Term
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Definition
| a reaction once started that proceeds on its own without external influence |
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Term
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Definition
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Term
| what two factors determine if a process will be spontaneous or not |
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Definition
| energy change or entropy change |
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Term
| if a process gives off energy it is considered |
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Definition
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Term
| if a process involves an increase in entropy, it is considered |
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Definition
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Term
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Definition
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Term
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Definition
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Term
| exotheremic and endothermic refer specificall to |
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Definition
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Term
| units used for energy changes |
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Definition
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Term
| energy cannot be (blank) but can be (blank) |
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Definition
| created or destroyed, converted into another form of energy |
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Term
| what two types of energy are often interconverted in chemical reactions |
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Definition
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Term
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Definition
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Term
| what is more probable, an ordered or disordered state |
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Definition
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Term
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Definition
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Term
| do all spontaneous reactions occur at the same rate |
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Definition
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Term
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Definition
| change in concentration/change in time |
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Term
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Definition
| the steps the molecules go through on the way from reactants to products |
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Term
| what two things must be true of molecules for a chemical reaction to take place |
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Definition
| molecules must collide and have proper orientation |
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Term
| collisions must have enough energy to |
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Definition
| break the bonds that already exist |
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Term
| what will happen if the collisions don't have enough energy to break the bonds? |
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Definition
| they will bounce off one another |
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Term
| what four things does heat increase in a chemical reaction |
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Definition
| energy, speed of molecules, number of collisions and force of collisions |
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Term
| does it take enery to break bonds |
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Definition
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Term
| is energy given off when bonds form? |
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Definition
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Term
| there is always an energy barrier to a reaction proceeding as written. What is this called |
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Definition
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Term
| The larger the activation energy the (blank) the rate. |
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Definition
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Term
| The smaller the activation energy, the (blank) the rate |
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Definition
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Term
| Is there any relationship between the activation energy and the energy change for the overall reaction |
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Definition
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Term
| How are two ways an increase in temperature increase the rate of reaction? |
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Definition
| number of collisions, force of collisions |
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Term
| how does an increase in concentration of reactants increase the rate of reaction |
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Definition
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Term
| how would you increase the rate of reaction when using a solid |
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Definition
| increase the surface area |
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Term
| how does a catalyst increase the rate of a reaction? |
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Definition
| It provides a new reaction pathway, which has a lower activation energy |
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