Chapter 15
False
A process cannot be spontaneous if it is exothermic and there is an increase in disorder.
True
A spontaneous process is a physical or chemical change that occurs with no outside intervention.
a. Calorimeter
An insulated device measuring the heat absorbed or released during a chemical or physical process. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
True
Combustion is the reaction of a fuel with oxygen.
g. Heat of Fusion
Energy required to melt one mole of a substance. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
h. Heat of Vaporization
Energy required to vaporize one mole of a liquid. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
b. Heat of Formation
Enthalpy change occurring when one mole of a compound forms from its elements. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
e. Heat of Combustion
Enthalpy change occurring when one mole of a substance is burned in the presence of oxygen. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
b. solid --> liquid --> gas
For a given substance, the entropy always increases in the following order: a. gas --> liquid --> solid b. solid --> liquid --> gas c. it depends on the substance d. it depends on the pressure
d. temperature and changes in entropy and enthalpy
Free energy change depends on a. change of entropy only b. temperature only c. change of enthalpy only d. temperature and changes in entropy and enthalpy
True
Free energy is the energy that is available to do work for reactions that take place at constant pressure and temperature.
False
Heat is a form of energy that flows from a cold object to a hot object.
c. Specific Heat
Heat required to raise the temperature on of one gram of a substance by 1 degree Celsius. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
False
Potential energy is the energy of motion.
a. first
The _____ law of thermodynamics states that energy is neither created nor destroyed. a. first b. second c. third d. fourth
b. second
The _____ law of thermodynamics states that entropy is always increasing. a. first b. second c. third d. fourth
d. Enthalpy
The amount of heat that is gained or lost during a reaction. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
True
The equation given below is a thermochemical equation. 2Fe(s) + 1.5O2(g) --> 1Fe2O3(s) + 1625 kJ
True
The law of conservation of energy states that energy is neither created nor destroyed.
f. Entropy
The measure of the amount of randomness or disorder in a system. a. Calorimeter b. Heat of Formation c. Specific Heat d. Enthalpy e. Heat of Combustion f. Entropy g. Heat of Fusion h. Heat of Vaporization
False
The symbol "h" is used to represent heat.
True
Thermochemistry is the study of heat changes that accompany chemical reactions and phase changes.
c. q = cXmXeT
What is the equation for calculating heat? a. c = mxqxeT b. m = cxqxeT c. q = cxmxeT d. eT = cxmxq
True
When "delta" G for a reaction is negative, the reaction is spontaneous.
False
When "delta" S for the reaction is negative, the reaction is spontaneous
c. heat energy is being converted to potential energy
When a substance is melting, the temperature of the solid --> liquid mixture stays constant because: a. heat is not being absorbed b. the solid is colder than the liquid c. heat energy is being converted to potential energy d. heat energy is being converted to kinetic energy
b. a measure of the average kinetic energy
Which of the following best describes temperature? a. heat absorbed or released in a chemical or physical change b. a measure of the average kinetic energy c. heat energy d. energy of change
