Thermal energy is best described as:

Energy due to the random motion of particles related to temperature.

Energy stored in chemical bonds.

Energy that cannot be transferred.

Potential energy in chemistry most often refers to:

Energy stored due to position or arrangement, such as in chemical bonds.

Energy due to motion of particles.

Chemical energy specifically refers to:

Energy stored in chemical bonds and released or absorbed during reactions.

Energy due to gravitational position.

Energy associated with electrical circuits only.

Energy that cannot change form.

Which statement aligns with the Law of Conservation of Energy?

Energy can neither be created nor destroyed; it only changes form.

Energy can be created in a closed system.

Energy is destroyed during exothermic reactions.

Energy only exists as heat or work, not both.

A hand warmer reaction that produces heat without light most likely involves which energy transformation?

Chemical energy to thermal energy

Thermal energy to chemical energy

Kinetic energy to potential energy

Electrical energy to chemical energy

Which statement best reflects the First Law of Thermodynamics?

Energy of the universe is constant; it can be transferred or transformed.

Energy can be created from nothing.

Heat flows spontaneously from cold to hot.

Entropy of a perfect crystal at 0 K is zero.

Which device is ruled impossible by the First Law of Thermodynamics?

Perpetual motion machine (of the first kind)

Which option best describes an energy diagram?

A graph showing the relative energies of reactants, products, and transition states

A table listing conversion factors

Which statement best describes the basic principle of energy flow between a system and its surroundings?

Energy is conserved; any energy lost by the system is gained by the surroundings.

Energy can be created within the system and destroyed in the surroundings.

Energy only flows from the surroundings to the system.

Energy flow is independent of the system–surroundings boundary.

In thermodynamics, which sign convention correctly represents heat q when the system absorbs heat from the surroundings?

q alternates sign depending on temperature

Which relationship correctly expresses the connection between the change in energy of the system (ΔE_system) and the change in energy of the surroundings (ΔE_surroundings)?

ΔE_system = −ΔE_surroundings

Which statement aligns with the concept of energy conservation in a closed system boundary?

Total energy change of system plus surroundings equals zero.

Total energy of the system increases without affecting the surroundings.

Total energy of the surroundings decreases regardless of system processes.

Energy conservation applies only to heat, not work.

If the surroundings perform work on the system (compression), what is the sign of w for the system, and how does this affect ΔE_system?

w is positive; ΔE_system increases

w is negative; ΔE_system decreases

w is zero; ΔE_system unchanged

w alternates sign; ΔE_system unpredictable

Considering energy flow principles, which scenario would increase the internal energy of the system?

System absorbs heat and surroundings do compression work.

System releases heat and does expansion work.

System releases heat while surroundings do compression work.

System absorbs heat and does expansion work.

Which statement best captures the relationship between system–surroundings energy changes during any physical or chemical process?

Energy lost by one is exactly gained by the other, maintaining conservation.

The system and surroundings can both gain energy simultaneously without loss elsewhere.

Energy changes are random and cannot be related.

Only heat transfer contributes to energy changes; work does not.

Which statement best defines heat in the context of thermodynamics?

Energy transferred between systems due to a temperature difference

The average kinetic energy of particles in a substance

The absolute measure of hotness on the Kelvin scale

A measure of how much matter an object contains

Which statement best defines temperature?

A measure of the average kinetic energy of particles

Energy in transit between two bodies

The total internal energy of a system

Work done on a system at constant pressure

Thermal equilibrium between two objects implies which condition?

No net heat flow occurs because temperatures are equal

Heat flows from the colder to the hotter object

Their specific heat capacities are identical

What is the general relationship between heat absorbed and temperature change for a given substance?

Heat absorbed is directly proportional to temperature change

Heat absorbed is inversely proportional to temperature change

Heat absorbed is independent of temperature change

Heat absorbed equals the square of temperature change

Heat capacity (C) is best described as which type of property?

Extensive, because it depends on the amount of substance

Intensive, because it does not depend on amount of substance

Neither intensive nor extensive

A spectral property unrelated to thermodynamics

Specific heat capacity (c) is best described as which type of property?

Intensive, because it is defined per unit mass (or per mole)

Extensive, because it scales with the amount of substance

A property that changes with the container size

Which statement correctly distinguishes heat capacity C from specific heat capacity c?

C depends on the total amount of substance; c is normalized per unit mass

C is per unit mass; c is for the whole object

Both C and c are intensive properties

Neither C nor c depends on the substance

Which statement best describes the sign convention for q in thermochemistry?

q is positive when the system absorbs heat from the surroundings

q is positive when the system releases heat to the surroundings

q is negative when the system absorbs heat from the surroundings

A metal sample releases 500 J of heat to water in a calorimeter. Which option correctly characterizes the process for the metal?

Endothermic; q > 0 for the metal

Isothermal; q = 0 for the metal

Complete Conceptual Connection 7.4: Which pair correctly matches the quantity and its definition in thermochemistry?

Heat capacity: energy required to raise the temperature of a system by 1°C

Enthalpy: energy associated solely with work

Entropy: heat absorbed at constant pressure

Latent heat: heat associated with temperature change only

Ch 7 Reading Guide Review

Authored by Barbara Will-Henn

Chemistry

University

NGSS covered

Used 2+ times

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MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which term refers to the study of heat involved in chemical reactions and physical processes?

Thermochemistry

Thermal physics

Electrochemistry

Stoichiometry

Tags

NGSS.HS-PS3-4

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Chemical hand warmers primarily provide which useful product of the reaction?

Electrical current

Light

Heat

Sound

Tags

NGSS.HS-PS3-4

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

When a hand warmer releases heat to its surroundings, the reaction is best classified as:

Endothermic

Exothermic

Isothermal

Athermal

Tags

NGSS.HS-PS3-4

NGSS.HS-PS1-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Which statement best defines energy in the context of chemistry?

Energy is matter that occupies space.

Energy is the capacity to do work or transfer heat.

Energy is any substance dissolved in water.

Energy is the number of particles in a system.

Tags

NGSS.HS-PS3-4

NGSS.HS-PS3-1

NGSS.HS-PS3-2

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Work in thermodynamics is most accurately described as:

Random motion of particles due to temperature.

Force acting through a distance.

Heat transferred at constant pressure.

Potential energy stored in bonds.

Tags

NGSS.HS-PS3-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Heat is:

Energy stored due to position.

Energy associated with the temperature-dependent transfer between system and surroundings.

Energy due to motion of an object as a whole.

Energy released only during nuclear reactions.

Tags

NGSS.HS-PS3-4

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Kinetic energy is primarily associated with:

Position in a field

Chemical bonds

Motion

Temperature difference alone

Tags

NGSS.HS-PS2-1

NGSS.HS-PS2-3

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