g Identify the oxidizing agent and the reducing agent in the following reaction. 2KMnO4(aq) 10FeSO4(aq) 8H2SO4(aq) --> K2SO4(aq) 2MnSO4(aq) 5Fe2(SO4)3(aq) 8H2O(l) A. KMnO4oxidizing agent, FeSO4 reducing agent B. H2SO4 oxidizing agent, FeSO4 reducing agent C. FeSO4 oxidizing agent, H2SO4reducing agent D. FeSO4 oxidizing agent, KMnO4reducing agent E. K2SO4 oxidizing agent, H2O reducing agent

A. KMnO₄oxidizing agent, FeSO₄ reducing agent

Explanation:

In chemical reactions, we have both oxidizing and reducing agents. This chemical reaction is referred to as Redox reaction.

Oxidizing agents or compounds can be defined as compounds that accepts or receives electrons from other compounds and this results in the oxidation of those other compounds. When oxidizing agents accept electrons from other agents, they are reduced. Oxidizing agents are also referred to as electron acceptors.

Reducing agents can be defined as agents or compounds that lose their electrons to other compounds or agents and they reduce those other compounds. When reducing agents lose electrons, they are oxidized in the process. Reducing agents are also called or referred to as electron donors.

In the question, above we were asked to identify the oxidizing and reducing agents.

a) The oxidizing agent in the chemical equation above is KMnO₄(aq). It is an oxidizing agent because in the chemical equation above, it has been reduced to 2MnSO₄(aq).

b) The reducing agent in the chemical equation above is FeSO₄(aq). It is a reducing agent because in the chemical reaction above,  it has been oxidized to 5Fe₂(SO4)₃(aq).

answer: enthalpy

explanation:

for a exothermic reaction, the energy is released i.e. the energy of the products is lower than the energy of the reactants.

= enthaply

= energy of products

= energy of reactants

as , thus comes out to be negative. negative value of enthalpy shows that the reaction is exothermic.