The resulting difference in the mercury levels will be equal to the final pressure of the gas. By manually moving the right tube up, we put still more pressure on the gas and force it to shrink to its original volume. When the temperature rises, the gas expands and pushes the mercury in the left tube down until the increased difference of mercury levels between the two tubes equalized that pressure. You should be able to see how it works if you look at the diagram below (based on the image copied from this document). Since the mercury in the first tube is kept at the same level, the volume of gas does not change and we can apply the Gay-Lussac's law.
The mercury level does not reach Zero by itself - it is brought to Zero by physically moving the second tube up or down. Why every time the mercury level should reach Zero in the first tube? The pressure changes with temperature according to the Gay-Lussac's law, which says (according to Wikipedia) that "for a given mass and constant volume of an ideal gas, the pressure exerted on the sides of its container is directly proportional to its absolute temperature". How does the pressure change with the change of temperature in this
0 kommentar(er)
