The Arrhenius equation is shown below. Determine what happens to the rate of the reaction (k) as various parameters are changed.
k=Ae^(-Ea/RT)
Temperature increases
Ea decreases
A increases
k increases
k increases
k increases
Which of the following is true about activation energies?
Exothermic reactions have negative activation energies
Fast reactions have large rate constants and large activation energies
Endothermic reactions always have large activation energies
The forward reaction sometimes has a lower activation energy than the reverse reaction
Which of the energies marked in the diagram represents the activation energy?
Which of the following is true about the reaction represented by the diagram above?
The reverse reaction is slower than the forward reaction
The rate of the reaction is the same forward and reverse directions
The forward reaction is slower than the reverse reaction
It is not possible to tell from the figure which way the reaction will be faster
A
The reverse reaction is slower than the forward reaction
For the following elementary reactions, give the molecularity and the rate law.
CH3NC(g) → CH3CN(g)
O3(g) +NO(g) → O2(g) + NO2(g)
O3(g) → O2(g) + O(g)
O3(g) + O(g) → 2O2(g)
unimolecular
Rate = k[CH3NC]
bimolecular
Rate = k[O3][NO]
unimolecular
Rate = k[O3]
bimolecular
Rate = k[O3][O]
Indicate whether each example is a homogenous or a heterogeneous catalyst.
2CO(g) + O2(g) → 2CO2(g) in a catalytic converter
NO2 catalyzes the breakdown of O3 in the upper atmosphere.
ammonia is synthesized from N2 and H2 using iron.
an acid (water) is used to catalyze the hydrolysis of an ester
CH3CO2CH3(aq) + H2O(ℓ) ⇌ CH3CO2H(aq) + CH3OH(aq)
heterogeneous catalysts
homogeneous catalyst
heterogeneous catalysts
homogeneous catalyst
What is the rate law for the following elementary step?
2 N O 2 → N O 3 ( g ) + N O ( g )
What is the molecularity of the reaction above?
Rate= k[NO2]^2
Bimolecular
In order to be considered consistent with a given reaction, a proposed mechanism must ______.
have elementary reactions that sum to the overall balanced equation for the reaction
have as many steps as there are reactants
have a bimolecular reaction as the rate limiting step
predict the experimental rate law
have at least one unimolecular step
A proposed mechanism for the reaction between nitrogen dioxide and fluorine is as follows:
NO 2 ( g ) + F 2 ( g ) → N O 2 F ( g ) + F ( g )
F( g ) + N O 2 ( g ) → N O 2 F ( g )
The rate law was experimentally determined to be k[NO2][F2]
-What is/are the rate determining step(s)?
The following reaction is at equilibrium in a flask.
2O3(g) ⇌ 3O2(g)
Which way does the equilibrium shift (to the left or to the right) if more O2 is added to the flask?
Which way does the equilibrium shift if more O3 is added to the flask?
If the volume of the flask is reduced, which way does the equilibrium shift?
Consider the reaction below and answer the following questions.
2H2(g) + O2(g) ⇌ 2H2O ∆Hrxn = -283 kJ/mol \n
Which way does the equilibrium shift if you increase the temperature?
The reaction is contained in a closed flask. Which way does the equilibrium change if the volume is decreased?
Which way does the equilibrium shift if the pressure is increased by the addition of argon?
In both questions #2 and #3 the pressure increases. What is the difference between the two situations?
To the left
To the right
No shift
In #2, decreasing the volume results in an increase in the partial pressures of all the gasses so the equilibrium is affected. In #3, the partial pressures of the reactants and products do not change so the equilibrium doesn't change.
For which of the following reactions is Kp = Kc?
2N H 3 ( g ) + 2 O 2 ( g ) ⇌ N 2 O ( g ) + 3 H 2 O ( g )
C a C O 3 ( s ) ⇌ C a O ( s ) + C O 2 ( g)
2N 2 H 4 ( ℓ ) + 2 N O 2 ( g ) ⇌ 3 N 2 ( g ) + 4 H 2 O ( ℓ )
4H C l ( a q ) + M n O 2 ( s ) ⇌ M n C l 2 ( a q ) + 2 H 2 O ( ℓ ) + C l 2 ( g )
PC l 3 ( g ) + C l 2 ( g ) ⇌ P C l 5 ( g )
Which direction does the reaction shift if you increase the partial pressure of the Cl2(g)?
Which direction does the reaction shift if you increase the temperature?
Which direction does the reaction shift if you increase the pressure by adding helium to the flask?
Towards the products
Towards the reaction
No shift