Factors that affect reaction rate
Conditions at equilibrium
Shifts in equilibrium
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| 817904529 | True or False: Reaction rate is proportional to the number of effective collisions. | True! Reactions happen due to collisions | |
| 817904530 | List 4 ways to increase collisions and thus increase reaction rate. | 1) Increase temperature (for solids) - this increases energy= increases movement = increases collisions 2) Increase surface area by crushing the reactants into smaller pieces - This increases the # of particles having collisions 3) Add a catalyst - this lowers the activation energy so reactants don't have to gain as much energy to react 4) Increase the concentration of the reactants = increases the # of particles colliding | |
| 817904531 | In a potential energy diagram for a reaction, the presence of a catalyst will be shown with what? | It will be shown with a dashed line that is below the original activation energy curve. | |
| 817904532 | What does chemical equilibrium mean? | Equal rates of forward (reactants to products) and reverse (products to reactants) reactions. Does NOT mean equal amounts of the reactant and product just equal rates of transfer! | |
| 817904533 | In an equilibrium expression, the _____ go on top in brackets. | Products | |
| 817904534 | A K (equilibrium constant) greater than 1 tells you that the reaction: | proceeds mostly to completeion (to products) | |
| 817904535 | When a reaction is at equilibrium and the pressure is increased, how will it react? | It will shift to the side with less mess - side with less stuff on it! | |
| 817904536 | A reaction is at equilibrium. One of the reactants is increased. What happens? | Shift to the product side to use up extra reactant. | |
| 817904537 | A reaction is at equilibrium. One of the reactants is constantly removed from the reaction. What happens? | Shift to the reactant side to replace the removed reactant. |
