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MCAT Warm-up
MCAT I

1 .       Passage I (Questions 1-8)

What is the approximate ratio of the longest to the shortest wavelength shown? 



2 .       Passage I (Questions 1-8)

The wavelengths shown are given in nanometers (nm), where 1nm = 10-9m. Which of the following represents the shortest-wavelength spectral line shown in meters? 



3 .       Passage I (Questions 1-8)

In Scientist 1's view, the shortest wavelength transition represents the: 



4 .       Passage I (Questions 1-8)

Which relation would Scientist 1 use to convert wavelength to energy most directly



5 .       Passage I (Questions 1-8)

For Scientist 1, a transition in hydrogen having = 610 nm would be: 



6 .       Passage I (Questions 1-8)

Scientist 2 views the transition at 434 nm as: 



7 .       Passage I (Questions 1-8)

Scientist 2's views would be reinforced by which of the following?

I. The finding that other atoms gave similar emission spectra in the same spectrometer.

II. The finding that other atoms gave different emission spectra in the same spectrometer.

III. Evidence that the spectrometer contained hydrogen atoms. 



8 .       Passage I (Questions 1-8)

Another researcher analyzes the light from a tungsten filament lamp using the same spectrometer, and finds that a broad spectrum of wavelengths are present in the region from 400 to 650 nm, with no sharp lines. These findings support: 



9 .       Passage II (Questions 9-12)

If a small quantity of sulfide ion is introduced into the mixture of Zn2+ and Pb2+, what will precipitate first? 



10 .       Passage II (Questions 9-12)

Which of the following expressions should the chemist use to calculate the concentration of sulfide at which PbS will precipitate? 



11 .       Passage II (Questions 9-12)

The chemist wonders how difficult it will be to prepare the dilute solutions of sulfide indicated in Table 2. How many S2- ions per cubic centimeter are represented in the solution indicated in the first row of the table? 



12 .       Passage II (Questions 9-12)

What is the value of [S2-] when pH is 2.0? 



13 .       Passage III (Questions 13-18)

From Experiment 1, the student concludes that the solubility of the salt is: 



14 .       Passage III (Questions 13-18)

Based on LeChatelier's Principle, how will the solubility of the compound in 0.1 M NaOH compare to the solubility of the compound in water? 



15 .       Passage III (Questions 13-18)

Which of the following expressions would allow the student to solve for the approximate concentration of Mg2+ in the alkaline solution? 



16 .       Passage III (Questions 13-18)

The student decides to measure the solubility of the salt in strong acid solution, as in Experiment 3. How would the solubility in acid compare to the solubility in the basic solution? 



17 .       Passage III (Questions 13-18)

Which of the following expressions could be used to calculate the solubility of the solution prepared in Experiment 3? 



18 .       Passage III (Questions 13-18)

Which of the following can the student conclude?

I. Ksp is pH-dependent.

II. The solubility of Mg(OH)2 is pH-dependent.

III. The pH-dependence of this solubility serves as a model for all other magnesium salts. 



19 .       Passage IV (Questions 19-23)

Once the substance in the flask is vaporized, how do changes in temperature affect the number of moles of gas in the flask (assuming the flask to be open and the pressure and volume to be constant)? 



20 .       Passage IV (Questions 19-23)

Which of the following did the student use to calculate the number of moles of gas in the flask at 100° C? 



21 .       Passage IV (Questions 19-23)

Which of the following did the student use to calculate the molecular weight of the gas in the flask? 



22 .       Passage IV (Questions 19-23)

Which of the following errors might explain the difference between the molecular weight calculated by the student and the figure given by the instructor? 



23 .       Passage IV (Questions 19-23)

The student decides to investigate whether the discrepancy in molecular weight measurements is due to molecules that bind together to form aggregates in the gas phase. If such aggregated molecules occurred in the gas sample, which of the following would be affected?

I. The number of molecules

II. The total weight of the gas

III. The average speed of the molecules 



24 .       Passage V (Questions 24-28)

Theory 1 relates the: 



25 .       Passage V (Questions 24-28)

According to Theory 1, which of the following expresses the rate of this reaction?

3M + 2N --> 4P
 



26 .       Passage V (Questions 24-28)

According to a proponent of Theory 2: 



27 .       Passage V (Questions 24-28)

A chemist studies the rate of the reaction

2NO2 + F2 --> 2NO2F

According to Theory 1, the rate of this reaction is proportional to: 



28 .       Passage V (Questions 24-28)

The chemist suspects that the reaction given in the previous question proceeds in two stages:

NO2 + F2 --> NO2F + F (Stage 1)

F + NO2 --> NO2F (Stage 2)

According to Theory 2, if Stage 1 is much slower than Stage 2, then the overall reaction rate: 



29 .       Passage VI (Questions 29-35)

The pair of salts with the least and greatest solubility in pure water, respectively, are: 



30 .       Passage VI (Questions 29-35)

The solubility of Pb(OH)2 in the presence of 0.1 M cation is: 



31 .       Passage VI (Questions 29-35)

The solubility of a given salt in pure water is: 



32 .       Passage VI (Questions 29-35)

The solubility of a given salt in the 0.1 M cation solution can be calculated as which of the following? 



33 .       Passage VI (Questions 29-35)

Which of the lead salts listed produces the greatest concentration of Pb2+ when added in excess to pure water? 



34 .       Passage VI (Questions 29-35)

Excess BaF2 is added to pure water; then Ba(NO3)2 is added until the solution is 0.1 M in Ba2+. Which of the following is true? 



35 .       Passage VI (Questions 29-35)

Solution A is 0.1 M in both Ba(NO3)2 and Ca(NO3)2. To 100 mL of solution A, a student adds 1.0 mL of 0.1 M Na2SO4. What will be the result? 



36 .       If 22.5 g of NiCl2 reacts completely with a sufficient amount of NH3 and NaBr to form Ni(NH3)2Br2Cl2, which of the following expressions gives the number of moles of product that are formed? (at. wt. of Ni = 58.7, of Cl = 35.5, of Br = 79.9) 



37 .       Which is the correct electron-dot formula for H2O2



38 .       Which of the following is closest to the pH of a mixture containing 1.0 mole each of formic acid (whose Ka is 1.8 x 10-4) and potassium formate? 



39 .       If 1.0 mole each of graphite at 350K (Cp = 8.63 J/mol deg) and water at 273K (Cp = 4.18 J/mol deg) are put together in an insulated container, which of the following gives the final temperature (T) of the water in degrees C? 



40 .       A "3-minute egg" cooked in Boston might require extra cooking time in: 



41 .       An electron in a hydrogen atom is excited to a state where l = 2 and n = 4. This state is referred to as: 



42 .       The solubility of AgCl in water can be increased by: 



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