Using the ideal gas law we can correct the atmospheric pressure of liquid in the tube different from that in the beaker.
The ideal gas law, PV = nRT
This law is used to evaluate the gas law constant R in this experiment. When determining R, the other parameters P, V, n, and T of the equation must be available from experiment. This means that it can be measured in the laboratory.
This experimental procedure is based on the chemical reaction of metallic magnesium and hydrochloric acid to produce hydrogen gas. The volume, pressure, and temperature at which hydrogen is collected are measured. From the known amount of magnesium used and the stoichiometry of the subsequent reaction, the number of moles of hydrogen produced can be calculated.
Mg(s) + 2 HCl(aq) → MgCl₂ (aq) + H₂ (g)
Once the hydrogen is collected in the eudiometer tube above the aqueous solution, the reaction is complete. To find the pressure PH₂of hydrogen gas, the vapor pressure of water PH₂O at the measured temperature must be subtracted from the atmospheric pressure Patm. Therefore, the pressure of hydrogen is
PH₂ = Patm – PH₂O
If the liquid level (step 3) cannot be equalized after the reaction is complete, further correction is required as the pressure of the gas (hydrogen and hydrogen) in the tube . Water vapor does not equal atmospheric pressure. In such cases, the level difference should be measured as accurately as possible with a meter stick. Note that the tube scale is in milliliters, not millimeters. We should use a meter stick or ruler. This difference, which represents the desired pressure difference, must be converted to mm or Hg. This can be achieved by dividing the measured height difference in millimeters by 13.5 (the ratio of Hg to the density of the aqueous solution).
To learn more about Atmospheric pressure, refer:
https://brainly.com/question/15215203
#SPJ4
