Balanced equation:
2 Al(s) + 6 HCl(aq) ====> 2 AlCl3(aq) + 3
H2(g)
Reaction type: single replacement
Aluminium is oxidized and H is reduced
Balanced equation:
4 S(s) + CH4(g) = CS2(l) + 2
H2S(g)
Reaction type: double replacement
Sulfur is reduced and Carbon is oxidized
Balanced equation:
C3H8(g) + 5 O2(g) = 3
CO2(g) + 4 H2O(l)
Reaction type: double replacement
Carbon is oxidized and oxygen is reduced
Balanced equation:
Cu(s) + Ag{+}(aq) = Ag(s) +
Cu{+}(aq)
Reaction type: single replacement
Copper is oxidized and Silver is reduced
any oxidation-reduction reactions can be balanced by i spection. Try to balance the following reactions by...
4. (6 pts.) Oxidation-Reduction Reactions: write out two ways you can identify the species that has been oxidized in a redox reaction: b. Identify the element reduced and the element oxidized in the following oxidation- reduction reactions. Fe(s) + CuCl2(aq) FeCl2(aq) + Cu(s) Element Oxidized: Element Reduced: C(s) + O2(g) → C02(g) Element Oxidized: Element Reduced:
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
Identify the species (atoms/ elements) undergoing oxidation and reduction in the following equations, assign oxidation numbers to each, and write balanced net ionic equations. a) Cu(s) Cu2+(aq) + 2e- b) Cl2(aq) + 2e- Cl-(aq) c) Cu(s) + Cl2(aq) Cu2+(aq) + 2Cl-(aq) d) 4CuO(s) + CH4(g) 4Cu(s) + CO2(g) + 2H2O(l) e) 2CuSO4(aq) + 4KI(aq) 2CuI (aq) + 2K2SO4(aq) + I2(aq) f) Cu2O(s) + Fe(SO4)3 (aq) + H2SO4(aq) 2CuSO4(aq) + 2FeSO4(aq) + H2O(l)
(10 pts) Balance the following redox reactions by first separating the oxidation and reduction half-reactions. a. Cut (aq) + Fe (s) Fe3+ (aq) + Cu(s) b. Cu(s) + HNO3 (aq) Cu2+ (aq) + NO (g) (basic solution) c. NH(aq) + O2(g) → N03 (aq) + H2O(l) (acidic solution) d. Cd(s) + NiO(OH)(s) + Ca(OH)2(s) + Ni(OH)2(s) (Nicad battery) e. The oxidation of iodide ion (1) by permanganate ion (MnO4) in basic solution to yield molecular iodine (12) and manganese(IV) oxide...
RODOX EXAMINATION An oxidation-reduction reaction involves the (1) sharing of electrons (3) transfer of electrons (2) sharing of protons (4) transfer of protons In this reaction, CO→ 2 CO + O2 the oxidation number of carbon changes from: (1) 0 to +4 (3) +3 to 0 (2) +2 to +4 (4) +4 to +2 Which balanced equation represents a redox reaction? AgNO3 (aq) +NaCl (aq) →AgCl (s) +NaNO3 (aq) H2CO3 (aq)...
Classify the following reactions as precipitation reactions, oxidation-reduction reactions, or acid-base reactions. NaCl(aq) + AgNOg(aq) → NaNO3(aq) + AgCl(s) | | BaCl2(aq) + Na2so,(aq) → BaSO4(s) + 2NaCl(aq) 4Al(s)302(g) 2Al,03(s) 2Hgls)+O2(g) 2HgO(sZn(s) Cu2(aq) Zn2+(a)+Cu(s) Mg(OH)2(aq) + 2HCI(aq) → 2H20(l) + MgC12(aq) | | 3KOH(aq) + H,PO,(aq) → K,POdaq) + 31 120(l) Precipitation Oxidation-reduction Acid-base
Redox Equations Which of the following reactions are redox reactions? Identify the substance oxidized, the substance reduced, the oxidizing agent, the reducing agent. 1.2 Mg(s) + O2(g) → 2 MgO (s) 2. H SO. (aq) + Al(OH) (aq) → Al(SO.) (aq) + H,O (1) 3. 2 Na (s) + H2O (1) ► 2 NaOH(aq) + H2(g) 4. Cao (s) + CO2(g) → Caco, (s) 5. AgNO, (aq) + NaCl (aq) ► AgCl(s) + NaNO, (aq) Identify the substance oxidized, the...
1. Provide the oxidation number for each of the underlined elements in following compounds or ions: (6) a) H3AsO3 b) d) H4P207 C202² KCIO4 N2H4 2. Which one of the following is not a oxidation-reduction reaction? (2) A) 2H2(g) + O2(g) → 2H2O(1) B) Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g) C) H2O(l) + NH3(g) → NH(aq) + OH(aq) D) FeSO4(aq) + K2Cr2OH(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) + K2SO4(aq) + 7H2O(1) E) Cl2(g) +2KBr(aq) + Bra(l) + 2KCl(aq)...
Consider a reaction of copper reacting with silver ions in aqueous CuSO4 and AgNO3 solutions Cu(s) + 2 Ag+(aq) -> Cu2+(aq) + 2Ag(s) a) Indicate which substance loses electrons and which substance gains electrons. b) When a substance is oxidized it loses electrons. Write the oxidation half-reaction. c) When a substance is reduced it gains electrons. Write the reduction half-reaction. d) Add the oxidation and reduction half-reactions to give the overall reaction of copper reacting with silver ions. In order...
[References] Balance each of the following oxidation-reduction reactions by using the oxidation states method. (Use the lowest possible coefficients for all reactions.) C.110(9) + 02(9) — CO2(g) + H2O(g) E K(s) + HCl(aq) — K+ (aq) + CI+ (aq) + H2(g) Col+ (aq) + Ni(s) - Co2+ (aq) + Ni2+ (aq) Mg(s) + H2SO4 (aq) MgSO4(aq) + H2(g) 0 Submit Answer Try Another Version 5 item attempts remaining