For the reaction:  Br2 + ClO– → Br– + ClO3– Which species is oxidized?   ClO–   Br2   ClO3– Which species is the oxidizing agent?   ClO–   Br2   Br–

Write a balanced net ionic equation for a redox reaction that results in the formation of potassium chloride. (Assume that potassium chloride is not a starting material, and assume the reaction takes place in aqueous solution.) X, Не (aq), 2K(ag)+Cl, (aq) KCI(aq)

When the following skeletal equation is balanced under basic conditions, what are the coefficients of the species shown? CIO+ 12+ CI Water appears in the balanced equation as a (reactant, product, neither) with a coefficient of (Enter 0 for neither.) Which species is the oxidizing agent?

In the following reaction, what species is the reducing agent?: Ca + Br2 --> CaBr2 Са Br2 This not an oxidation-reduction reaction

Identify the reactant that is being reduced, the reactant that is being oxidized, the reducing agent, the oxidizing agent, and determine how many electrons have been transferred from one atom to another in the following equation.   Al        +         P      →        AlP   Aluminum:         Phosphorus:       Determine the oxidation number of each element in aluminum phosphide.   Al:   P:

2Ag + HPO,²+ H,0→H¿PO,¯ + Ag,0+ OH¯ 2-+ In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent:

How many total electrons are transferred during the reaction of the oxidation of oxidation according to the following reaction? C(s) + O2(g)  -->  CO2(s)

How to tell what element is being oxidized and reduced in a redox reaction with no visible charge in the equation? 2Au(s) + 6HCl(aq) = 2AuCl3(aq) + 3H2(g) 4Fe(s) + 3O2(g) = 2Fe2O3(s)

Which substance is oxidized in each reaction? a) 2Zn(s) + O2(g) = 2ZnO(g)  b) CH4(g) + 2 O2(g) = CO2(g) + H2O(g)    c) Sr(s) + F2(g) = SrF2(s)

For each of the following reactions, identify the elements that are oxidized and reduced, the oxidizing and reducing agents, and how many moles of electrons are transferred in the overall reaction. a. 4Fe(s) + 302(g) → 2Fe2O3(s) b. 2Ag(s) + H2S(g) → Ag2S(s) + H2(g) c. 2 Al(s) + 3 CuCl2(aq) → 2 AlCl3(aq) + 3 Cu(s) d. 2NaHCO3(s) → Na2CO3(s) + H20(1) + CO2(g) e. CH4(g) + 2 02(g) → CO2(g) + 2H2O(1)