Energy Changes in Chemical Reactions

The video tutorial explains the differences between endothermic, exothermic, endergonic, and exergonic processes, focusing on the flow of energy. It discusses potential energy changes in reactions and introduces the concept of free energy, which is the energy available to perform work. A combustion example illustrates energy release, and the tutorial concludes with a discussion on calculating Gibbs free energy, accounting for entropy and temperature.

What is the main difference between endothermic and exothermic processes?

• The temperature change

• The direction of energy flow

• The type of energy involved

• The speed of the reaction

In endothermic reactions, what happens to potential energy?

• It increases

• It decreases

• It is converted to kinetic energy

• It remains constant

What type of energy change is associated with endergonic reactions?

• Thermal energy

• Potential energy

• Kinetic energy

• Free energy

What is a common example of a reaction that releases energy?

• Formation of ice

• Electrolysis of water

• Combustion of hydrocarbons

• Photosynthesis

During a combustion reaction, what happens to potential energy?

• It remains unchanged

• It is converted to light

• It is released as heat

• It is absorbed

What is the role of entropy in energy calculations?

• It increases the total energy

• It decreases the usable energy

• It converts energy to mass

• It has no effect

What does Gibbs free energy account for in a reaction?

• Total energy produced

• Energy lost to the surroundings

• Energy required to start the reaction

• Usable energy after accounting for entropy

Which equation is used to calculate Gibbs free energy?

• E = mc^2

• PV = nRT

• ΔG = ΔH - TΔS

• F = ma

What is the significance of temperature in the Gibbs free energy equation?

• It is irrelevant to the equation

• It affects the potential energy

• It keeps the equation dimensionally consistent

• It determines the speed of the reaction

Why can we never achieve 100% yield in chemical reactions?

• Because of temperature fluctuations

• Due to measurement errors

• Because of entropy

• Due to energy conservation