Potential energy is due to the composition or position of an object.

The heat required to vaporize one mole of a liquid is called its molar enthalpy of vaporization.

Free energy is the energy that is available to do work for reactions that take place at constant pressure and temperature.

Thermochemistry is the study of heat changes that accompany chemical reactions and phase changes.

Enthalpy is the heat content of a system at constant pressure.

During a chemical reaction, the chemical potential energy of a substance is released as kinetic energy.

Energy is the ability to do work or produce heat.

Energy exists in two basic forms, potential and kinetic energy.

Rusting is not a spontaneous process

A spontaneous process is a physical or chemical change that occurs with no outside intervention.

Chemical systems contain neither kinetic energy nor potential energy.

The kinetic change for a reaction can be calculated by adding two or more thermochemical equations and their enthalpy changes.

In thermodynamics, the universe is defined as the system plus its surroundings.

Potential energy is the energy of motion.

The amount of energy required to raise the temperature of one gram of pure water by one degree Celsius is defined as:

The SI unit of heat and energy is the __________.

What is the equation for calculating heat?

One calorie equals __________ joules.

How much heat is evolved from 54.0 g glucose (C₆H₁₂O₆), according to the equation for calculating heat?

Calculate the enthalpy change of the reaction CH₄ (g) + 2Cl₂(g) CCl₄ (l) + 2 H₂ (g), using thermochemical equations:

When a 50.0-g nugget of pure gold is heated from 35.0°C to 50.0°C, it absorbed 5200.0 J of energy. Find the specific heat of gold.

If molar enthalpy of vaporization of ethanol is 38.6 kJ/mol, how many moles of ethanol are vaporized, when the required heat is 200.72 kJ?

Calculate the enthalpy change of the reaction 2CO(g) + 2NO(g)---> 2CO(g) +N(g) using thermochemical equations: