module 5 - physical chemistry and transition elements Flashcards
what is short hand for concentration of reactant ‘A’
[A]
what is the correlation between rate and concentration
directly proportional
define zero order
when the concentration has no effect on rate of reaction
in a zero order reaction:
- concentration of a reactant is to the power of 0
- any number raised to the power of 0 =1
- doesn’t appear in the rate equation
- concentration does not influence the rate of reaction
in a first order reaction:
if the concentration of A is doubled (x2) the reaction rate is increased by a factor of 2^1
(directly proportional)
in a second order reaction:
if the concentration is of A is doubled, the reaction rate increases by a factor of 2^2 = x4
what is the rate equation
rate = K [A]^m [B]^n
k = rate constant
[ ] = concentration
m&n are orders
what is the trend in concentration-time graphs for:
zero order
first order
second order
zero: straight line with negative gradient
first order: downward curve with a decreasing gradient over time - half life is constant
second order: also a downward curve but steeper at the start and tails off more slowly
define exponential decay
first order reactions have a constant half life (time taken for half a reactant to be used up)
what are the trends in rate-concentration graphs for:
zero order
first order
second order
zero: straight horizontal line with zero gradient
first: straight line directly proportional
second: upward curve with increasing gradient
how can you find the rate constant (k) from rate-concentration graphs for:
zero order
first order
second order
zero - y intercept
first: gradient
second: cannot be determined
how do you work out the initial rate of reaction from a concentration-time graph
draw a tangent at T=0 and calculate the gradient
what does the rate equation only include?
reacting species involved in the rate-determining step.
what is the Arrhenius equation? And what do the letters stand for?
k = A e^(-Ea/RT)
k = rate constant
A = frequency factor
Ea = activation energy
R = gas constant (8.314)
T = temperature (Kelvin)
what is the logarithmic form of the Arrhenius equation
Ln k = - Ea/R (1/T) + Ln A