This e-lesson consists of 3 objectives; 5.12, 5.15 and 5.11. I’ll e-mail the other objective separately. Instructions for Objective 5.12 and 5.15 1. 5.12+5.15 Starter. Watch the video and think about the question. No need to type anything. 2. 5.12+5.15 Questions. Open the animation. Forward this e-mail to your blog and complete the questions. 3. 5.12+5.15 Plenary. Open the attached ppt. View as slide show. Think about what the blanks in the table are. Check your answers with slide 2. No need to type anything. 4. Answers to step 2 will be sent separately. Don’t look at them until you’ve done the work!
5.12+5.15 Starter 02 November 2011 16:15 > Questions
· Why does the needle on the meter move when gas particles are introduced into the box?
· What does the meter measure? Answers
· The gas particles collide with all of the walls of the container. The wall on the right moves outwards and moves the needle.
· Pressure. The gas particles colliding with the walls makes a force on the walls. The walls have a surface area so the quantity measured is pressure, p=F/A. 5.12+5.15 Questions 02 November 2011 15:55
· 5.12 recall that molecules in a gas have a random motion and that they exert a force and hence a pressure on the walls of the container
· 5.15 understand that an increase in temperature results in an increase in the speed of gas molecules
[cid:image001.png@01CC9986.E18EA0B0] Try the animation http://www.lon-capa.org/~mmp/kap10/cd283.htm
1. How do the particles create a pressure?
-> The particles 'bump' into the wall, and as they have the kinetic energy, this energy is exerted on the wall when the particles collide with the wall - this energy is known as 'pressure'
2. If you increase the temperature, how does the movement of the particles change?
-> By increasing the temperature, you increase the average kinetic energy of the fluid, therefore the particles have more energy and they move around faster.
3. If you increase the temperature, how does the number of collisions per second change?
-> The number of collisions/second would increase, as they move faster, so they have a higher chance of colliding with both each other, and the wall (collision theory)
4. If you increase the temperature, what does this do to the pressure?
-> By increasing the temperature, you increase the amount of collisions per second (particles with the wall), meaning that in a given period of time, more force is exerted on the same amount of surface area and from the equation: p = F/A, this means that the pressure would thereby also increase.
5.12+5.15 Plenary 02 November 2011 15:55 > 
5.12+5.15 Starter 02 November 2011 16:15 > Questions
· Why does the needle on the meter move when gas particles are introduced into the box?
· What does the meter measure? Answers
· The gas particles collide with all of the walls of the container. The wall on the right moves outwards and moves the needle.
· Pressure. The gas particles colliding with the walls makes a force on the walls. The walls have a surface area so the quantity measured is pressure, p=F/A. 5.12+5.15 Questions 02 November 2011 15:55
· 5.12 recall that molecules in a gas have a random motion and that they exert a force and hence a pressure on the walls of the container
· 5.15 understand that an increase in temperature results in an increase in the speed of gas molecules
[cid:image001.png@01CC9986.E18EA0B0] Try the animation http://www.lon-capa.org/~mmp/kap10/cd283.htm
1. How do the particles create a pressure?
-> The particles 'bump' into the wall, and as they have the kinetic energy, this energy is exerted on the wall when the particles collide with the wall - this energy is known as 'pressure'
2. If you increase the temperature, how does the movement of the particles change?
-> By increasing the temperature, you increase the average kinetic energy of the fluid, therefore the particles have more energy and they move around faster.
3. If you increase the temperature, how does the number of collisions per second change?
-> The number of collisions/second would increase, as they move faster, so they have a higher chance of colliding with both each other, and the wall (collision theory)
4. If you increase the temperature, what does this do to the pressure?
-> By increasing the temperature, you increase the amount of collisions per second (particles with the wall), meaning that in a given period of time, more force is exerted on the same amount of surface area and from the equation: p = F/A, this means that the pressure would thereby also increase.
5.12+5.15 Plenary 02 November 2011 15:55 >
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