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Chemistry Chpt. 6
vitamins
| 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 |
Created by:
Capty103
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