Video-Charles Law ExperimentÃ¯Â¼Å¡

Charles Law- data sheet

on the fileÃ£â‚¬â€š

Data Table:

Trial 1

Trial 2

Temperature of boiling water (T1)

100. Ã‚Â°C

100. Ã‚Â°C

Temperature of air after cooling on the water bath

(T2)

23.0 Ã‚Â°C

23.0 Ã‚Â°C

Initial volume of air in the flask at the temperature

of boiling water (V1)

138 ml

255 mL

Volume of water drawn into the flask (V H20 )

26.0 mL

47.0 mL

Volume of moist air (V2 wet) drawn into the flask

when cooling. V2 wet = V1-V H2O

Volume of air collected at the cool temperature

after the vapor pressure correction in Equation 2.

(V2 measured)

Volume of air collected at the cool temperature

calculated using Charles’ Law (V2 calculated)

Atmospheric pressure in mmHg (P total)

760. mmHg

760. mmHg

Water vapor pressure (in mmHg) at temperature T2

(P water) (from Table 1)

Percent error between V2 measured and V2

calculated

Table I. Vapor Pressure of Water as a Function of Temperature

Temperature (0)

Vapor Pressure (mm) Temperature (C) Vapor Pressure (mm)

20

21

10

11

12

13

14

15

16

17

18

19

9.2

9.8

10.5

11.2

12.0

12.8

13.6

14.5

15.5

16.5

17.5

18.6

19.8

21.1

22.4

23.8

25.2

26.7

28.3

29

30

30.0

31.8

Calculations:

a. The air collected in the flask at the lower temperature also contains water vapor. So we refer

to this volume as Vz wet. We can calculate V2 wet by subtracting the volume of water (V H20)

drawn into the flask from the initial volume of air in the flask V1.

b. In order for us to calculate the volume of air collected at the cool temperature (V2 measured)

, we have to use a vapor pressure correction. This correction is done using the Daltons Law of

Partial Pressures. In Equation 2, we subtract the vapor pressure of water in the flask at the

cooler temperature to calculate the experimental value of V2 (V2 measured).

P total-P water

V2 measured=V2 wet x

Equation 2

P total

C. Using Charles’ Law calculate the theoretical value for V2 (V2 calculated) by substituting values

for V1, T1 and T2 in equation 1. Show your work below.

d. Calculate the Percent error in between your experimental and theoretical value for V2:

|V2 measured-V2 calculated

% error=

x 100%

V2 calculated

Show your work for calculating % error:

Name:

Discussion questions:

1. Why do we need to clamp the rubber tube when we are transferring the flask from the boiling

water to the cool water? Explain how this will affect your results.

2. If a balloon holds 3.7 L of gas at 25 Ã‚Â°C, what will be the volume of the balloon at 46 Ã‚Â°C?

Assuming constant pressure. Show your work.

3. Discuss two sources of error in this experiment that might account for a high percentage error

between V2 measured and V2 calculated.

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