Description
ANES 500
Chapter 8 Assignment
Name: __________________ Due 11:30 pm on 11/01/2021
Fall 2021_2022
Grade__________
General Instructions
Provide suitable responses for the problems shown below. The assignment is to be completed
individually and returned by 11:30 pm EDT on Monday, November 1, 2021. Where applicable,
show your work to receive full credit. Late assignments will be assessed a penalty of 10 % of the
overall grade per day late.
How to Return This Assignment
You may upload the document to the drop box in Canvas as a Word file, a pdf file, a jpeg file, a
scanned file, etc. The document may also be returned as an email attachment in canvas. If
the file is too large, try compressing it using free services such as wecompress.com. Do not
return the file using our outlook email. For those who save each page of the assignment as a
pdf or image file, you may combine them into one document as follows:
•
Locate the files in Windows File Explorer.
•
Right click on the first file.
•
Choose “Combine Supported Files in Acrobat…” A new dialog box will pop up, but you
may have to minimize other files to see it.
•
Drag the files from Explorer into this box.
•
If necessary, change the order of the files using “Move Up” or “Move Down.”
•
Click on “Combine Files.” You will be prompted for a file name.
If applicable, you may also copy and paste images in a Word document, and then save the
document as a pdf file. Instructions for writing or type on a pdf document will be sent to you
as a separate document. Please ensure that your work is legible and your file is complete
before and after sending.
ANES 500
Chapter 8 Assignment
Name: __________________ Due 11:30 pm on 11/01/2021
Fall 2021_2022
Grade__________
1. Consider the contents of Flasks I – IV when answering questions 2(a) to 2(e). Flask I contains
a glucose solution. Flasks II and III contain pure water. Flask IV contains a red blood cell
suspended in a saline solution of unknown concentration. (5 Pts)
(a) If Flask I and Flask II were heated equally, which liquid will boil first?
(b) If Flask I and Flask II were heated to 50 oC, which flask, if any, would have the lower
vapor pressure?
(c) If Flask I and Flask III were placed in a freezer, which liquid will freeze first?
(d) If the temperature in Flask I is 10 oC higher than in Flask III, which flask will have the
higher vapor pressure?
(e) Is the solution in Flask IV isotonic, hypertonic, or hypotonic? The arrows indicate the net
movement of water.
2. Decide whether the following statements are true (T) or false (F): (6 pts)
(a) Colligative properties depend on the number of molecules present, not on the kind of
molecules used.
(b) Under identical conditions, the vapor pressure of a solution is expected to be higher than
that of the pure solvent from which it is made.
(c) Adding a nonvolatile solute to a pure solvent will decrease its freezing point.
(d) Adding a nonvolatile solute to a pure solvent will increase its vapor pressure.
(e) Adding a nonvolatile solute to a pure solvent will increase its boiling point.
(f) Osmotic pressure is not a colligative property and has no dependence on solute
concentration.
3. The allowable concentration of lead in drinking water is 0.0015 mg per 100 grams. (a) What
is this concentration in parts per million (ppm)? (b) What is this concentration in parts per
billion (ppb)? (c) In some countries, the allowable concentration of manganese in water is
0.0500 ppm. What is this concentration in mg per 100 grams? (6 pts)
4. A solution is prepared by dissolving 1.25 gram of KCl in enough water to give 275 mL of
solution. (a) How many moles of KCl are in the solution? (b) How many millimoles of KCl
are in the solution? (c) What is the molarity of the solution? Show your work and report your
answers to 3 significant figures. (6 pts)
5. Calculate the percent concentration (w/v) of KCl in the previous problem. Show your work
and report your answers to 3 significant figures. (4 pts)
6. How many grams of glucose are there in 775 milliliters of a 15% (w/v) glucose solution?
Show your work and report your answers to 3 significant figures. (4 pts)
7. A reaction calls for 0.311 mole of glucose. (a) Calculate the mass of glucose that is required
for this reaction. (b) If the available glucose solution has a molarity of 2.50 mole/liter (2.50
Molar), how many milliliters of this solution will be needed to supply the 0.311 mole of
glucose? Show your work and report your answers to 3 significant figures. (6 pts)
7. A solution contains 0.130 mole CaCl2, 0.275 mole of NaCl, and 0.250 mole of MgCl2, how
many mEq of each ion are in the solution? Show your work and report your answers to 3
significant figures. (6 pts)
8. A solution is prepared by dissolving 5.50 grams of MgCl2 in enough water to give 375 mL of
solution. Calculate (a) the molarity and (b) the normality of the solution. Show your work
and report your answers to 3 significant figures. (6 pts)
