Energy, Thermodynamics, and Chemical Reactions

A set of flashcards summarizing key concepts from the lecture on energy, thermodynamics, and chemical reactions, designed to aid in exam preparation.

What is thermodynamics?

The study of energy transporters and how reactions are motivated to happen.

What happens to potential energy as a rock falls down a hill?

As the rock falls, it gains maximum kinetic energy and has high potential energy at the top.

What is electrostatic potential energy associated with?

It is associated with charged particles and their interactions.

How does the distance affect electrostatic potential energy?

It is inversely proportional; as distance decreases, potential energy increases.

What defines a positive balance in the context of a credit card analogy?

A positive balance means you owe money, which is less stable compared to having a negative balance.

What are the two main forms of energy?

Kinetic energy and potential energy.

What is considered endothermic in a thermodynamic system?

When the system absorbs heat, leading to an increase in temperature of the surroundings.

What is exothermic?

When the system releases heat, leading to a decrease in temperature of the surroundings.

What does the formula for electrostatic interactions depend on?

It depends on the magnitudes of the charges and the distance between them.

What do we measure internal energy as a function of?

Internal energy is considered a state function that changes based on initial and final states.

What is enthalpy defined as?

Enthalpy is internal energy plus the product of pressure and volume.

How do you calculate work done by a gas?

Work is calculated using the formula: work = -PΔV.

What happens when a gas expands in a piston?

The system does work, which is considered negative.

What is the significance of having different signs for heat and work in a thermodynamic process?

The signs influence whether the internal energy has a net gain or loss based on heat and work interactions.

What is the importance of internal energy being a state function?

It indicates that only the initial and final states matter, not the path taken during the process.

What is the role of kinetic and potential energy in chemical reactions?

These energies affect the stability and favorability of reactants and products.

How does the behavior of particles in a closed system influence energy exchange?

The energy exchange depends on heat transfer and work done between the system and surroundings.

In a thermodynamic context, what does a negative internal energy change indicate?

It indicates that the system has lost energy.