Question | Answer |
The transfer of thermal energy between two bodies that are different temperatures | Heat |
________ is the measure of thermal energy | Temperature |
What is energy | Energy is the capacity to do work |
Energy that comes from the sun and is earth's primary energy source | Radiant energy |
Energy that is associated with the random motion of atoms and molecules | Thermal energy |
Energy that is stored within the bonds of chemical substances | Chemical energy |
Energy that is stored within the collections of neutrons and protons in the atom | Nuclear energy |
Energy that is available by virtue of an object's position | Potential energy |
Thermochemistry | The study of heat change in chemical reactions |
System | The specific part of the universe that is of interest in the study |
Endothermic process | Any process in which heat has to be supplied to the system from the surroundings |
Exothermic process | Any process that gives off heat transfers thermal energy from the system to the surroundings |
Thermodynamics | The scientific study of the interconversion of heat and other kinds of energy |
State function | Properties that are determined by the state of the system, regardless of how that condition was achieved. |
Heat given off by the system to the surroundings | Exothermic |
Heat absorbed by the system from the surroundings | Endothermic |
First law of thermodynamics | Energy can be converted from one form to another, but can not be created or destroyed |
Chemical energy lost by combustion= | =energy gained by the surroundings |
Enthalpy(H) | Used to quantify heat flow into or out of a system in a process that occurs at constant pressure |
Heat given off or absorbed during a reaction at constant pressure | Enthalpy |
The stoichiometric coefficients always refer to the number of ______ of a substance | Moles |
Specific heat (s) of a substance | The amount of heat (q) required to raise the temperature of one gram of the substance by one degree celsius |
Heat capacity (C) of a substance | The amount of heat required (q) to raise the temperature of a given quantity (m) of the substance by one degree Celsius |
Hess law | When reactants are converted to products, the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps |
Lattice Energy (U) | The energy required to completely separate one Mile of a solid ionic compound into gaseous ions |
Heat of Hydration | The enthalpy change associated with the hydration process |
Heat of Dilution | Heat change associated with the dilution process |
Thermodynamics | Scientific study of the interconversion of heat and other kinds of energy |
State of a system | The value of all relevant macroscopic properties such as: composition, energy, temperature, pressure, volume, etc |
State functions (E, P, V, T) | Properties that are determined by the state of the system regardless of how that condition was achieved |
First law of thermodynamics | Energy can be converted from one form to another, but cannot be created or destroyed (Law of conversation of energy) |
Work (w) | Force times distance
Fâ¢d |
Energy | The capacity to do work |
Law of conservation of energy | The total quantity of energy in the universe is assumed constant |
Heat | The transfer of thermal energy between two bodies that are at different temperature. Heat flows from "hot" object to "cold" object. Heat can be either absorbed or released. |
Open system | Can exchange mass and energy, usually in the form of heat, with its surrounding |
Closed system | Allows only energy transfer (not mass) between system and surrounding |
Isolated system | No heat nor mass exchange between system and surrounding |
Surrounding | The rest of the universe outside the system |
Extensive property
Can't be measured directly | Enthalpy |
Enthalpy of reaction | H > 0 endothermic
H < 0 exothermic |
Calorimetry | The measure of heat exchanges |
The amount of heat (q) | Is equal to the product of the mass of the object and its specific heat times the change of its temperature |
Standard state | P= 1atm
T= 25â¢c |
Standard enthalpy of formation | The heat change that results when one mole of a compound is formed from its elements at 1atm pressure |
Avogadros law | At a constant temperature & pressure the volume of a gas is directly proportional to the amount of gas particles |
Real gas | Doesn't behave like ideal gases due to the interaction between the molecules & gas molecules regardless of size, has infinitesimal volume. They behave according to the van der waals equation |
Charles law | For a fixed amount of gas at constant pressure the volume of the gas is directly proportional to the temperature of the gas |
Ideal gas law | Hypothetical gas where P-V-T behavior can be completely accounted for by the ideal gas equation |
STP
Standard Temperature & Pressure | R = PV/nT
P= 1atm
V= 22.414l
n= 1mol
T= 273.15k |
Boyles Law | For fixed amount of gas at constant temperature the volume of the gas is inversely proportional to the pressure of the gas |
T/F
For any endothermic process, the temperature of the surrounding is warmer than the system | False |
T/F
In all electromagnetic radiations, those having high frequencies would also have large wavelengths | False |
T/F
According to the quantum numbers, there is a "4d" orbital | True |
T/F
At constant pressure, the reaction: 2NH3(g)----> 3H2(g)+N2(g) is a system that does work on the surrounding | True |
T/F
Specific heat is the amount of heat required to raise the temperature of a given quantity of substance by 1â¢c | False |
T/F
For a given element, the size of its cation is generally smaller than its anion | True |
T/F
Given the specific heat of aluminum is 0.900 J/gâ¢c and iron is 0.444J/gâ¢c. It would take longer to raise the temperature of iron by 1â¢c than that of aluminum under the same heat condition | False |
T/F
Nitrogen has five valence electrons | True |
T/F
The ground state of an electron in an element is when the electron is most stable | True |
T/F
Despite the fact boron and magnesium are in different groups, it is found that they have many similarities in their chemical behaviors. | False |