A thermodynamically unfavorable reaction can become favorable when coupled to a highly reaction. A thermodynamically unfavorable reaction can become favorable when coupled to a highly reaction. Ionic Exergonic Neutral Endergonic

Ionic Exergonic

Explanation:

Exergonic reactions have negative Gibbs free energy and hence are spontaneous.

Endergonic reactions have negative Gibbs free energy and are non-spontaneous and low temperature.

Endergonic reactions require external supply of energy. But such reactions can be made spontaneous or favorable by coupling with exergonic reaction via a common intermediate.

Therefore, the correct answer is Ionic Exergonic.

your picture is not part of the scientific method.

answer: - 3.) the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.

solution: - as per the rules, oxidation number of oxygen in its compounds is -2. the sum of oxidation numbers of all the elements of a molecule or compound is zero.

also, the oxidation number in elemental form is zero.

in no, the oxidation number of o is -2 so the oxidation number of n is +2 so that the sum is zero.

similarly, the oxidation number of c in co is +2 and o is -2.

on product side the oxidation number of n is 0 as it is in the elemental form() .

oxidation number of c in carbon dioxide is +4 as there are two oxygen in it and we know that each oxygen is -2.

so, oxidation number of n is changing from +2 to 0 and the oxidation number of c is changing from +2 to +4.

since nitrogen is reduced and hence no is acting as an oxidizing agent. carbon is oxidized and so co is acting as a reducing agent.

so, the right choice is number 3.)the oxidation state of nitrogen in no changes from +2 to 0, and the oxidation state of carbon in co changes from +2 to +4 as the reaction proceeds.