Experiment No. 1

Group No. Name: | Date Performed: | Course & Section: | Date Submitted: | Program & Year: | Professor: |

Experiment 1
GASLAWS
A. Combined Gas Law Temperature of Boiling Water in Kelvin (T1) | | Temperature of Cold Water in Kelvin (T2) | | Atmospheric Pressure in mm Hg (P1) | | Vapor Pressure of Water at T2 in mm Hg | | Final Pressure of Air in mm Hg (P2) | | Volume of Water Collected in the Flask in mL (Vwater) | | Initial Volume of Dry Air in mL (V1) | | True Value of the Final Volume of Air in mL (V2) | | Experimental Value of V2 in mL | | Percent Error | |

Show the calculations for the following: 1. Final Pressure of the Air

2. True Value of the Final Volume of the Air

3. Experimental Value of V2

4. Percent Error

Why do we have to dry the Erlenmeyer flask at the start of the experiment?

What is the reason for making the levels of the water the same inside and outside the Erlenmeyer flask while it was submerged in cold water?

What are the possible sources of errors in this experiment?

B. Graham’s Law of Diffusion Distance Travelled by Ammonia in cm (dNH3) | | Distance Travelled by Hydrogen Chloride in cm (dHCl) | | Molar Mass of Hydrogen Chloride in g/mole (MHCl) | | Experimental Molar Mass of Ammonia in g/mole (MNH3) | | True Molar Mass of Ammonia in g/mole (MNH3) | | Percent Error | |

Show the computations for the following: 1. Experimental Molar Mass of Ammonia

2. Percent Error

Why should the glass tubing be dry?

What are the possible sources of errors in this experiment?

CONCLUSION

REPORT