In the redox reaction below, which is the reducing agent? cl- cl2 mn2+ mno2

            Cl⁻ is the reducing agent.

Explanation:

The redox reaction is as follow:

                    MnO₂  + 4H⁺ + 2Cl⁻   →   Mn²⁺ + 2H₂O + Cl₂

One should know the following terms,

Reducing agent:

                          An atom or element which tends to lose electron during a chemical reaction and get itself oxidized. In above reaction Cl⁻ is reducing agent as it carries a negative charge (means it has one extra electron) on the reactant side while, it has zero oxidation state on the product side. It means going from -1 to 0 the Cl lost one electron hence, it is an reducing agent according to definition.

Oxidizing Agent:

On the other hand oxidizing agent is an element or compound which tends to accepts electron(s) and get itself reduced. In above reaction Mn has an oxidation state of +4 on reactant side and after gaining electron from Cl it has changed to +2 on the product side. Hence, it has reduced but has oxidized the Cl atom so it is an oxidizing agent according to definition.

false

because it does not have the potential to be entirely used up

"standard molar enthalpy:

h2o ( liquid water ) : - 285.8 kj/mole

h2o ( water vapor ) : - 241.8 kj / mole.

δhrxn = - 241. 8 - ( - 285.8 )= -241.8 + 285.8 = 44.0

answer: 44.0 kj"