laws
whats the law of conservation of energy
energy can’t be created, only be transferred
what is enthalpy (H), measured in what
measure of the total energy of a thermodynamic system (J)
particles must collide with enough energy and the right orientation
where does inital rate start
at 0. always
assumptions of calorimtetry
no heat was lost
heat released by the calorimeter is disregarded
all aqueous solutions have the same density as water [1.0M]
what happens during energy transfer
some thermal heat is always lost
whats the value of exothermic
negative (graph goes down)
whats activation energy (Ea)
minimum amount of energy needed to start a reaction
a bump in reaction (needs to go higher before the product can be formed)
whats is rate of reaction
speed, change in reactants/products consumed over time
bond energy: reactants - products (exothermic)
heat of formation: products - reactants
whats the first thermodynamic law
change forms but energy isn’t made of destroyed
whats the value of endothermic
positive (graph goes up)
whats a first vs. second order reaction
first order: straight line
second order: curved line
whats average rate of reaction
slope between two points
rate mechanism: what are intermediates
compounds/elements that appear in the elementary steps that don’t appear in the final equation
whats the second thermydynamic law
heat diffusion
whats bond energy
amount of energy it takes to break a bond
what does a catalyst do to Ea
decreases the activation energy needed to start the reaction
whats instantaneous rate of reaction
slope at a certain point (tangent)
whats are a few charactersitics of the rate-determining step (general, graph etc.)
slowest step
overall rate is dependent on this step
highest bump: slowest step/limiting reactant
whats the third thermydynamic law
heat always goes towards absolute zero
whats heat of formation
total energy formed
whats rate mechanism
series of elementary steps that get you to your final product
what are six factors that affect rate
nature (some are faster/slower)
more collisions/concentrations of reactants = faster
more pressure of reactants = faster
more surface area of reactants = faster
higher temp = faster
catalyst = faster
what does Δ mean
change in (temperature, enthalopy etc.)