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Module N
Reaction Rates, Equilibrium
| Question | Answer |
|---|---|
| Speed's definition | is considered a rate |
| Reaction rate's definition | the change of the amount of reactant or product over time (how fast are products made) |
| Collision theory's definition | atoms, ions, and molecules can react to form products when they collide if the particles have enough kinetic energy and the correct orientation at the time of collision |
| Activation energy's definition | the minimum energy needed to be absorbed for the reaction to occur |
| What are the 2 things required for products to be made? | Activation energy must be met (this means they have enough) Proper collision of the particles |
| Does an exothermic reaction ever gain energy? | Yes, it must gain its activation energy. Overall it will still lose energy. |
| Where on an endo or exo graph are products starting to be made? | At the top of the activation energy "bump" is where reactants begin to transform into products provided there is a proper collision |
| Why does refrigerating your leftovers help them to stay safe to eat? | Lowering the temperature slows the reaction rates of mold and bacteria formation |
| Why would it not be recommended to drink milk left in a hot car? | The increase in temperature increased the rate of reaction of the milk spoiling. |
| What reacts faster, a 10g block or 10g of powder | 10g of powder |
| Which would decrease the reaction rate? 1) increasing the temperature 2) breaking up the item into smaller pieces 3) lowering the concentration | 3) lowering the concentration |
| True or False A catalyst is used up. | False |
| True or False A catalyst is considered a reactant | False |
| True or False A catalyst lowers the needed activation energy | True |
| True or False A catalyst speeds up a reaction | True |
| True or False At equilibrium, the concentration (aka amount) of reactants equals the concentration of the products | False, the concentrations will no longer change but they do not need to be equal (lots of students get this wrong and think this is true) |
| True or False At equilibrium, the speed of the forward and reverse reactions are the same | True, this is what is "equal" in equilibrium |
| Using N2 + H2 <--> NH3 which is a reversible reaction at equilibrium... How does the reaction shift when more N2 is added? | The reaction shifts right to regain equilibrium |
| Using N2 + H2 <--> NH3 which is a reversible reaction at equilibrium... How does the reaction shift when more NH3 is added? | The reaction shifts left to regain equilibrium |
| Using N2 + H2 <--> NH3 which is a reversible reaction at equilibrium... How does the reaction shift when some H2 is removed? | The reaction shifts left to regain equilibrium |
| Using SO3 <--> SO2 + O2 which is a reversible reaction at equilibrium... Which of the following would produce more products by speeding up the forward reaction 1) Adding more O2 2) Removing some SO3 3) Removing some SO2 | 3) Removing some SO2 will shift the reaction to the right speeding up the forward reaction and make more products |
| Using SO3 <--> SO2 + O2 which is a reversible reaction at equilibrium... Which of the following would produce more reactants by speeding up the reverse reaction 1) Removing some O2 2) Removing some SO3 | 2) Removing some SO3 |
Created by:
erika.johnson
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