Term
| At what stage of a reaction do the atoms have the highest energy? |
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Definition
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| Why does a higher concentration make a reaction go faster? |
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Definition
| There are more collisions per second only. |
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Term
| In a reaction (at equilibrium) that makes more moles of gas than it consumes, what is the eddect of increasing the pressure? |
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Definition
| The reaction makes more products. |
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Term
| In a chemical reaction with a Keq of 1 * 10^8, the ____. |
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Definition
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Term
| What is the effect of adding more water to the following equilibrium reaction? CO2 + H20 <->H2CO3 |
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Definition
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Term
| What are the units for a reaction rate? |
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Definition
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Term
| Why does a catalyst cause a reaction to proceed faster? |
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Definition
| The activation energy is lowered only. |
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Term
| What happens to a reaction at equilibrium when a product is removed from the reaction system? |
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Definition
| The reaction makes more products. |
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Term
Which of the following does NOT affect the rate of a chemical reaction?
A. the equlibrium position
B. the temperature
C. the concentration of reactants
D. the presence of a catalyst |
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Definition
| A. the equilibrium position |
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Term
| If a reaction it reversiblem what are the relative amounts of reactant and products at the end of the reaction? |
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Definition
| some product;some reactant |
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Term
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Definition
| lowering the activation energy barrier |
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Term
| What happens to a reaction at equilibrium when more reactant is added to the system? |
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Definition
| The reaction makes more products. |
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Term
| The rate of a chemical reaction normally _______ as reaction concentration increases. |
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Definition
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