Raising the temperature speeds up the rate of a chemical reaction by increasing?

Question

A. the effectiveness of the collisions, only
B. the frequency of the collisions, only
C. both the effectiveness and the frequency of the collisions
D. neither the effectiveness nor the frequency of the collisions

Answer 1

C

Think about it. If I lit a fire under your butt, you would move faster and with more energy. If you are blindfolded and I am chasing you around the room with a bunsen burner, you are going to run into the walls of the room more often and with a lot more energy! So that means, more collisions and collisions that occur more frequently. As opposed to if I just left you in a room (blindfolded) and asked you just to walk around. You would bump into the wall, not all that often and you would be moving very slowly since you can't see!

By increasing the number of collisions and the effectiveness of the collisions you increase the liklihood that the species have enough energy to get over the energy barrier for that reaction. The energy barrier is called the activation energy. When the activation energy is exceeded then the reaction happens. Increasing temp causes more reactants per unit time to have the ability to/be more likely to have the energy needed for hte reaction to occur.

Answer 2

c)it will strengthen the style of debris that have sufficient kinetic capability to react while they collide additionally, elevating the temperature could strengthen the style of collisions at any given 2nd, yet temperature strengthen isn't a catalyst. A catalyst is many times yet another factor extra to velocity the reaction.

Answer 3

adding heat to a reaction, speeds things up because the molecules are colliding more often, which speeds the reaction. now, i am almost certain that it also adds to the effectiveness because they are all hitting at different angles, which a lot of reactions can only happen when certain angles are formed...so, i am fairly sure that the answer is C

Answer 4

B. Also by raising the available Gibbs free energy (or 'activation energy').

Doug

Answer 5

I would agree with C