chem 2 exam 2 pract Flashcards
For similar bimolecular reactions, rate constants typically decrease as the size and complexity of the reactants increase.
True. Larger and more complex molecules tend to have lower rates due to increased steric hindrance and fewer effective collisions
The activation energy for a one-step reaction is the energy required to reach the transition state. t/f
True. Activation energy is indeed the energy barrier that must be overcome to reach the transition state.
Higher collision frequency results in faster rates. t/f
True. More frequent collisions typically increase the likelihood of successful reactions, leading to faster reaction rates
The transition state for a reaction is the lowest energy structure intermediate between reactants and products.
False. The transition state is not the lowest energy structure; it is the highest energy state along the reaction pathway. It represents a point of maximum energy where old bonds are breaking and new bonds are forming.
It is often found that the rates of reaction generally increase with an increase in temperature.
True. Increasing temperature usually increases the kinetic energy of molecules, leading to more frequent and more energetic collisions.
in a reaction mehcnaism the intermidiate is
what is produced in one step then used in the enxt
the step with the highest activation energy (i.e., the slowest step) is the one that
limits how fast the entire reaction can proceed.
k means
rate constant
Δn
final moles-initial moles
increasing volume increase shift to the
right
Q<K eq shift to the
right
Q>K eq shift to the
left
Q=K eq system shifts
doesnt shift its equalibirum
if a system leans to the right it favors
products
if a system leans to the left it favors
reactants
