5314175
Descripción
Fichas por Amelia Claire, actualizado hace más de 1 año
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Creado por Amelia Claire
hace más de 8 años
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| Pregunta | Respuesta |
| Conservation of Energy 1st Law of Thermodynamics | Energy can neither be created nor destroyed - it can only change form The total Energy of the universe is constant = 1st Law of Thermodynamics |
| System | System = part of universe under study (e.g. - chemicals in a flask) |
| Surroundings | Surroundings = the rest of the universe (or as much as needed (e.g. - the flask) |
| Universe | Universe = System + Surrounds |
| Internal Energy | Internal Energy depends on: Temperature Type of material (mass and particles) Amount of material (number of particles) |
| Calculating Thermodynamic Changes | Energy change of a final system = ΔE = E final - E initial |
| ΔE positive : internal energy increases | |
| ΔE negative : internal energy decreases | |
| Heat Capacity | Heat capacity = E required to raise the T(temperature) of an object by 1°C Specific Heat Capacity = E required to heat 1 gram of substance by 1°C Molar Heat Capacity = E required to heat 1 mole of substance by 1°C |
| Specific Heat | Energy required to change Temp of an object is: Heat required = mass x specific heat x ΔTq = m c ΔT or… Heat required = moles x molar heat capacity x ΔT q = n cm ΔT |
| When heat is ADDED to a system | q (heat) is positive the change is endothermic temperature decreases (liquid water boils to become gaseous water) |
| When heat is REMOVED from a system | q (heat) is negative the change is exothermic temperature increases (gaseous water condenses to become liquid water) |
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