Practise MYP Chemistry questions on 5.16 Endothermic and Exothermic Reactions and review the explanations to check your understanding.
Use these questions for topic practice and to find ideas you want to revisit in your notes or lessons.
True or False: The products of an endothermic reaction are generally more energetically stable than the reactants because they have absorbed energy.
In an endothermic reaction, which statement correctly describes the bond energy balance?
True or False: In an exothermic reaction, the chemical system contains less enthalpy after the reaction than it did before.
![ Energy profile diagram where the reactant energy level is at , the peak of the curve is at , and the product energy level is at . ] Based on the diagram description, what is the value of the enthalpy change ()?
When considering the evaporation of sweat from a thermodynamic perspective, why does the skin feel cooler?
True
False
No energy is required to break bonds, and energy is only released during formation
The energy required to break bonds in the reactants is less than the energy released when forming bonds in the products
The energy required to break bonds in the reactants is greater than the energy released when forming bonds in the products
The energy required to break bonds is exactly equal to the energy released during formation
True
False
Evaporation is an exothermic process that lowers the local temperature
The sweat molecules release energy to the skin as they turn into a gas
The chemical bonds within the water molecules are being broken, which is exothermic
The liquid sweat absorbs heat energy from the skin to overcome attractive forces
