Question | Answer |
True or False: Reactions take place at different speeds | True |
Define Rate of Reaction | change of concentration of reactant per unit time |
What is initial rate? | constant rate verses time |
What happens to the rate of reaction as the reactant begins to be used up? | it decreases |
How do molecules react to each other? | by colliding with each other |
Why do most collisions do not result in a reaction? | because millions of collisions happen per second, thus effecting the rate of reaction. We look at the collisions that make the product |
What are some collisions effective and others are not? | two reasons: 1.) activation energy- the energy needed for molecules to make a new product 2.) the angle the molecule forms toward another molecule (look at orgchem and how lewis dot structures are angle. There is a reason why they are angled like that |
products can not form unless they go | "over the hill" read text for explanation |
activation energy is __________ _________ to the rate of reaction. | inversely related |
the speed of reaction is ________ to the __________. | proportional, to the probability of effect of collision |
What are the four things that the rate of reactions affect when dealing with activation energy level? | 1.) nature of reaction 2.) concentration 3.) temperature 4.) presence of a catylist |
concentration of a reaction is __________ to the rate of reaction | directly proportional |
reaction rate increases with ______ | increasing temperature |
temperature vs effects of reaction | temperature increases the collision of molecular forces, thus the # of collisions raises out of total collisions. |