Rasmussen University Chemistry Worksheet

Question 11 Point
Describe how surface area, temperature, and intermolecular forces are related to the rate of
evaporation of a liquid and vapor pressure.
Question 2
1 Point
Why can’t the kinetic molecular theory be applied to liquids and solids?
Question 3
1 Point
What are the 3 interactions that happens in a solution between the solute and the solvents? Describe
the interactions in terms of salt dissolved in water.
Question 4
1 Point
Describe the 4 standards that gases need to have in order to fit the kinetic molecular theory of gases.
Question 5
1 Point
Identify which of these gases exhibit non-ideal gas behavior:
Gas A, Gas B, Gas C, Gas D, Gas E, Gas F
Gas E
Gas D
Gas C
Gas A
Gas F
Gas B
Question 6
1 Point
A box contains 100 particles of gas at room temperature. What is the correlation between the volume
and pressure in a box containing a certain amount of gas particles and why?
Question 7
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. You are checking the purity of the air in a unit of the hospital and find the following
readings: CO2 (17.8 Pa), O2 (20.2 bar), CO (56.6 psi), N2 (71.7 mmHg), SO2 (22.4 torr), and Ar (42.3 atm).
What is the total pressure of the unit?
Question 8
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. A scuba diver has been brought into the hospital because he had to come up really
quickly since his oxygen tank was running out. The problem with doing this is that it causes a
phenomenon called “bends” where the volume of the oxygen in the blood stream can increase too
quickly if the pressure around the body is changed too quickly. If the scuba diver had 4.0 L of gas at
atmospheric pressure, what was the volume of the gas when scuba diver dove down to 130ft below sea
level (110kPa)?
Question 9
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. Patient A has a collapsed lung and needs to be airlifted to a different hospital for
treatment. You know from your schoolwork that pressure has an effect on volume, and the pressure
changes as altitude changes. If the volume of the collapsed lung is at 1435mL on the ground (1 atm),
what would the volume of the lung be at 632mmHg?
Question 10
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. How many moles of gas are in a helium tank that holds 22.4L, kept at room temperature
and atmospheric pressure?
Question 11
1 Point
In a liquid state, molecules can be compressed.
True
False
Question 12
1 Point
Liquids have more tightly packed molecules than solids.
True
False
Question 13
1 Point
Which of these examples are liquids with high vapor pressure (evaporates easily)?
Motor oil, maple syrup, honey
Rubbing alcohol, acetone, Butane, Propane
Alcohol, vinegar, acetone
Mercury, water, glycerin
Question 14
1 Point
Which of these examples are liquids with low vapor pressure (doesn’t evaporate easily)?
Glycerin, motor oil, honey
Rubbing alcohol, acetone
Gasoline, propane
Water, alcohol
Question 15
1 Point
Using the phase diagram, identify the phase that water is in for the following conditions: 98kPa and 80˚C
DiagramDescription automatically generated
Liquid
Triple point
Solid
Gas
Critical point
Question 16
1 Point
Using the phase diagram, identify the phase that water is in for the following conditions: 10000kPa and
50˚C
DiagramDescription automatically generated
Solid
Liquid
Gas
Critical point
Triple point
Question 17
1 Point
Identify which of these molecules has the highest boiling point and give the reasoning why in terms of
intermolecular force. H2O, KCl, CO2
Question 18
1 Point
Identify which of these molecules has the highest boiling point and give the reasoning why in terms of
intermolecular force. CHCl3, CH3COOH, CO2
Question 19
1 Point
Identify the following phase change as endothermic or exothermic processes: Gas to liquid
Endothermic
Exothermic
Question 20
1 Point
Identify the following phase change as endothermic or exothermic processes: Liquid to gas
Endothermic
Exothermic
Question 21
1 Point
Reference this image and identify whether the following solution is saturated, supersaturated or
undersaturated: KBr at a solubility of 60 at 20˚C
Supersaturated
Undersaturated
Saturated
Question 22
1 Point
Reference this image and identify whether the following solution is saturated, supersaturated or
undersaturated: NaBr at a solubility of 130 at 50˚C
image00460e5e3f9.gif
Supersaturated
Undersaturated
Saturated
Question 23
1 Point
Calculate the molality of the following solution: 65g of KCl in 46.6g of water
Question 24
1 Point
Calculate the molality of the following solution: 30g of NaCl in 350g of water
Question 25
1 Point
Calculate the molality of the following solution: 37g of glucose (C6H12O6 ) in 64g of water
Question 26
1 Point
Calculate the mass percent of the following solution: 13g of KBr in 93g of water
Question 27
1 Point
Calculate the mass percent of the following solution: 65g of KCl in 46.6g of water
Question 28
1 Point
Calculate the mass percent of the following solution: 37g of glucose in 64g of water
Question 29
1 Point
Describe how the boiling point and freezing point is affected when a solute is mixed into a solution.
Question 30
1 Point
Describe how temperature and pressure affects the solubility of a solute in a solution.
Part two
Question 1
1 Point
Describe how surface area, temperature, and intermolecular forces are related to the rate of
evaporation of a liquid and vapor pressure.