9. How many grams of KCl are needed to prepare 255 mL of a 1.13 % KCl solution (w/v)?
Show your work and report your answers to 3 significant figures. (4 pts)
10. A solution contains 0.25% (w/v) Xanax. (a) What is its concentration in mg/cc? How many
milligrams of Xanax can be obtained from 3.00 cc of this solution? Show your work and
report your answers to 2 significant figures. (5 pts)
11. (a) A solution is labeled 1:90,000. (a) Determine the dosage equivalence in mg/cc. (b) What
is the dosage equivalence in percent concentration? (c) How many milligrams of the
medication are in 10.0 cc of this solution? Show your work and report your answers to 3
significant figures. (6 pts)
12. Calculate the molality of a KCl solution that contains 5.52 grams of KCl in a total of 112
grams of solution. Show your work and report your answer to 3 significant figures. (5 pts)
13. Calculate solubility of CO2 in water at 25.0 oC if its partial pressure is 3.20 atm. Assume kH
for CO2 is 3.10 x 10-2 mole/(L.atm). Show your work and report your answer to 3 significant
figures. (5 pts)
14. A solution is prepared by dissolving 21.5 grams of glucose to a total volume of 0.250 L. (a)
What is the molarity of the solution? (b) If the temperature of the solution is 25.0 oC, what is
its osmotic pressure? π = MRT. R = 0.08206 L.atm/K.mole. Show your work and report
your answers to 3 significant figures. (5 pts)
ANES 500
Exam 4, Part 2
Fall 2021_22
Name_________________
Due 11:30 pm on 11/8/2021
Grade__________
General Instructions
Provide suitable responses for the problems shown below. The exam is to be completed
individually and returned by 11:30 pm EDT on Monday, November 8, 2021. Where applicable,
show your work to receive full credit. Late assignments will be assessed a penalty of 10 % of the
overall grade per day late. Exams submitted after answers are posted will not be accepted.
How to Return This Assignment
You may upload the document to the drop box in Canvas as a Word file, a pdf file, a jpeg file, a
scanned file, etc. The document may also be returned as an email attachment in canvas. If the file
is too large, try compressing it using free services such as wecompress.com. Do not return the file
using my outlook email. For those who save each page of the assignment as a pdf or image file,
you may combine them into one document as follows:
•
Locate the files in Windows File Explorer.
•
Right click on the first file.
•
Choose “Combine Supported Files in Acrobat…” A new dialog box will pop up, but you
may have to minimize other files to see it.
•
Drag the files from Explorer into this box.
•
If necessary, change the order of the files using “Move Up” or “Move Down.”
•
Click on “Combine Files.” You will be prompted for a file name.
If all else fails, you may fax the document to the attention of Dr. Farrell using Fax: 407-303-8136.
Please ensure that your work is legible, and your file is complete before sending. Exams
submitted after answers are posted will not be accepted.
Name____________________
Due 11:30 pm on 11/8/2020
Grade__________
1. Determine whether each of the following statements are true (T) or false (F): (10 pts)
(a) When the particles in an ideal gas collide, part of their kinetic energy is changed to other
forms of energy.
(b) An elastic collision is one in which there is some no loss of kinetic energy.
(c) The particles in a liquid are much further apart than those in a gas.
(d) There are no forces of attraction or repulsion between particles in an ideal gas.
(e) Increasing the temperature of a gas increases the speed of its particles.
(f) Increasing the temperature of a gas in a container will not affect its pressure if the volume
is constant and the number of gas particles remain the same.
(g) The pressure of a gas is inversely proportional to its volume, even when its temperature is
not constant.
(h) If the gas in a cylinder does not expand when it is heated, its pressure will increase.
(i) According to Charles’s law, the volume of a gas is proportional to its absolute temperature.
Therefore, if the temperature of a gas doubles from 25 oC to 50 oC, its volume will also
double
(j) The number of molecules in a gas is directly proportional to the volume of the gas at
constant pressure and temperature.
2. Which of the following statements is not consistent with the properties of a gas? (3 pts)
(a) A gas occupies more space and is less dense than the liquid or solid from which it is
formed.
(b) The particles in a gas do not attract or repel each other.
(c) The particles in a gas collide with each other.
(d) Gases compress more easily than liquids and solids.
(e) The particles in a gas loses kinetic energy with each collision.
3. The graph below shows the vapor pressure of two pure solvents as a function of temperature.
(a) What is the vapor pressure of Solvent A at 20 oC? (b) What is the vapor pressure of Solvent
B at 90 oC? (c) If a nonvolatile solute was dissolved in Solvent B at 90 oC, will its vapor
pressure increase or decrease? (d) Which solvent has the stronger intermolecular force? (4 pts)
4. Identify the three different gas laws that are depicted in the graphs shown below. (3 pts)
5. (i) The plot shown below is a graphical representation of which of the following gas laws? (2
pts)
(a) Charles’s law
(b) Avogadro’s law
(c) Ideal gas law
(d) Gay-Lussac’s law
(e) Boyle’s law
(ii) Use the above graph to estimate the volume of the gas at 500 K. (2 pts)
6. Which of the following gases would be expected to have the fastest effusion rate? (3 pts)
(a) C3H8
(Propane)
(44.10 g/mol, d = 1.9397 kg/m3)
(b) C2H4
(Ethylene)
(28.05 g/mol, d = 1.2340 kg/m3)
(c) CO
(Carbon monoxide)
(28.01 g/mol, d = 1.2321 kg/m3)
(d) CH4
(Methane)
(16.04 g/mol, d = 0.7057 kg/m3)
(e) H2
(Hydrogen)
(2.02 g/mol, d = 0.0887 kg/m3)
7. Which of the following changes would lead to an increase in the pressure of the gas in the
aluminum cylinder shown below? Assume that the cylinder contains one mole of CO2 gas.
