MCAT Physical : Physical Chemistry
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Example Question #121 : Physical Chemistry
Which of the following are true concerning the rate-limiting step of a chemical reaction?
I. It is the slowest step
II. Cannot be altered by a catalyst or enzyme
III. Involves the transition state with the highest activation energy
IV. Is un-affected by a change in reactant concentration or reaction temperature
III and IV
I, II, and III
I only
I and III
I, II, III, and IV
I and III
The rate-limiting step of any reaction will always have the highest activation energy, and thus be the slowest step in a chemical reaction (hence the name). It can be altered with the help of a catalyst, by changing the concentration of reactions, and by altering the reaction temperature. These changes can affect the energy of a transition state or chemical equilibrium, altering the rate-limiting step. Only choices I and III are true.
Example Question #122 : Physical Chemistry
Consider the following overall reaction:
The rate law for this reaction is determined to be:
What can we conclude about the reaction, based on the rate law?
Carbon monoxide is a solid, so it is not included in the rate law
The slow step involves two nitrogen dioxide molecules
The fast step involves two nitrogen dioxide molecules
The overall reaction must be done twice
The slow step involves two nitrogen dioxide molecules
Since the rate law does not match the overall reaction, we can assume that the reaction has multiple steps.
In a multistep reaction, the slowest step will determine the rate law. As a result, we can conclude that the overall reaction has a slow step, in which two nitrogen dioxide molecules react. The coefficient becomes the exponent. Note that this is only the case because we are working with the identified slow step, which can only be determined experimentally.
Carbon monoxide only enters into the equation in the faster step, and is not included in the overall rate law.
Example Question #123 : Physical Chemistry
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
At which point(s) on the above graph would you expect to find bonds forming and breaking?
3 and 4
2 and 4
2, 3, and 4
3 only
2 and 3
2 and 4
It may be tempting to include points 2, 3, and 4, but only points 2 and 4 actually have bonds in the process of forming and breaking. This lack of stability is what gives these points the highest relative energy levels on the diagram. Point 3 is a relatively stable intermediate, stabilized by the fact that it does not have bonds in active flux.
Example Question #124 : Physical Chemistry
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
In the reaction diagram, which point is most instrumental in determining the rate of the forward reaction?
5
2
3
1
4
2
Point 2 is at the highest peak on the chart. The difference between the energy level at this point and the energy level of the reactants is the activation energy. This is the energy that the reactants must overcome to proceed to the lower energy products. Overcoming this point takes energy, and is the primary limiting factor in the speed of any reaction.
Example Question #41 : Reaction Kinetics
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
After much thought, the scientist in the passage determines that the reaction depicted in the diagram must be either a radical reaction or a combustion reaction. Which of these options is more likely?
A radical reaction, as point 3 would correspond to a radical intermediate
A combustion reaction, as they contain radical intermediates
A radical reaction, as they are always exothermic
A combustion reaction, because they are always endothermic
A combustion reaction, as they contain carbocation intermediates
A radical reaction, as point 3 would correspond to a radical intermediate
A radical reaction would be a more likely candidate in this case, as step 3 on the diagram would correspond to the stable intermediate. In the radical reaction, this would correspond to a radical intermediate.
Combustion reactions typically don't have a stable intermediate, and are typically exothermic (not endothermic as the answer choice indicates).
Example Question #42 : Reaction Kinetics
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
The scientist in the passage is able to determine that the reactants in the diagram are hydrophilic compounds. Which of the following is likely to decrease the energy level of the reactants?
Dissolution in ethane
Increased occupance of d and f orbitals in the reactants' electronic structures
Dissolution in carbon tetrachloride
Increased abundance of pi bonds in the reactants' bonding patterns
Resonance structures for the reactants' chemical structures
Resonance structures for the reactants' chemical structures
Of any of these changes, only the presence of resonance structures will decrease the overall energy level of hydrophilic compounds. The two solution options both reference nonpolar solvents (though carbon tetrachloride has polar bonds, their geometry cancels out any net dipole moment). Additionally, pi bonds are high energy bonds, and d and f orbitals are high energy orbitals.
Resonace allows greater charge distribution and stability, thus reducing energy level.
Example Question #41 : Reaction Kinetics
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
The scientist in the passage is attempting to modify the reaction as it is ongoing, and adds a catalyst to the vessel. Which points will not move with the addition of a catalyst?
