Reaction type of a question that i don t know

hrough a series of redox reactions involving water and oxygen, the ultimate reaction is Fe (iron) + O2 (molecular, elemental oxygen) Yields Fe2O3 (red rust). The charge of iron in rust is +3; the charge of oxygen in rust is -2. a. What is the charge of metallic iron? Atmospheric oxygen? How do you know? b. What is oxidized in this reaction? What is reduced? 7. In raku firing of ceramics, a piece of clay is formed, then glazed, often with some type of copper, iron, cobalt, or other metallic compound. The product is removed hot from the kiln and placed in a container of sawdust, leaves, or other combustible materials. The burning quickly consumes all the oxygen, and produces a “reductive” environment. You know that the half reaction: Cu yield Cu+2 + 2 e- is an oxidation. a. Write this in reverse to show what happens to the copper ions in glazes in a reductive environment. Explain, then, why raku firing yields interesting effects.

hrough a series of redox reactions involving water and oxygen, the ultimate reaction is Fe (iron) + O2 (molecular, elemental oxygen) Yields Fe2O3 (red rust). The charge of iron in rust is +3; the charge of oxygen in rust is -2. a. What is the charge of metallic iron? Atmospheric oxygen? How do you know? b. What is oxidized in this reaction? What is reduced? 7. In raku firing of ceramics, a piece of clay is formed, then glazed, often with some type of copper, iron, cobalt, or other metallic compound. The product is removed hot from the kiln and placed in a container of sawdust, leaves, or other combustible materials. The burning quickly consumes all the oxygen, and produces a “reductive” environment. You know that the half reaction: Cu yield Cu+2 + 2 e- is an oxidation. a. Write this in reverse to show what happens to the copper ions in glazes in a reductive environment. Explain, then, why raku firing yields interesting effects.

d lead (II) sulfate precipitates (a) Write a balanced chemical equation for the reaction (b) Write the net ionic equation for the reaction (c) What type of reaction is occurring? (d) What is the limiting reagent? The excess reagent? (e) How many grams of lead (II) sulfate are formed? (f) In the lab, a chemistry student mixed the two solutions together and formed 9.40 g of lead (II) sulfate. What percent yield did the student obtain?