Kinetics, Equilibrium, Le Chatlier Flashcards
Chemical reaction definition
reactions –> products
products –> reactions
each reaction has specific rates
orientation and speed are important in chemical reactions. T/F?
increasing temperature increases the forward rate of the reaction. T/F?
True
True
spontaneous reaction definition
it happens without further help or input
moving from high energy state to lower energy state.
ATP + water (high energy with neg phosphates)—spontaneous—–> ADP +
Transition states are momentary arrangements. This state is very high energy and unstable (activation energy) which prompts reaction to drop in energy
Difference between total energy and activation energy
Greater the activation energy the slower the reaction proceeds. T/F
True
more work needed for bigger hill
what does a catalyst do?
- lowers activation energy
- cant be consumed or used up
- doesnt effect free energy of reactants or products
- biological or abiological (ions)
What are elementary steps of a reaction?
An elementary step (or elementary reaction) is one step in a series of simple reactions that show the progress of a reaction at the molecular level. A reaction mechanism is the sequence of elementary steps that together comprise an entire chemical reaction
What is the rate limiting step
is the slowest step in the reaction that delays the rate of everything else
What do the exponents in the overall rate law tell you about the order of the reaction?
exponent => second order ==> needs 2 of that molecule in parenthesis
what is equilibrium?
Equilibrium is when the rate of the forward reaction equals the rate of the reverse reaction. All reactant and product concentrations are constant at equilibrium
K (equilibrium constant) = [products] / [reactions]
What happens to K when we move away from equilibrium?
The system always works to reestablish equilibrium - Le Chateliers Principle