Circle all that apply. (3 pts)
(a) Using a cylinder made of a different metal while keeping everything else the same.
(b) Reducing the number of CO2 collisions occurring within the container.
(c) Increasing the temperature of the CO2 gas.
(d) Partially squeezing the walls of the container together with a can crusher, while keeping
everything else the same.
(e) Replacing ½ mole of the CO2 with ½ mole of glucose but keeping everything else the
same.
8. The gas cylinder shown below contains an ideal gas under different experimental conditions.
(a) Which gas law best describes the behavior of this gas? (b) Calculate the final pressure of
the gas in atm and in mmHg. (c) Decide if the pressure in the right cylinder will increase,
decrease, or remain the same if the gas temperature increases by 10 oC, but at a fixed volume
of 15.8 L. Show your work and report your answer to 3 significant figures. (6 pts)
9. A sample of CO2 has a volume of 256 mL at 26.6 oC and 1.13 atm. (a) What will be the
volume of this gas at – 44.5 oC and 1.13 atm? (b) If the pressure remains constant at 1.13 atm,
will the moles of gas (n) change if the volume (V) and the absolute temperature (T) of the gas
double? Show your work for part (a) and report your answer to 3 significant figures. (6 pts)
10. (a) Which of the two gases shown below would effuse faster? (b) How much faster would this
gas effuse? Show your work and report your answer to 3 significant figures. (4 pts)
Gas A: C3H8 (Mm 44.10 g/mol)
Gas B: C2H4 (Mm 28.05 g/mol)
11. A mixture is made up of 221 grams CO2 and 63.0 grams of N2. (a) Calculate the moles of each
gas in the mixture. (b) What is the mole fraction of N2 in the mixture? (c) If the total pressure
of the mixture is 779 torr, calculate the partial pressure of N2 in the mixture. Show your work
and report your answers to 3 significant figures. (6 pts)
12. (a) A balloon contains 1.56 liters of helium at 283 K and 0.989 atm. What change in
temperature will be required to increase the volume of the balloon 1.98 liters and change its
pressure to 1.07 atm? (b) A second balloon contains 15.6 liters of helium at 298 K and 1.00
atm. Use the ideal gas law to calculate the moles of helium in the balloon. Show your work
and report your answers to 3 significant figures. (6 pts)
13. A 2.00-liter balloon contains 0.0611 mole of helium at a temperature of 298 K and a pressure
of 0.747 atm . If the volume of the balloon increased to 2.76 liters at the same temperature and
pressure, how many moles of helium are now in the balloon? Show your work and report your
answer to 3 significant figures. (4 pts)
14. A 2.00-L balloon contains 0.0315 moles N2 and 0.0215 moles CO2 at 299 K. (a) Use the ideal
gas law to calculate the partial pressure of N2 in this mixture. (b) Calculate the partial pressure
of CO2 in the mixture. (c) Calculate the total pressure of the two gases in atmospheres. Show
your work and report your answers to 3 significant figures. R = 0.08206 L.atm/K.mole. (6 pts)
15. A vessel contains 2.15 liters of CH4 gas at a temperature of 312 K and a pressure of 2.17 atm.
(a) Use the ideal gas equation to calculate the moles of CH4 in the cylinder. (b) What is the
mass of CH4 in the cylinder? Show your work and report your answer to 3 significant figures.
(5 pts)
16. A second vessel contains CH4 gas at a temperature of 211 K and a pressure of 0.998 atm.
Calculate the density of CH4 in grams per liter. Show your work and report your answer to 3
significant figures. (4 pts)
17. A solution is made by dissolving 15.0 g of glucose (C6H12O6) in 137 g of water. (a) Calculate
the percentage (w/w) of glucose in the solution. (b) What is the molality of this solution? Show
your work and report your answer to 3 significant figures. (5 pts)
18. A solution is made by dissolving 0.0228 g of glucose (C6H12O6) in enough water to make 448
mL of solution. (a) What is the molarity of this solution? (b) What is the concentration of this
solution in mg/mL? (c) What is the concentration of this solution in ppm? Show your work and
report your answers to 3 significant figures. (6 pts)
19. A 2.00-Liter solution contains 0.431 mole each of BaCl2 and MgCl2. (a) How many Eq of each
ion are in the solution? (b) Find the normality of Ba2+ ions in the solution. Show your work and
report your answers to 3 significant figures. (6 pts)
20. How many grams of glucose are needed to prepare 275 mL of a 10.5 % glucose solution (w/v)?
Show your work and report your answers to 3 significant figures. (4 pts)
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