SCH3U1

Gas Assigned:

GAS NUMBER / PAGE NUMBER / NAME
1. / 2-3 / Darius E., Connor
2. / 4-5 / Taylor, Liz
3. / 6-7 / Harrison, Stefan SB
4. / 8-9 / Bassi, Max
5. / 10-11 / Bill, Andrew M.
6. / 12-13 / Darius R.
7. / 14-15 / Andrew J.
  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:hydrogen

Mass of the Gas:6.0 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 42.6
-60 / 52.4
-20 / 62.3
20 / 72.1
60 / 82.0
100 / 91.8
140 / 101.7
180 / 111.5
220 / 121.4

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important:Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volumeon your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extendingthe line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:oxygen

Mass of the Gas:100 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 44.4
-60 / 54.6
-20 / 64.0
20 / 75.1
60 / 85.4
100 / 95.6
140 / 105.9
180 / 116.2
220 / 126.4

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:carbon dioxide

Mass of the Gas:220Pressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 71.0
-60 / 87.4
-20 / 103.8
20 / 120.2
60 / 136.6
100 / 153.0
140 / 169.4
180 / 185.8
220 / 202.3

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:carbon dioxide

Mass of the Gas:2000 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 645.2
-60 / 794.4
-20 / 943.6
20 / 1092.8
60 / 1242.0
100 / 1391.1
140 / 1540.3
180 / 1689.5
220 / 1838.7

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:helium

Mass of the Gas:25 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 88.7
-60 / 109.2
-20 / 129.7
20 / 150.3
60 / 170.8
100 / 191.3
140 / 211.8
180 / 232.3
220 / 252.8

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:nitrogen

Mass of the Gas:100 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 50.7
-60 / 62.4
-20 / 74.1
20 / 85.9
60 / 97.5
100 / 109.3
140 / 121.0
180 / 132.7
220 / 144.5

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.

4. a) Calculate the number of moles of your gas,

b) Based on the volume of the gas at 0oC, what is the molar volume (the volume of 1 mole of your gas) at this temperature? (molar volume = V/n)

5. Charles’ Law describes the relationship between temperature and volume of a gas. Using the internet, research and state Charles’ Law in words and as a formula.

Making Connections:

1. Aerosol cans bearing this symbol warn against placing them near sources of heat.

a) What does Charles’ Law predict will happen to the volume of the gas in an aerosol can as the temperature is increased?

b) The volume of an aerosol can is fixed and cannot change. How will heating the can affect the pressure within the container?

c) What could eventually occur as the can is heated?

2. Jacques Charles was interested in ballooning as a hobby.

a) Calculate the density of your gas at any 2 temperatures.

b) What happens to the density of a gas as it is heated?

c) Why would this relationship be very interesting and useful for Charles and his hobby?

3. The x-intercept value that you determined is only a theoretical value. What will actually happen to the gas you have studied when it is cooled to a very low temperature?

SCH3U1

  1. Charles’ Law

Goal:To determine the relationship between the volume and the temperature of a gas when the pressure and mass are held constant.

Name of the Gas:chlorine

Mass of the Gas:120 gPressure:101.3 kPa

Temperature (oC) / Volume (L) / Temperature (K) / V/T (L/K)
-100 / 24.0
-60 / 29.5
-20 / 35.1
20 / 40.6
60 / 46.2
100 / 51.7
140 / 57.3
180 / 62.8
220 / 68.4

Analysis:

1. Plot a graph of volume (y-axis) vs. temperature (x-axis). Important: Set up the x-axis for temperature values from -300 oC to 240 oC. Set up the y-axis for volumes from 0 to x Litres (where x is slightly greater than your highest volume on your data table). Be sure to include a descriptive title, labeled axes and units on your graph.

2. Draw a solid line of best fit through your data points. Extrapolate the relationship to lower temperatures by extending the line of best fit as a dashed line until it intersects the x-axis.

3. Convert each temperature from Celsius to Kelvin and record.

4. Calculate the ratio V/T by dividing the volume by the Kelvin temperature and record.

Questions:

1. What relationship do you observe between the temperature and volume of a gas?

2. At what temperature does the line of best fit intersect the temperature axis? What is the significance of this temperature?

3. When Jacques Charles’ carried out a similar experiment, he determined this value to be

-273oC. Assuming this was correct, calculate the percentage error for your value.