# IB Chemistry - Charles' Law Lab Report

Gas laws experiment

Relationship between Volume and Temperature and find Absolute Zero

Aim: to measure accurately the volume of a fixed mass of gas at different temperatures and use these data to determine the relationship between the variable and to determine absolute zero, the temperature at which the volume would theoretically drop to zero.

Raw data

1. The volume of water in 250ml beaker = 150ml

Data Processing

1. % of uncertainty on temperature = 0.5/temperature*100 = 0.5/24*100 = 2.08 = ±2%
2. Absolute uncertainty on temperature = temperature*% of uncertainty on temperature = 24*2% = ±0.48
3. Kelvin = ℃+273 = 24+273 = 297
4. Height = End of capillary – Bottom of bubble = 6.0 – 2.2 = 3.8cm
5. % of uncertainty on height = % of uncertainty on the end of capillary + % of uncertainty on the bottom of bubble = (0.05/6.0*100) + (0.05/height*100) = 0.83+ (0.05/3.8*100) = 0.83 + 1.32 = 2.15= ±2%
6. Absolute uncertainty on height = Height*% of uncertainty on height = 3.8*2% = ±0.076
7. H(V)/T = k(constant) = 3.8/279 = 0.014 (Temperature should be replaced into Kelvin)
8. % of uncertainty on constant = % of uncertainty on temperature + % of uncertainty on height = 2 + 2 = 4%
9. Absolute uncertainty on constant = constant*% of uncertainty on constant

= 0.014*4% = 5.6*10∧-4

Questions

• Form the graph that has been made by the result of the experiment, the relationship between temperature and height (which is same as height in this experiment) was directly proportional.
• The Charles’ law defined that the relationship between temperature and the volume for a gas at constant pressure is linear or V=k (constant)T. Every gas we use gives the same value of temperature for this intercept, -273℃ and the behaviour of gases tells us that the temperature has an absolute zero. So if I want to double the volume at constant pressure of ...