less than energy in for breaking bonds
more than energy taken in for breaking bonds
equal to the energy taken in for breaking bonds
remains the same as the energy taken in
Explanation
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Exothermic reactions release energy when:
- Bond-making releases more energy than bond-breaking needs
- Usually feels hot, like combustion or neutralization.
Example: CH₄ + O₂ → CO₂ + H₂O + heat 
I dont think there's a correct answer to this MySchool pls review
Option B seems to be correct but its not correct
Or I'm i the one thinking like that
The correct answer is B. more than energy taken in for breaking bonds.Why is this the case?Every chemical reaction involves two distinct energy stages:Breaking Bonds: This requires an input of energy (endothermic process).Making Bonds: This releases energy (exothermic process).In an exothermic reaction, the amount of energy released when new bonds are formed in the products is greater than the energy required to break the bonds in the reactants. This "extra" energy is released into the surroundings, usually as heat, causing the temperature to rise.Summary of Energy ChangesTo help you remember, you can look at the overall enthalpy change ($\Delta H$):Exothermic: Energy Out > Energy In ($\Delta H$ is negative).Endothermic: Energy In > Energy Out ($\Delta H$ is positive).
