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8.E: Exercises

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    Multiple-Choice Questions

    1. Which of the following is not a postulate of the kinetic molecular theory of gases? 

      1. The average kinetic energy of the gas molecules is proportional to the absolute temperature.  

      2. Gas particles attract and repel one another. 

      3. The size of the gas particles is negligible compared to the distances between them.  

      4. Pressure arises due to the collisions between gas particles and the walls of the container.  

    2. What is the SI unit for pressure? 

      1. Atmosphere 

      2. Pounds per square inch 

      3. Bar 

      4. Pascal 

    3. Boyle’s law relates which two variables? 

      1. Volume and pressure 

      2. Volume and temperature  

      3. Pressure and temperature 

      4. Moles and temperature  

    4. If a 2.0 L sample of a gas at 25 °C has a pressure of 2.4 atm, what is the pressure of this gas if its volume is decreased to 0.50 L at 25 °C?  

      1. 0.60 atm 

      2. 2.4 atm  

      3. 7.2 atm  

      4. 9.6 atm  

    5. Which of the following is the weakest intermolecular force?  

      1. Dipole-dipole attractions  

      2. Ion-dipole interactions  

      3. Dispersion forces  

      4. Hydrogen bonding  

    6. You dissolve a solid in a glass of water and feel the glass heat up. What do you know about the dissolution process?  

      1. The process is exothermic.  

      2. The process is endothermic.  

      3. The water molecules slow down on average.  

      4. Weaker bonds were formed compared to the bonds that were broken.  

    7. Which of the following compounds is a strong electrolyte?  

      1. Sucrose  

      2. Ethanol  

      3. Hydrochloric acid  

      4. Ammonia  

    8. Molarity is defined as moles of solute divided by what?  

      1. Mass of solution  

      2. Mass of solvent  

      3. Liters of solvent  

      4. Liters of solution  

    9. A 0.200 L solution contains 0.0200 moles of sodium chloride. What is the molarity of sodium chloride in this solution?  

      1. 0.00400 M  

      2. 0.100 M  

      3. 0.220 M  

      4. 10.0 M  

    10. If a hypotonic solution is injected into the bloodstream, which of the following will occur?  

      1. Red blood cells will shrivel  

      2. Hemolysis  

      3. Both a and b  

      4. Neither a nor b  

    Warm-up problems

    1. Car tires typically have a pressure range of 32–35 psi. If a tire has a pressure of 34 psi on a day when the temperature is 18.3 °C, what is the tire pressure (assuming no change in volume) if the temperature drops to 1.67 °C? Be sure to use the appropriate unit for temperature when solving this problem.
    2. If a balloon has an initial pressure of 1.07 atm and a volume of 14.0 L, what is its pressure if the volume is decreased to 12.0 L, assuming a constant temperature and amount of gas?
    3. Identify the intermolecular forces present in the following solids:
      1. CH3CH2OH
      2. CH3CH2CH3
      3. CH3CH2Cl
    4. Identify the intermolecular forces present in the following solids:
      1. HCl
      2. H2O
      3. CO2
    5. Arrange each of the following sets of compounds in order of increasing boiling point:
      1. HCl, H2O, SiH4
      2. F2, Cl2, Br2
    6. Arrange each of the following sets of compounds in order of increasing boiling point:
      1. CH4, C2H6, C3H8
      2. O2, NO, N2
    7. What is the expected electrical conductivity of the following solutions?
      1. NaOH(aq)
      2. HCl(aq)
    8. What is the expected electrical conductivity of the following solutions?
      1. C6H12O6(aq) (glucose)
      2. NH3(aq)
    9. Indicate the most important type of intermolecular attraction responsible for solvation in each of the following solutions:
      1. Methanol (CH3OH) dissolved in ethanol (C2H5OH)
      2. Methane (CH4) dissolved in benzene (C6H6)
    10. Indicate the most important type of intermolecular attraction responsible for solvation in each of the following solutions:
      1. The polar halocarbon CF2Cl2 dissolved in the polar halocarbon CF2ClCFCl2
      2. O2(l) in N2(l)
    11. Determine the molarity for each of the following solutions:
      1. 10.5 kg of Na2SO4·10H2O in 18.60 L of solution
      2. 7.0 × 10−3 mol of I2 in 100.0 mL of solution
      3. 1.8 × 104 mg of HCl in 0.075 L of solution
    12. Determine the molarity for each of the following solutions:
      1. 1.457 mol KCl in 1.500 L of solution
      2. 0.515 g of H2SO4 in 1.00 L of solution
      3. 20.54 g of aluminum nitrate in 1575 mL of solution
    13. Determine the molarity for each of the following solutions:
      1. 2.76 kg of CuSO4·5H2O in 1.45 L of solution
      2. 0.005653 mol of Br2 in 10.00 mL of solution
      3. 0.000889 g of glycine (C2H5NO2) in 1.05 mL of solution
    14. What is the mass of solute in 0.500 L of 0.30 M glucose (C6H12O6) used for intravenous injection?
    15. What is the mass of solute in 200.0 mL of a 1.556 M solution of KBr?
    16. An experiment in a general chemistry laboratory calls for a 2.00 M solution of HCl. How many mL of 11.9 M HCl would be required to make 250. mL of 2.00 M HCl?
    17. What is the final concentration of the solution produced when 225.5 mL of a 0.09988 M solution of Na2CO3 is allowed to evaporate until the solution volume is reduced to 45.00 mL?
    18. Define a hypotonic solution.
    19. Define a hypertonic solution.

