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Definition
| The Study of energy and it's transformations |
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| Energy change that occurs during chemical reaction involving heat |
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| refers to the capacity to do work, that is to move or displace matter |
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| energy used to cause an object with mass to move |
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| Potential Energy Equation |
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Definition
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Definition
System: Includes the molecules we want to study
Surroundings: Are everything else |
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| First Law of Thermodynamics |
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Definition
- Energy cannot be created or destroyed
-The energy of a system and surroundings is constant
-Any energy transferred from a system must be transferred to the surrounding and vice/versa |
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Definition
The sum of all the kinetic and potential energies of the components of the system
- delta E=Efinal-Einitial |
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| When Energy is Exchanged between the system and the surroundings it is exchanged as either (q) or work(w) |
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Definition
| -equation: Change in E= q+w |
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| Thermodynamic quantities have 3 parts |
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Definition
| number, unit, & a sign that gives them a direction |
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Definition
| -When a system absorbs heat, causing the kinetic energy to go up |
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Definition
| -When the system loses heat |
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| Pressure-Volume Work (p-v work) |
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Definition
The work involved in the expansion of gases
- w=-PdV |
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Definition
the Heat (q) transferred between the system and the surroundings during a chemical reaction carried out under constant pressure, often referred to as "heat content"
- at a constant pressure, the change in enthalpy equals the heat gained or lost |
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Definition
- Is the internal energy plus the product of pressure & volume of the system
dH=dE+PdV
-dH is the change in enthalpy |
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| Standard Enthalpies of a Reaction |
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Definition
| Is the enthalpy change for a reaction in which the reactants in their standard states yield products in their standard states |
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| Equation for Bomb Calorimetry |
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Definition
| qrxn=-Ccal*Change in Temp |
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| In bomb calorimetry since the reaction is carried under constant volume what are we measuring really instead of the the change in H. (Enthalpy) |
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Definition
- We are measuring dE, the internal energy
-dE=qv |
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| What's another name for Bomb Calorimetry? |
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Definition
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| What type of Calorimeter is used when the volume is constant |
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Definition
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| For bomb calorimetry what is the most common type of reaction being studied? |
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Definition
| Under these conditions the most common type of reaction is combustion. |
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Definition
| Amount of energy required to raise the temperature of an object by 1 K (1 degree celsius) J/k |
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| The Heat Capacity (Cm)(molal capacity) |
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Definition
| Is 1 mol of a substance that is the molal heat capacity (cm) |
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| The specific heat capacity of |
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Definition
| 1g of a substance is the specific heat capacity or specific heat |
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What is calorimetry?
What is a calorimeter |
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Definition
It is the measure of heat flow
It is an apparatus that measures heat flow |
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Definition
| (quantity of heat transferred)/(grams of substance)(temperature change) |
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Term
| Constant pressure calorimeter |
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Definition
| - measures change in enthalpy (H) of a rxn occuring in solution during which atmospheric pressure remains constant, easiest way is to use a cofee-cup calorimeter to measure heat-accompanying reactons at constant pressure |
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Term
| What happens in the coffee-cup calorimeter when the heat is produced y the qrxn |
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Definition
| it is entirely absorbed by the solution, & it does not escape the calorimeter |
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Term
| What does Heat gain=Heat loss |
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Definition
The heat gained by the sol'n, qsol'n, is equal to the magnitude to qrxn
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-qsol'n=Cs*m*dT=-qrxn |
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Term
| in Constant pressure Calorimetry for dilute aqueous soln's |
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Definition
| -The specific heat of the sol'n will be close to pure water (4.184J/g-k) |
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