Term
| What is the law of conversion of energy? |
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Definition
| Energy can neither be created or destroyed, only converted from one form to another. |
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Term
| What is the equation for kinetic energy? What values have a large effect on kinetic energy? |
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Definition
KE = .5mv^2
From this we can see that KE is dependent upon mass and velocity |
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Term
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Definition
| A force acting over a distance. Or motion against an opposing force. |
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Term
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Definition
| A transfer of energy measured by differences in temperatures. |
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Term
| What are the two ways to transfer energy? |
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Definition
| work and heat are the two ways to transfer this. |
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Term
| What is a state function? |
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Definition
| A property of the system that depends only on its present state, it is independent of the pathway. They're always written in capital letters. Ex- pressure=P, energy=E |
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Term
| What is an exothermic reaction? |
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Definition
| A reaction in which energy flows out of the system. It feels hot. |
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Term
| What is an endothermic reaction? |
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Definition
| A reaction in which energy flows into the system. |
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Term
| What do we know about the law of the conversion of energy and exothermic reactions? |
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Definition
| The energy lost by the system is equal to the energy gained by the surroundings. |
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Term
| What is true of potential energy in exothermic reactions? |
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Definition
| The potential energy stored in the chemical bonds is being converted into thermal (random kinetic energy) energy via heat. |
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Term
| Why do exothermic reactions release heat? |
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Definition
| These types of reactions release this energy form because they are losing potential energy. |
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Term
| What is the first law of thermodynamics? |
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Definition
1.The energy of the universe is a constant.
2. The internal energy in of a isolated system is constant.
3. Energy is neither created or destroyed in chemical reactions and physical changes. |
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Term
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Definition
The sum of the kinetic and potential energies of all the 'articles' in the system.
Delta E = q+w |
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Term
| What can internal energy be changed by? |
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Definition
| Delta E can be changed by heat and/or work. |
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Term
| What does the sign reflect in a thermodynamic equation? |
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Definition
| The sign in this type of equation reflects the systems's point of view. |
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Term
| What does a positive sign indicate? |
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Definition
| This type of sign indicates the system's energy is increasing. |
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Term
| What does a negative sign indicate? |
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Definition
| This type of sign indicates the system's energy is decreasing. |
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Term
| What does it mean if work is positive or negative? |
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Definition
| If w is positive, the surroundings are doing work on the system. If w is negative, the system is doing work on the surroundings. |
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Term
| What is the formula for pressure? |
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Definition
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Term
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Definition
| A system where energy and matter are exchanged. For example, the human body. |
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Term
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Definition
| A system where only energy is exchanged. For example, a sealed ice pack. |
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Term
| what is an isolated system? |
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Definition
| A system where there is no exchange of energy or matter. For example, a thermos with a sealed lid. |
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Term
| What's the difference between work and heat? |
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Definition
| heat is random motion of particles while work is organized motion of particles |
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Term
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Definition
| This state function is related to the average energy of particles in a system. |
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Term
| What is a vital aspect about the relation of temperature and energy in two different systems? |
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Definition
| Two systems may be at the same temperature but posses different energies due to their size. |
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Term
| What is a non state function? |
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Definition
| A function that is dependent on how the system got to it's current state. Will be written in lower case letters: work=w, heat=q |
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Term
| What can be said about the absolute value of internal energy? |
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Definition
| We can never know the absolute value of this state function. We can only find the change in E |
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Term
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Definition
| A situation where external pressure=zero so the system does no work and therefore loses no energy. |
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Term
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Definition
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Term
| What is the relationship between change in enthalpy and heat at a constant pressure? |
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Definition
| Under this condition, the change in enthalpy of the system is equal to the energy flow as heat. |
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Term
| How do we find enthalpy change in a chemical reaction? |
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Definition
| Heat of reaction is found by subtracting the enthalpy of the reactants from the enthalpy of the products. |
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Term
| At a constant pressure, what is change in enthalpy equivalent to? |
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Definition
| Under this constant state function, Delta H is equivalent to heat. |
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Term
| What is the only way to change an ideal gas's kinetic energy? |
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Definition
| Heat is the only way to change this type of gas's kinetic energy |
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Term
| What is molar heat capacity? |
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Definition
| The energy required to raise the temperature of 1 mole of that substance by 1 K. |
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Term
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Definition
| The transfer of heat energy into or out of a system undergoing a chemical or physical change at constant pressure. |
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Term
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Definition
| Adding heat energy to a sample will cause it to increase in temperature assuming there is no chemical reaction, phase change, and no significant work done. |
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