Question 2
1 Point
Identify which of these gases exhibit non-ideal gas behavior:
Gas A, Gas B, Gas C, Gas D, Gas E, Gas F
Gas D
Gas A
Gas C
Gas F
Gas B
Gas E
Question 3
1 Point
Describe the 4 standards that gases need to have in order to fit the kinetic molecular theory of gases.
Question 4
1 Point
Why can’t the kinetic molecular theory be applied to liquids and solids?
Question 5
1 Point
What are the 3 interactions that happens in a solution between the solute and the solvents? Describe
the interactions in terms of salt dissolved in water.
Question 6
1 Point
A box contains 100 particles of gas at room temperature. What is the correlation between the volume
and pressure in a box containing a certain amount of gas particles and why?
Question 7
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. Patient A has a collapsed lung and needs to be airlifted to a different hospital for
treatment. You know from your schoolwork that pressure has an effect on volume, and the pressure
changes as altitude changes. If the volume of the collapsed lung is at 1435mL on the ground (1 atm),
what would the volume of the lung be at 632mmHg?
Question 8
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. A scuba diver has been brought into the hospital because he had to come up really
quickly since his oxygen tank was running out. The problem with doing this is that it causes a
phenomenon called “bends” where the volume of the oxygen in the blood stream can increase too
quickly if the pressure around the body is changed too quickly. If the scuba diver had 4.0 L of gas at
atmospheric pressure, what was the volume of the gas when scuba diver dove down to 130ft below sea
level (110kPa)?
Question 9
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. It is the middle of the summer and a room in the ICU is a lot warmer than it should be. A
patient has been wheeled into the room and needs to be put on oxygen. When the room was at room
temperature, the pressure in the gas was at 250 psi for 13L of gas. What is the pressure in the gas
cylinder since the room warmed up and if the volume of the gas increased to 20L?
Question 10
1 Point
You are a nurse and you have several patients that need treatment. Thank goodness you were taught
how to manipulate gas laws in order to help the patients. Help each patient solve the issue they are
encountering. How many moles of gas are in a helium tank that holds 22.4L, kept at room temperature
and atmospheric pressure?
Question 11
1 Point
In a liquid state, molecules can be compressed.
True
False
Question 12
1 Point
In a gaseous state, molecules can move past each other.
True
False
Question 13
1 Point
Which liquid has the lowest surface tension?
Water
Mercury
Glycerin
Alcohol
Question 14
1 Point
Which of these examples are liquids with low vapor pressure (doesn’t evaporate easily)?
Rubbing alcohol, acetone
Gasoline, propane
Glycerin, motor oil, honey
Water, alcohol
Question 15
1 Point
Using the phase diagram, identify the phase that water is in for the following conditions: 22,089kPa and
374˚C
DiagramDescription automatically generated
Gas
Critical point
Solid
Triple point
Liquid
Question 16
1 Point
Using the phase diagram, identify the phase that water is in for the following conditions: 100kPa and
110˚C
DiagramDescription automatically generated
Solid
Gas
Critical point
Triple point
Liquid
Question 17
1 Point
Identify which of these molecules has the highest boiling point and give the reasoning why in terms of
intermolecular force. CHCl3, CH3COOH, H2O
Question 18
1 Point
Identify which of these molecules has the highest boiling point and give the reasoning why in terms of
intermolecular force. CHCl3, CH3COOH, CO2
Question 19
1 Point
Identify the following phase change as endothermic or exothermic processes: Solid to liquid
Exothermic
Endothermic
Question 20
1 Point
Identify the following phase change as endothermic or exothermic processes: Liquid to solid
Endothermic
Exothermic
Question 21
1 Point
Reference this image and identify whether the following solution is saturated, supersaturated or
undersaturated: NaCl at a solubility of 20 at 100˚C
Saturated
Undersaturated
Supersaturated
Question 22
1 Point
Reference this image and identify whether the following solution is saturated, supersaturated or
undersaturated: NaBr at a solubility of 130 at 50˚C
image00460e5e3f9.gif
Undersaturated
Saturated
Supersaturated
Question 23
1 Point
Calculate the molality of the following solution: 13g of KBr in 93g of water
Question 24
1 Point
Calculate the molality of the following solution: 11.6g of NaNO3 in 86g of water
Question 25
1 Point
Calculate the molality of the following solution: 30g of NaCl in 350g of water
Question 26
1 Point
Calculate the mass percent of the following solution: 4.2g of LiBr in 52.6g of water
Question 27
1 Point
Calculate the mass percent of the following solution: 65g of KCl in 46.6g of water
Question 28
1 Point
Calculate the mass percent of the following solution: 30g of NaCl in 350g of water
Question 29
1 Point
Describe how the boiling point and freezing point is affected when a solute is mixed into a solution.
Question 30
1 Point
Describe how temperature and pressure affects the solubility of a solute in a solution.
Explain the anatomical concepts associated with human development. Summarize this module’s key
points in 5-6 sentences.
Explain the physiological concepts associated with human development. Summarize this module’s key
points in 5-6 sentences.
How will you apply the concepts you have learned about human development in real life and in your
future career?
Which topic within this module has been the most valuable to your learning experience and why?

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