agent H2O2 → O2 KBrO3 → KBr Fe + FeSO4 → Fe2(SO4)3 Na2C2O4 → CO2 I2 → KIissue 1For the reaction below, complete the equation summary table. If an element has no change in oxidation number, leave the last two columns blank. 4 HCl + O2 ® 2 H2O + 2 Cl2 Element # oxy initial # oxy final e- lost or won oxidized or reduced Oxidizing agent or Reducing agent H +1 → +1 0 --- --- → →