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Chem Review test9-12
chem review
| Question | Answer |
|---|---|
| Thermodynamics | the study of energy and its transformation form one form to another |
| Energy | the capacity to do work |
| Work | a force acting through a distance |
| First law of thermodynamics | Energy can neither be created nor destroyed, only transferred between the system and its surroundings |
| Thermal Energy | Energy associated with the temperature of an object |
| Chemical Energy | Energy stored in chemical bonds of elements |
| Second law of thermodynamics | For any process to be spontaneous, to occur without outside intervention, energy must be dispersed (energy becomes more spread out in any spontaneous process) |
| Entropy | Energy dispersal |
| Joule | Named after James Joule, energy could be converted from one type to another as long as the total energy was conserved |
| calorie | the amount of energy required to hear 1g of water by 1°C |
| 1cal = How many Joules? | 1cal = 4.18J |
| 1cal = How many Large Calories? | 1cal = 1000Calories (Large “C” for big calories) |
| 1Quad = How many Joules? | 1.06 x 10^18 Joules |
| 1 Kilowatt-hour = How many Joules? | 1 Kilowatt-hour = 3.6 x 10^6 Joules |
| Power | Energy per unit of time. The rate of energy output or input to time (is not energy) power = 1watt or power = 1 joule/sec |
| Temperature | the measure of the kinetic energy associated with the motion of its composite atoms and molecules |
| Fahrenheit scale | 32°F is freezing, and 212°F is boiling (water) |
| Celsius Scale | 0°C is freezing, and 100°C is boiling (water) |
| Kelvin scale | 0K is absolute zero, no negatives |
| Celsius to Kelvin? | K = °C + 273 |
| Fahrenheit to Celsius | °C = 5/9 * [°F – 32] |
| Celsius to Fahrenheit | °F = 9/5 * [°C] + 32 |
| Heat capacity | the quantity of heat energy required to change the temperature of a given amount of the substance by 1 °C |
| Exothermic reactions | Give off energy to the surroundings |
| Endothermic reactions | absorb energy from its surroundings |
| Enthalpy of reaction (∆H [rxn]) | Example: ∆H [rxn] = -49.3 kJ/g CH₄ means that 49.3 kJ are emitted for each gram of CH₄ that is burned |
| Fossil fuels | made mostly of hydrocarbons |
| Natural gas | mixture of methane and ethane |
| Petroleum | large mixture of hydrocarbons |
| Photosynthesis | sunlight + 6CO₂ + 6H₂O → 6O₂ + C₆H₁₂O₆ |
| Greenhouse gasses | CO₂, CH₄ |
| Pressure | an inherent quantity associated with are and the gases that compose it |
| Atmosphere | The layer of air that surrounds the earth |
| Barometers | a device that measures pressure |
| Pressure = ? | Pressure = a / Volume, a is a constant of proportionality |
| P₁ V₁ = ? | P₁ V₁ = P₂ V₂ |
| Relationship between Pressure and temperature | V₁/T₁ = V₂/T₂ |
| Combined Gas law | (P₁ V₁)/T₁ = (P₂ V₂)/T₂ |
| Nitrogen Fixation | the process of breaking N₂ triple bond |
| Respiration | C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O + Energy |
| Troposphere | from ground level to 10km (all life, mountains, and weather) |
| Stratosphere | 10 to 50km, contains the ozone (O₃) |
| Mesosphere | 50 to 80km, and burns up meteors |
| Ionosphere | 80km and up, northern lights, and burns up meteors |
| Chlorofluorocarbons | (CFC’s) a chemical that replaced ammonia and sulfur dioxide in refrigeration and air-conditioning, but prevented the break down of other harmful man made chemicals in the atmosphere |
| Cohesive Forces | Attractions between molecules (holds liquids and solids together) |
| Evaporation | Molecules in a liquid, undergoing constant random motion, may acquire enough energy to overcome attractions with neighbors and fly into the gas phase |
| Crystalline Solids | Solids in which the constituent particles have long-range order |
| Crystalline Structure | The repeating pattern of molecules or atoms |
| Melting point | the point where a solid becomes a liquid |
| Boiling point | When something goes from a liquid to a gas |
| Dispersion | the weakest cohesive force, are the result of small fluctuations in the electron clouds of atoms and molecules. These fluctuations result in instances where electrons are not evenly distributed in the molecule forming an instantaneous dipole |
| London Force | Dispersion |
| Instantaneous dipole | temporary bonds with atoms |
| Permanent dipoles | Strong attractions between atoms and molecules |
| Polar Molecules | have permanent dipoles |
| Molarity: (M) = ? | Molarity: (M) = moles solute / liters solution |
| Parts per million (ppm) = ? | Parts per million (ppm) = (grams solute / grams solution) x 10^6 |
| Milligrams per liter (mg/L) = ? | Milligrams per liter (mg/L) = milligrams solute / liters solution |
| Flash freezing | quickly freezing organic things to keep the water in them from expanding too much and causing cell rupture. |
| Blue Baby | when a baby ingests nitrates and affects the hemoglobin in the baby’s blood causing the baby to look bluish |
| Water Treatment process | Public water treatment: Reservoir → Wire Mesh Screen → Coagulation → Settling tank → Sand or Gravel Filtration → Activated Carbon Filtration or Aeration →Chlorination |
Created by:
Foxman
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