Question

A certain chemical reaction's reactants have an energy of 1,341 kJ/mol and the products have an energy of 1,646 kJ/mol. Is this reaction endothermic or exothermic? What is the best explanation for your choice?(1 point) Responses Endothermic, because product energy minus reactant energy is +305 kJ/mol and energy is put in. Endothermic, because product energy minus reactant energy is +305 kJ/mol and energy is put in. Exothermic, because the product's energy is higher so the energy change will be -305 kJ/mol and energy is released. Exothermic, because the product's energy is higher so the energy change will be -305 kJ/mol and energy is released. Endothermic, because the product's energy is higher so energy went in. Endothermic, because the product's energy is higher so energy went in. Exothermic, because the reactant + the product energy is 2,987 kJ/mol.

Answer 1

The correct response is:

Endothermic, because product energy minus reactant energy is +305 kJ/mol and energy is put in.

Here's the reasoning:

1. Energy of Reactants vs. Products: The reactants have an energy of 1,341 kJ/mol, and the products have an energy of 1,646 kJ/mol.

2. Calculating Energy Change: The change in energy (ΔE) is calculated as: \[ \Delta E = \text{Energy of products} - \text{Energy of reactants} = 1,646 , \text{kJ/mol} - 1,341 , \text{kJ/mol} = +305 , \text{kJ/mol} \]

3. Interpretation of Energy Change: Since the value is positive (+305 kJ/mol), it indicates that energy was absorbed from the surroundings during the reaction.

4. Conclusion: Therefore, this reaction is endothermic because energy is taken in to convert the reactants into products, resulting in a higher energy state for the products.