Understanding Thermodynamics

What does the system refer to in thermodynamics?

• The entire universe

• The part of the universe that is not being studied

• The part of the universe that we are studying

• Only the kinetic energy of particles

What does 'delta E' represent in the first law of thermodynamics?

• The change in external energy of the system

• The total energy of the universe

• The work done by the system

• The change in internal energy of the system

If heat flows into the system from the surroundings, how is 'q' defined?

• Negative

• Positive

• Zero

• Undefined

What does a negative 'delta H' indicate?

• An endothermic process

• No change in enthalpy

• The system is at equilibrium

• An exothermic process

What is the change in internal energy if 6000 joules of heat is added to the system and 2000 joules of work is done by the system?

• 4000 joules

• 8000 joules

• 2000 joules

• 0 joules

What signifies an exothermic process in a chemical reaction?

• Absorption of heat from the surroundings

• Release of heat to the surroundings

• No change in temperature

• Decrease in kinetic energy

How is work ('w') defined when it is done by the system on the surroundings?

• Negative

• Zero

• Undefined

• Positive

What does the first law of thermodynamics, delta E = q + w, fundamentally represent?

• Conservation of mass

• Conservation of energy

• Increase in entropy

• Decrease in system's energy

In the context of thermodynamics, what are the surroundings?

• Only the immediate area outside the system

• Only living organisms around the system

• Everything in the universe except the system

• The container holding a system

What does a positive change in enthalpy (delta H) indicate?

• The system is losing heat

• An endothermic process

• No change in the system's energy

• An exothermic process