Thermodynamics and Equilibrium Concepts

The video tutorial covers the concepts of formation reactions, focusing on the calculation of delta H and delta G. It explains the importance of balancing equations for one mole and how to calculate the entropy change (delta S) using the Gibbs free energy equation. The tutorial also discusses the effect of temperature on the spontaneity of reactions, emphasizing the role of the T delta S term. Finally, it explores the relationship between equilibrium constants and temperature, providing a comprehensive understanding of these thermodynamic principles.

What is the enthalpy change (ΔH) for the formation of NH3 when the reaction is balanced for one mole?

• Negative 46.2 kJ

• Positive 46.2 kJ

• Negative 92.4 kJ

• Positive 92.4 kJ

How do you calculate the free energy change (ΔG) for the reaction when the coefficients are doubled?

• Multiply ΔG by 0.5

• Multiply ΔG by 2

• Add 10 to ΔG

• Subtract 10 from ΔG

What is the unit typically used for reporting entropy change (ΔS)?

• Kilojoules per mole

• Joules per mole Kelvin

• Kilojoules per Kelvin

• Joules per Kelvin

Which equation is used to calculate the entropy change (ΔS) from ΔH and ΔG?

• Gibbs Free Energy Equation

• Charles's Law

• Ideal Gas Law

• Boyle's Law

What happens to the Gibbs free energy (ΔG) when the temperature increases and both ΔH and ΔS are negative?

• ΔG becomes zero

• ΔG becomes more positive

• ΔG remains unchanged

• ΔG becomes more negative

How does an increase in temperature affect the spontaneity of a reaction with negative ΔH and ΔS?

• The reaction remains equally spontaneous

• The reaction becomes less spontaneous

• The reaction becomes more spontaneous

• The reaction becomes non-spontaneous

What is the equilibrium constant (K) when the partial pressures of all gases are one atmosphere?

• K = -1

• K = 0

• K = 1

• K = 10

At what temperature does the Gibbs free energy (ΔG) become zero for the reaction?

• 500 K

• 273 K

• 467 K

• 298 K

What is the relationship between ΔG and the equilibrium constant (K) when K equals 1?

• ΔG is zero

• ΔG is undefined

• ΔG is negative

• ΔG is positive

Which of the following is true when ΔG is zero?

• The reaction is non-spontaneous

• The reaction is at equilibrium

• The reaction is spontaneous

• The reaction rate is maximum