Chem 2 4th Quarter Exam

In an endothermic process, the enthalpy change (∆H) is:

• 1. Positive

• 1. Negative

• 1. Zero

• 1. Undefined

At the start of a reversible process, the reaction proceeds towards the formation of:

• Reactants

• Products

• Equilibrium

• Catalysts

Enthalpy change (∆H) is a measure of:

• The energy transferred as heat during a process

• The work done by the system on the surroundings

• The change in the number of moles of gas in a reaction

• The change in temperature of the system

The analogy of a bank balance is used to explain enthalpy change because:

• It helps us understand state functions

• It simplifies the concept of enthalpy

• It demonstrates the relationship between pressure and volume

• 1. It emphasizes the importance of constant pressure conditions

In a chemical reaction, if the change in internal energy is negative, it indicates that:

• Energy is conserved

• Energy is released

• Energy is absorbed

• 1. Energy is converted

The change in internal energy of a system is directly related to:

• The mass of the system

• The volume of the system

• The temperature of the system

• The pressure of the system

How is the spontaneity of a reaction determined?

• By calculating the change in system entropy (ΔSsys).

• By calculating the change in surroundings entropy (ΔSsurr).

• By calculating the change in system enthalpy (ΔHsys).

• By calculating both ΔSsys and ΔSsurr.

What is the function of Gibbs free energy (G)?

• It determines the entropy change of the universe.

• It determines the spontaneity of a reaction in the system.

• It determines the enthalpy change of the system.

• It determines the temperature of the system.

The standard entropy of reaction (ΔS°rxn) is also known as:

• Heat of reaction

• Enthalpy of reaction

• Gibbs free energy change

• Entropy change of the system

Which of the following can be negative in a spontaneous process?

• 14. ΔSuniv

• 14. ΔSsys

• 14. ΔSsurr

• 14. Both ΔSsys and ΔSsurr