Reviewing for a test - need an answer and explanation.

base your answer to the following question on the information below.
the reaction between aluminum and an aqueous solution of gold (i) sulfate is represented by the unbalanced equation below.

al (s) + au2so4 (aq) -> al2(so4)3 (aq) + au (s)

determine the total mass of au sproduced when 6.52 grams of al reacts completely with 3.58 grams of au2so4 to produce 5.95 grams of al2(so4)3.

Temperature is _related to the average kinetic energy of a gas. inversely directly not disproportionally

Oxidation-reduction reactions (often called "redox" for short) are reactions that involve the transfer of electrons from one species to another. oxidation states, or oxidation numbers, allow chemists to keep track of these electron transfers. in general, one element will lose electrons (oxidation), with the result that it will increase in oxidation number, and another element will gain electrons (reduction), thereby decreasing in oxidation number. the species that is oxidized is called the reducing agent or reductant. the species that is reduced is called the oxidizing agent or oxidant. to sum up: oxidation = increase in oxidation state = loss of electrons = reducing agent reduction = decrease in oxidation state = gain of electrons = oxidizing agent part a which element is oxidized in this reaction? fe2o3+3co→2fe+3co2 enter the elemental symbol. view available hint(s) is oxidized part b which element is reduced in this reaction? 2hcl+2kmno4+3h2c2o4→6co2+2mno2+2kcl +4h2o enter the elemental symbol. view available hint(s) is reduced

This image is an example of a(n) a) atom. b) compound. c) mixture. d) molecule.