    Medium

    1. If a balloon with a volume of 13.8 L at a temperature of 23.0 °C and a pressure of 1.0 atm is allowed to rise to a location in the atmosphere where the pressure is 0.75 atm and the temperature is 18.5 °C, what is the balloon's new volume?
    2. A gas sample has an initial volume of 20.0 mL at 25.0 °C and 0.985 atm. If the pressure is increased to 1.98 atm and the volume is decreased to 10.2 mL, what is the gas sample's final temperature (in kelvin units)? Assume the amount of gas remains constant.
    3. What mass of NaCl is required to make 500.0 mL of a 0.250 M solution of NaCl?
    4. Calculate the volume of a 0.530 M solution of HCl needed to make 250.0 mL of a 0.125 M solution of HCl.
    5. Why do the boiling points of the noble gases increase in the order He < Ne < Ar < Kr < Xe?
    6. Neon and HF have approximately the same molecular masses. Explain why the boiling points of neon and HF differ.
    7. The melting point of H2O is 0 °C. Would you expect the melting point of H2S to be −85 °C, 0 °C, or 185 °C? Explain your answer.
    8. When KNO3 is dissolved in water, the resulting solution is significantly colder than the water was originally.
      1. Is the dissolution of KNO3 an endothermic or exothermic process?
      2. What conclusions can you draw about the intermolecular attractions involved in the process?
    9. What does it mean when we say that a 200 mL sample and a 400 mL sample of a salt solution have the same molarity? In what ways are the two samples identical? In what ways are the two samples different?
    10. Explain reverse osmosis and how this can be used to purify water.
    11. If red blood cells added to a solution are observed to shrivel up, does the solution have a higher or lower salt concentration than the red blood cells? Explain your answer.

    Challenge

    1. An oxygen tank for a patient has a volume of 10.0 L and contains oxygen at a pressure of 2015 psi. Assuming no change in the oxygen temperature, determine how long (in minutes) this tank of oxygen will last if the oxygen is delivered at a pressure of 14.7 psi (atmospheric pressure) and a flow rate of 12.0 L/min. (Hint: first calculate the volume of oxygen at 14.7 psi).
    2. A common intravenous solution is 0.9% saline, which contains 0.900 g of NaCl in 100.0 mL of solution. This solution is commonly used as it is isotonic with blood. Patients suffering from hyponatremia (where the sodium concentration in the blood is less than normal) are sometimes treated with 3% saline (3.00 g NaCl in 100.0 mL of solution). Serum levels are typically reported in units of mEq/L or milliequivalents per liter. As NaCl produces one sodium ion per formula unit of NaCl, mEq/L for sodium is equivalent to mmol/L. Determine the molarity and mEq/L sodium ion concentrations for 0.9% and 3% saline.

    Health-Related Questions

    1. Calculate the molarity for each of the following solutions:
      1. 0.195 g of cholesterol (C27H46O) in 0.100 L of serum, the average concentration of cholesterol in human serum
      2. 4.25 g of NH3 in 0.500 L of solution, the concentration of NH3 in household ammonia
      3. 1.49 kg of isopropyl alcohol (C3H7OH) in 2.50 L of solution, the concentration of isopropyl alcohol in rubbing alcohol
      4. 0.029 g of I2 in 0.100 L of solution, the solubility of I2 in water at 20 °C
    2. Calculate the molarity for each of the following solutions:
      1. 293 g HCl in 666 mL of solution, a concentrated HCl solution
      2. 2.026 g FeCl3 in 0.1250 L of a solution used as an unknown in general chemistry laboratories
      3. 0.001 mg Cd2+ in 0.100 L, the maximum permissible concentration of cadmium in drinking water
      4. 0.0079 g C7H5SNO3 in one ounce (29.6 mL), the concentration of saccharin in a diet soft drink

    8.E: Exercises is shared under a CC BY 4.0 license and was authored, remixed, and/or curated by LibreTexts.

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