6.Balance the given skeleton reaction: O2(g) + NO(g) + H₂O(l) → NO3¯¯(aq) + H+ (aq) A. 2,4,3,4,4 B. 2,3,4,4,4 C. 3,4,2,4,4 D. 3,2,3,4,4

8 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?

Balance the following using the half-reaction method. Identify oxidation, reduction, reducing agent, oxidizing agent. i. Be(NO3)2 (aq) + Ce(s)--> Ce(NO3)3(aq) + Be(s) ii. A container contains H2SO3, H2SO4, Pb2+, Pb4+ and NO3- in distilled water. Create a balanced chemical reaction (Net Ionic Equation, including states of matter) for the spontaneous reaction in the container

Balance the following Redox Reaction. Always include the state of each species: (s), (l), (g), or (aq). O2(g) + Sb(s) → H2O2(l) + SbO2-(aq) (basic) Format:  A. Write the Balanced Oxidation Half Reaction B. Write the Balanced Reduction Half Reaction C. What is the Reducing agent? Oxidizing agent? D. Write the overall balanced equation.

1- Balance the following redox reactions using the oxidation number method a. NaClO + H2S = NaCl + H2SO4 b. Sn + HNO3 + H2O = H2SnO3 + NO   2- Balance the following redox reactions using the half-reaction method. a. Mg + Al+3 = Mg+2 + Al b. H2O2 + Cr2O72- = O2 + Cr+3 (in acidic solution)   2.Rank the following entities in order of increasing strength as oxidizing agents. (1=weakest oxidizing agent and 6= strongest oxidizing agent) Cd+2(aq)                   IO3-1(aq)                 K+1(aq)                       H2O(l)                    AuCl4-1(aq)                     I2(s)   3. Indicate which of the following pairs of substances, when combined, will result in a spontaneous chemical reaction. Write spontaneous or non-spontaneous. a.    K+1(aq) and Na(s)                   b.   Cr+2(aq) and K(s)                   c.    Pb+2(aq) and Fe(s)           d.   Ag(s) and Sn+2(aq)

Complete and balance the reaction between calcium carbonate and hydrochloric acid. Then give the correct product side of the reaction. Choose one: a. → CaCl2 (aq) + H2CO2 (aq) b. none of these c. → CaCl2 (aq) + H2O (l) + CO2 (g) d. → 2 CaCl (aq) + H2CO2 (aq)

For the following redox reactions, please balance them in basic solution and indicate the impactof pH on the reaction (e.g., lower pH favors, disfavors, has no effect on the reaction).

Identify the reducing and oxidizing agents and determine the species that is oxidized and the species that is reduced. Mg Fe2+ Mg 2+ a. Fe b. Cu2+ Sn Sn2+ Cu с. H2 CH2=CH2 CH3CH3 Reducing agent Oxidizing agent Species being reduced Species being oxidized

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A. +2 13. In the reaction, 2H₂ (g) + O₂ (g) → 2H₂O (g), which of the following is the oxidizing agent? C. H₂O B. 0₂ A. H₂ D. None of the choices 14. In the reaction, 2H₂ (g) + O₂(g) → 2H₂O (g), which of the following is the reducing agent? C. H₂O A. H₂ B. 02 D. None of the choices 15. What are the original and final oxidation numbers for iron in the smelting of iron from iron oxide? Fe2O3(s) + 3CO(g) → 2Fe(s) + 3C02(g) C.0 +2 A. +2 0 B. +3-0 D. No change 16. A reducing agent reduces other substances and loses electrons; therefore, its oxidation state will C. stay the same B. increase A. decrease ? D. none of the choices 17. A monoatomic ion has an oxidation state equal to its charge. What is the oxidation state of Ca²+? A. +2 B. +1 C.0 D.-2 18. In the reaction, Fe2O3 (1) + CO (g) → Fe (I) + CO2 (g), how many electrons does Fe gain? A. 1 B. 2 C. 3 D. 4 19. In the reaction, Fe2O3 (1) + CO (g) → Fe (1) + CO2 (g), how many electrons does Fe gain? A. 1 B. 2 C. 3 D. 4 20. Which of the…