4 only
1 only
2 and 4
1 and 5
2 only
1 and 5
Points 1 and 5 are the energy levels of the reactants and products, respectively. These levels do not change with the action of a catalyst, and instead are fixed by the thermodynamic nature of the chemical species involved. A catalyst would lower activation energies by providing an alternate route to reach the products from the reactants, and thus would likely affect points 2, 3, and 4.
Example Question #121 : Physical Chemistry
Carbonic anhydrase is an important enzyme that allows CO2 and H2O to be converted into H2CO3. In addition to allowing CO2 to be dissolved into the blood and transported to the lungs for exhalation, the products of the carbonic anhydrase reaction, H2CO3 and a related compound HCO3-, also serve to control the pH of the blood to prevent acidosis or alkalosis. The carbonic anhydrase reaction and acid-base reaction are presented below.
CO2 + H2O 
H2CO3 
If the reaction series presented above is occurring during alkalosis, H2CO3 may be considered a(n) __________.
intermediate
cannot be determined
enzyme
hormone
intermediate
First, we need to see what the information the question provides us, namely that the reaction is occurring during alkalosis. In alkalosis, we know that the H+ concentration is too low, thus the reaction must be favoring the products in order to reduce the effects of alkalosis (Le Chatlier’s Principle). The H+ is low on the products side, so the reaction shifts to the right. Next, we need to determine where in the reaction H2CO3 is and what is happening to it. We can see that H2CO3 is formed from CO2 and H2O, but then is used up to create HCO3- and H+. In the scenario of alkalosis, H2CO3 will be formed then used (the definition of an intermediate).
Example Question #1141 : Mcat Physical Sciences
For any given chemical reaction, one can draw an energy diagram. Energy diagrams depict the energy levels of the different steps in a reaction, while also indicating the net change in energy and giving clues to relative reaction rate.
Below, a reaction diagram is shown for a reaction that a scientist is studying in a lab. A student began the reaction the evening before, but the scientist is unsure as to the type of the reaction. He cannot find the student’s notes, except for the reaction diagram below.
Upon further review, the scientist realizes that the reaction in question involved formation of a carbocation that quickly reacted again to form stable products. At which point would we most likely find this carbocation in the above diagram?
4
5
3
2
1
3
Point 3 is where you would expect to find a relatively stable intermediate. An intermediate is more stable than a transition state, but not as stable as the original reactants and final products. Stability is inversely proportional to energy, thus we are looking for the point that is between the highest and lowest energies in the reaction. By this logic, point 1 is the reactants, 2 and 4 are transition states, 3 is a stable intermediate, and 5 is the products.
Example Question #1 : Thermodynamics Of Phase Changes
A scientist prepares an experiment to demonstrate the second law of thermodynamics for a chemistry class. In order to conduct the experiment, the scientist brings the class outside in January and gathers a cup of water and a portable stove.
The temperature outside is –10 degrees Celsius. The scientist asks the students to consider the following when answering his questions:
Gibbs Free Energy Formula:
ΔG = ΔH – TΔS
Liquid-Solid Water Phase Change Reaction:
H2O(l) ⇌ H2O(s) + X
The scientist prepares two scenarios.
Scenario 1:
The scientist buries the cup of water outside in the snow, returns to the classroom with his class for one hour, and the class then checks on the cup. They find that the water has frozen in the cup.
Scenario 2:
The scientist then places the frozen cup of water on the stove and starts the gas. The class finds that the water melts quickly.
After the water melts, the scientist asks the students to consider two hypothetical scenarios as a thought experiment.
Scenario 3:
Once the liquid water at the end of scenario 2 melts completely, the scientist turns off the gas and monitors what happens to the water. Despite being in the cold air, the water never freezes.
Scenario 4:
The scientist takes the frozen water from the end of scenario 1, puts it on the active stove, and the water remains frozen.
Which of the following are possible quantities for the “X” present on the right side of the Liquid-Solid Water Phase Change Reaction?
I. Entropy
II. Heat
III. Water Vapor
I and II
I, II, and III
I and III only
II only
I only
II only
As water freezes, it releases heat into the universe to balance the local loss of entropy encountered by ordering atoms into a rigid solid structure. Entropy, in contrast, is not a commodity that can be released by a reaction in the same way as heat. Also, water vapor would not be released on only one side of the equation. Water vapor would exist with in equilibrium with both solid and liquid, but would not appear as an additional product with the solid phase in this reaction.
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