Thermochemistry
976213940 | Energy | The capacity to do work. Its formula is =q (heat) +w (work) | |
976213941 | Work | The result of a force acting through distance and its formula is =-P∆V | |
976213942 | Heat | Flow of energy caused by a temperature difference and its formulas =m×Cs×∆T or E+PV | |
976213943 | Kinetic Energy | Energy of motion. | |
976213944 | Potential Energy | Energy associated with position or composition chemical energy. | |
976213945 | Law of Conservation of Energy | Energy can neither be created or destroyed→transferred. | |
976213946 | Kinetic Energy Formula | KE=1/2mv² | |
976213947 | Joule Formula | 1 kgm²/v² | |
976213948 | Calorie | Originally defined as the amount of energy require to raise the T of 1 g of H₂0 by 1°C. | |
976213949 | 1,000 calorie | How many calories are in 1 Calorie? | |
976213950 | 1st Law of Thermodynamics | The total energy of the universe is constant. | |
976213951 | Internal Energy (E) | The sum of the kinetic and potential energies of all of the particles that compose the system. | |
976213952 | The current state | What does the value of a state function depend on? | |
976213953 | Work and heat | What are two things that are not state functions because it matters how they got there? | |
976213954 | It is gained by the surroundings | What happens to energy lost by the system? | |
976213955 | Energy | What can be exchanged with heat and work? | |
976213956 | Heat Capacity | The quantity of heat required to change the T by 1°C. | |
976213957 | Molar Capacity | raise the T of mole by 1°C. | |
976213958 | Pressure-volume work | When the force is caused by a volume change against an external pressure. | |
976213959 | Calorimetry | Measure of the thermal energy of reaction (system) by observing ∆T of the surroundings. | |
976213960 | Bomb Calorimeter | Used for combustion reactions. | |
976213961 | Enthalpy | The sum of a systems internal energy and the product of its pressure and volume. (H) | |
1017809201 | endothermic | The sign for an __________ reaction has a positive ∆H and absorbs heat from the surroundings; feels cold to touch. | |
1017809202 | exothermic | The sign for an __________ reaction has a negative ∆H and gives off heat to the surroundings; feels warm to touch. | |
1017809203 | extensive property | Enthalpy for a reaction of heat is an ___________. | |
1017809204 | multiplied | If a chemical equation is ___________ through by some factor the ∆Hrxn is also multiplied by some factor. | |
1017809205 | sign | If a chemical reaction is reversed, the ∆Hrxn changes _____. | |
1017809206 | sum | If a chemical reaction can be expressed as the sum of a series of steps, then ∆Hrxn for the overall equation is the ____ of the heats of reactions for each step. | |
1017809207 | gases | The standard state for _______ is pure gas at pressure of exactly of 1 atm. | |
1017809208 | liquids or solids | The standard state for _________ the pure substance is in its most stable form at a pressure of atm and T of interest (usually 25°C). | |
1017809209 | enthalpy change | The standard ________ ________ is ∆H° is the change in enthalpy for a process when all reactants and products are in their STD states. | |
1017809210 | pure compound | The standard enthalpy of formation ∆Hf° for a ______ __________ is the change in enthalpy when 1 mole of the compound forms from its constituent elements in their STD states. | |
1017809211 | compound | The standard enthalpy for a pure _______ in its STD state is ∆Hf°=0. | |
1017809212 | standard heat of formation | ∆Hf° is also called... | |
1017809213 | loses | As the system (+) gains thermal energy, the system ______ (-) energy. | |
1017809214 | loses | As work is done on the system (+), the system done by the system ______ energy. | |
1017809215 | flows, out | As energy ______ into the system, energy flows _____ of the system. | |
1017809216 | volume, negative | As ______ increases, work is done on the surroundings, so work should be ________. | |
1023889556 | state function | Internal energy is a ______ _______, which means its value depends only on the state of the system, now on how the system arrived at that state. | |
1023889557 | intensive | Specific heat capacity and molar heat capacity are ________ properties-they depend on the kind of substance being heated, not the amount. |