1. Introductory Chemistry lab 213 Experiment: Application of Gas Laws
Instructor: Tabassum Ashfaq
Done by: Zainab Alnasser Manal Alsabti Aysha Al-Ansari Israa Al-Abbas
Zainab Al-Wakeel Abrar Al-Shuail

2. Outline:
Introduction
Illustration of the experiment.
conclusion

3. Introduction:
There is an ideal gas equation where we can determine the behavior of many gases under many conditions.
It was first stated by a man called “Émile Clapeyron”, where he combine Boyle’s law and Charel’s law.
In and 1857 two men could derived that equation from the Kinetic energy.

4. The Equation:
(n) is the state of an amount of gas determined by its volume, temperature, and pressure. Note that the temperature used in this equation is in the SI unit which is Kelivn. The volume in liters, and the pressure in atm.
R= P.V/n.T

5. The Experiment and the idea behind it!
In this experiment we used the hydrogen gas by dissolving magnesium metal (Mg) in an excess of hydrochloric (HCl) Acid.
To get the hydrogen gas we collected it by the displacement of water. The gas we collected was a mixture of gas and water vapor or you can call it ( wet hydrogen gas)

6. The given table for the experiment!
Data:
Mass of magnesium
Final water level(ml)
Temperature of water and hydrogen gas
Vapor pressure of water (mmhg)

7. What you need is:
As you can see, a beaker filled with water, a buret, a pipette filler, a funnel, a thermometer, a small piece of magnesium metal and HCl (hydrochloric acid)
What we used!

8. First:
you should weight the small piece of magnesium. Then record the mass in the table given
Experiment!

9. Mass of magnesium
.0193
Final water level(ml)
Temperature of water and hydrogen gas
Vapor pressure of water (mmhg)

10. Add 10ml Acid! 1: : :

11. AFTER THAT ADD DISTILLED WATER
BUT DO Not fill it to the top

12. Now bend the magnesium strip
Be careful not to bend too much place it in the buret to a depth at least 5cm.

13. Then fill it with distilled water until the magnesium strip submerge.
Now using a glass rod
Push the strip down carefully. The strip must be acting like a spring against the buret sides.
Then fill it with distilled water until the magnesium strip submerge.

14. To cover the top of the buret.
Now place your thumb
To cover the top of the buret.

15. Now carefully!!
Turn the buret over and put it inside the beaker. **Remove your thumb when the top or (the mouth) of the buret is under water

16. Magnesium reacting with the Acid
The density of Acid is higher than water so it will sink and when it reaches the magnesium strip it will start reacting.

17. See the hydrogen gas
Starts evolving

18. After the reaction is complete
One: Adjust the position of the buret until the water levels inside and outside are equal. Read the level of the water and record on the data sheet
Second: measure the temperature of the water and record the information as well.
Mass of magnesium
.0193
Final water level(ml)
8 ml
Temperature of water and hydrogen gas
21 ˚C
Vapor pressure of water (mmhg)

19. The vapor pressure of water
It will be given according to the temperature and the water level
Mass of magnesium
.0193
Final water level(ml)
8 ml
Temperature of water and hydrogen gas
21 ˚C
Vapor pressure of water (mmhg)
18.7 mmhg

20. Now we will start calculating:
Molar mass of Mg: from the Periodic table = 24.3 g/mol
Moles of Mg reacted: mass/molar mass /24.3= moles.
Moles of Hydrogen gas (n): its going to be equal to the moles of Mg reacted = moles
Temperature (T) in SI units: 21˚C+273= 294 K
Pressure of dry hydrogen gas (p) (atmospheres): P= pressure(760 mmHg- vapor pressure of water) = = we divide it by 760 to get it in atm unit
Volume of hydrogen gas (V in liters): we used small pipette max(25) so the final water level= 17ml /1000 = .017 L

21. The R constant
Finally to find the constant R We just need to substitute in the main formula
R=P.V/n.R.T
=.9754 X .017 / X 294
= L.atm/K per moles

22. Conclusion
There are many equations for calculating the pressure, the volume, or the temperature for gases. But there’s only one equation that combines the other equations. It’s called the idea gas pressure
In conclusion we could calculate the constant R for all ideal gases. Under certain pressure and temperature, no matter what gas you make or use in your experiment, eventually you find the same constant R which is And that’s why they called it the ideal gas equation.
P.V=n.R.T

23. Thank you
Hope you enjoyed it 