Q1) Which of the following is a state function in thermodynamics?

a) Heat

b) Work

c) Enthalpy

d) Entropy

Q2) The First Law of Thermodynamics is a statement of conservation of:

a) Mass

b) Energy

c) Momentum

d) Entropy

Q3) The change in internal energy of a system is given by:

a) ΔU = q + w

b) ΔU = q - w

c) ΔU = q / w

d) ΔU = q * w

Q4) The SI unit of entropy is:

a) Joule (J)

b) Kelvin (K)

c) Joule/Kelvin (J/K)

d) Joule/Kelvin/Mole (J/K/mol)

Q5) The entropy of a perfect crystal at absolute zero temperature is:

a) Zero

b) Infinite

c) Constant

d) Negative

Q6) The entropy change for a reversible process is:

a) Always positive

b) Always negative

c) Always zero

d) Can be positive, negative, or zero

Q7) The Gibbs free energy equation is:

a) ΔG = ΔH - TΔS

b) ΔG = ΔH + TΔS

c) ΔG = ΔH / ΔS

d) ΔG = ΔH * ΔS

Q8) For a spontaneous process at constant temperature and pressure, the change in Gibbs free energy is:

a) Negative

b) Positive

c) Zero

d) Cannot be determined

Q9) The equilibrium constant (K) for a reaction is related to the standard Gibbs free energy change (ΔG°) by:

a) ΔG° = -RTln(K)

b) ΔG° = RTln(K)

c) ΔG° = -ln(K)

d) ΔG° = ln(K)

Q10) The standard entropy change (ΔS°) of a reaction can be calculated using:

a) ΔS° = ∑S(products) - ∑S(reactants)

b) ΔS° = ∑S(reactants) - ∑S(products)

c) ΔS° = ∑S(products) + ∑S(reactants)

d) ΔS° = ∑S(reactants) + ∑S(products)

Q11) A reaction will be spontaneous at all temperatures if:

a) ΔH is positive and ΔS is negative

b) ΔH is negative and ΔS is positive

c) ΔH is negative and ΔS is negative

d) ΔH is positive and ΔS is positive

Q12) The Clausius-Clapeyron equation relates:

a) Enthalpy and entropy

b) Pressure and volume

c) Temperature and volume

d) Temperature and pressure

Q13) A process is reversible when:

a) No energy is lost to the surroundings

b) The system is at equilibrium with the surroundings

c) The process occurs at constant temperature and pressure

d) The process occurs without any change in entropy

Q14) Hess's Law is based on the principle of:

a) Conservation of mass

b) Conservation of energy

c) Conservation of entropy

d) Conservation of enthalpy

Q15) A reaction is said to be exothermic when:

a) It releases heat to the surroundings

b) It absorbs heat from the surroundings

c) It releases work to the surroundings

d) It absorbs work from the surroundings

Q16) The term "adiabatic" refers to a process that occurs:

a) At constant temperature

b) Without any change in volume

c) Without any exchange of heat with the surroundings

d) Without any change in pressure

Q17) The enthalpy change for a reaction is independent of:

a) Pressure

b) Temperature

c) Volume

d) All of the above

Q18) The standard state conditions for a substance typically include:

a) 1 atm pressure and 0°C temperature

b) 1 atm pressure and 25°C temperature

c) 0 atm pressure and 0K temperature

d) 0 atm pressure and 100°C temperature

Q19) The heat capacity of a substance is defined as the amount of heat required to raise the temperature of:

a) 1 mole of the substance by 1°C

b) 1 gram of the substance by 1°C

c) 1 mole of the substance by 1K

d) 1 gram of the substance by 1K

Q20) The enthalpy change associated with a chemical reaction can be determined experimentally using:

a) Calorimetry

b) Spectroscopy

c) Titration

d) Chromatography