Title | Lab #4 charles |
---|---|
Course | General Chemistry I |
Institution | California State University Dominguez Hills |
Pages | 5 |
File Size | 238.1 KB |
File Type | |
Total Downloads | 91 |
Total Views | 114 |
Lab report for Charles law...
Charles’ Law
CHE 110-07
10/11/2017
Introduction: In this week’s experiment, we verified the linear relationship between volume and temperature; it is called Charles’ Law. We were to determine the volume at absolute temperature by graphical analysis. In this experiment, the volume of a given amount of air trapped in a graduated pipet is measured as a function of temperature.
Charles’ Law states that at constant pressure, the volume of a fixed amount of an ideal gas is proportional to its absolute temperature. Data: Temper at ur e
Vol ume( mL) bot t om
Vol ume( mL) t op
Netv ol umeof ai r( mL )
Room Temper at ur e
19. 9º C
7. 62mL
5. 61mL
2. 01mL
HotWat er
77. 5º C
7. 49mL
3. 61mL
3. 88mL
72. 5º C
7. 49mL
3. 60mL
3. 89mL
67. 5º C
7. 50mL
3. 75mL
3. 75mL
62. 5º C
7. 50mL
3. 81mL
3. 69mL
57. 5º C
7. 50mL
3. 88mL
3. 62mL
52. 5º C
7. 51mL
3. 95mL
3. 56mL
47. 5º C
7. 51mL
4. 00mL
3. 51mL
42. 5º C
7. 51mL
4. 04mL
3. 47mL
37. 5º C
7. 52mL
4. 12mL
3. 40mL
32. 5º C
7. 53mL
4. 17mL
3. 36mL
4. 1º C
7. 57mL
4. 57mL
3. 00mL
Col dWat er
Today’s atmospheric pressure: 760mmHg Density of air: 0.001205 g/mL
Graphs and calculations: 1.
2. n= (.00201 L)(1.205 g *L-1)/29.0 g*mol-1 = 8.352 x10^-5 moles 3. R=CP/n =(.00001838)(1)/8.352 x10^-5 =0.22 L*atm/mol K 4. R=0.08206 L*atm/mol K
Results and discussion: What I learned from today’s lab is how volume and temperature relate to each other when taking the measurements and plotting them in a graph.
Definitely, possible error such as heat from our hands can transfer over to graduated cylinder which could change temperature of water.
Questions: 1. This experiment deals with the relationship between volume and temperature for a fixed amount of gas at constant pressure. Design an experiment, which would allow you to study the relationship between pressure and temperature for a fixed amount of gas at constant volume. Show a diagram of the apparatus and a plot of P versus T for the data you expect to obtain. Is the relationship between P and T direct or
inverse?
As the temperature increases the pressure also increases and vice versa. 2. In this experiment, air was assumed to be an ideal gas. Does this assumption lead to a significant error? Explain your answer? This assumption would probably not lead to significant error unless the experiment is conducted through a change that would change the gas. 3. Show by calculation that the weighted-average “molecular weight” of air is 29.0 g ⋅ mol-1.
O 2 and N 2 are prevalent in air and make up almost entirely all of an air molecule. 6.704 (O 2 ) + 21.88(N 2 ) = 29 g(mol-1)...