which is true of the relation of the forward Kf and reverse Kr reaction rates? a
ID: 852239 • Letter: W
Question
which is true of the relation of the forward Kf and reverse Kr reaction rates?
a) kf always = kf
b) kf = 1/kf
c) kf/kf = equilibrium constant k
d) the ratio kf/kr is a funciton of the equilbirum constant
e) kf is always > kr
2) consider the two first order parallel reactions A-->B and A-->. if the activation energy of A--> B is greater than that of A-> C what should be done to mazimze theselectivity of B with respect to C?
a) run the reaction at high pressures
b) run the reactions at high temp
c) run the reactions at low volumes
d) run a pipe filtering C out of the reactor as made
e) recycle unused A
3) why can concentration not always be used in a mass balance?
a) concentration is not explicit in the ideal gas equation
b) the volume of the mix can change with reaction
c) concentration is a short-hand variable, not a property
d) concentration could be changed with scale up
e) concentration is independent of mass
4) in which reactors is dV part of the rate equation?
PFR
Batch
CSTR
None
All
Why?
a) because this / these reactor(s) is/are run at steady state
b) beacuse this/these reactor(s) must obey the continuity of energy
c) because this/these reactor(s) must obey the continuity of mass
d) because this/these reactor(s) change with respect to time
e) because this/these reactor(s) change with respect to volume
5) what happens at extended times in equilibrium reactions?
a) the thermodynamic values are achieved
b) the kinetic values become unsolvable
c) all reactants get used up
d) the temperature factor becomes negligible
e) no products are produced
Explanation / Answer
1. Ratio kf/Kr is a function of equilibrium constant
2. Run the reactions at high temperatur
3. The volume of mixture can change with reaction
4. PFR, because change with respect to volume
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