For the energy diagram of the chemical reaction depicted here, which statement is the best conclusion?

The overall reaction releases energy.

The overall reaction absorbs energy.

The activation energy is not represented on the graph.

The reaction will proceed without the input of energy.

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Explanation:

What is shown is a Potential Energy Diagram for an endothermic reaction. Note the beginning and ending potential energy values. The final energy value is greater than the initial energy value and means that the final products of the reaction have gained energy.

For your questions...

The overall reaction does NOT release energy, if fact the final products have more energy than did the reactants before reaction.

Yes, the overall reaction absorbs energy as indicated by the position of the graph energy values on the high end of the Reaction Progress.

The Activation Energy is, in fact, at the top of the transition curve and is also referred to as the Activation Complex.

All chemical processes require an amount of input energy - called the Activation Energy - in order to form products. All reactants BELOW this Activation Energy WILL NOT react. So in this case, the reaction WILL NOT proceed without the input of energy; or, in other words, ya gotta put some energy into the reactants to lift them to the activation point at the top of the curve.

they are both synthetic elements

explanation:

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