Chemical Reactions and Energy Concepts

How do we measure changes in internal energy?

• As temperature

• As enthalpy

• As volume

• As mass

What is the formula for the change in enthalpy (ΔH)?

• ΔH = HEAT of REACTANTS - HEAT of PRODUCTS

• ΔH = HEAT of PRODUCTS + HEAT of REACTANT

• ΔH = HEAT of PRODUCTS - HEAT of REACTANTS

• ΔH = HEAT of REACTANTS + HEAT of PRODUCTS

What does ΔH largely represent a change in?

• Kinetic energy

• Potential energy

• Chemical energy

• Electrical energy

What does the equation "Total or Internal Energy = KE + PE" represent?

• The relationship between kinetic and potential energy

• The formula for calculating force

• The equation for gravitational potential energy

• The principle of conservation of mass

What does "KE" stand for in the context of energy?

• Kinetic Energy

• Kilo Energy

• Key Energy

• Known Energy

In the equation "Total or Internal Energy = KE + PE," what does "Total or Internal Energy" refer to?

• The sum of kinetic and potential energy

• The difference between kinetic and potential energy

• Only kinetic energy

• Only potential energy

Which of the following is an example of kinetic energy?

• A rolling ball

• A book on a shelf

• A compressed spring

• A charged battery

What does the term "system" refer to in a chemical reaction?

• The entire universe.

• Only the reactants.

• The part of the universe being studied.

• Only the products.

What is the role of the surroundings in a chemical reaction?

• They are part of the system.

• They are not involved at all.

• They exchange energy with the system.

• They become products.

Which of the following is a characteristic of endothermic reactions?

• Release of heat.

• Absorption of heat.

• No change in energy.

• Increase in pressure.