Falling Ball Experiment

Does the height from which a ball falls affect the depth of the hole it leaves into the gelatin?

Objective: Investigate a relationship between a falling ball and the surface it falls in. 

Hypothesis:

The height is directly proportional to the depth of the hole. The increase in height means more potential energy, which means the ball will fall with more energy, hitting the ground making a deeper hole. Therefore, the hole in the gelatin will be deeper the higher the point from which the ball is dropped.

List of variables:

         Independent variable: height of the ball, controlled by throwing the ball from different heights on a vertical ruler, such as 30cm, 35cm, 40cm, etc.

         Dependent variable: depth of the hole, using a ruler to measure the depth of the hole the marble leaves.

         Controlled variables: weight and volume of the ball, controlled by using the same marble every time.

List of materials:

Marble

Gelatin (250mL water + 7g Flosorb)

Ruler
Beaker
Scale

Method:

         1.- Let the ball fall into the gelatin from a certain height and measure the depth of the hole.

         2.- Repeat step 1 from several heights.

3.- Create a table with the results and study the relationship between the variables.

Colligative Properties

Vapor pressure is caused by some molecules turning from a liquid into a gas.

(dibujo)
 Pure Water  
(dibujo)                                
solution of pre water and salt (not volatile)
Because there are now salt molecules taking up the spare surface, less molecules can turn to gas. So vapor pressure is lower.

knowing this we can assure that when there is more solute added to the solution, the vapor pressure will decrease.
Francois-Maire Raolt discovered that:

Vapor pressure of solution = vapor pressure of solvent x molar fraction of the solvent
              (P)                                         (Po)                                      (Xo)
This is called Raolt's Law. It can only be used when we make a solution with a solute that is non-volatile (which means it will not turn to gas).

Problem:
At 35 ºC water has a vapor pressure of 3.2 kPa (finish)

Vapor Pressure and Intermolecular Forces

We are investigating vapor pressure to relate it to intermolecular forces. Vapor pressure is the pressure exerted by vapor in a thermodynamic equilibrium with its condensed phases (solid or liquid) at a given temperature in a closed system. The vapor pressure indicates a liquid's evaporation rate. it is realted to the tendency of particles to escape from the liquid (or solid). A substane that has a high vapor pressure at normal temperatures is referred to as volatile. Anne Marie Helmenstine, 2014)
Intermolecular forces are forces of attraction or repulsion which act between neighboring particles (atoms, molecules or ions).

Schlenk Tube: We put the substance in here and from the schlenk tube we can properly take out all the hair with the vaccum.

Water Bath: We use this to heat up the sucstance to the desired temperature.

Vaccum Line: We use this to take the air out of the schlenk tube.

Vapor Pressure Sensor: We plug this into a laptop and our schlenk tube to record the vapor pressure of our substance.

2-Propanol or Isopropyl alcohol:
chemical compound with the molecular formula  C₃H₈O or C₃H₇OH. It's a colorless, flamavle hemical compound with a strogn odor. it has a melting point of 355.8 K and a molecular mass of 60. 

Temp (ºC)	Pressure
0	0,63
15	1,46
25	2,72
35	3,66

Temp (ºC)

Pressure

0

0,63

15

1,46

25

2,72

35

3,66

Table of chemical compounds showing their boiling points, vapor pressure and intermolecular forces.

Name of compound	Molecular formula	Diagram of structure	Boiling point (oC)	Temperatures when vapour pressure measured (oC)	Vapour pressure (kPa)	Types of intermolecular forces
Pentane	C­5H10		36	0 15 25 35	44.87 47 49.86 54	Van der Waal
Ethyl acetate	C4H8O2		77,1	0 15 25 35	11.75 30.83 30.43 50.47	Van der Waal, permanent dipole dipole
Butyl acetate	C6H12O2		127	0 15 25 35	0,25 16,18 22,15 26,42	Van der Waal, permanent dipole dipole
1-Butanol	CH3(CH2)3		117,7	0 15 25 35	0.63 1.46 2.72 3.66	Van der Waal, permanent dipole dipole, hydrogen bonding
Propyl acetate	C5H10O2		101.6	0 15 25 35	9,1 20.66 20.89 21.54	Van der Waal, permanent dipole dipole
2-Propanol	C3H8O		82	0 15 25 35	78.99 96.15 100.85 11.29	Van der Waal, permanent dipole dipole, hydrogen bonding

Explaination:
The boling point of pentane is the lowest one because of the intermolecular force it has. The only intermolecular force that pentane has is Van der Waal, so we can assume that the boiling point of this compound will be at a very low temperature.
The compound witht the highest boling point is butyl acetate, which doesn't have hydrogen bonding, that is the strongest type of bonding. Because of this reason we have to think that the permanent dipole dipole forces of this compound are really high.
1-Butanol and 2-Propanol have all 3 types of forces but their boling point is lower than butyl acetate. so the three forces of this compound must be waker than the two of  butyl acetate.
References:
Anne Marie Helmenstine, P. 2014. Vapor Pressure Definition - Chemistry Glossary Definition of Vapor Pressure. [online] Available at: http://chemistry.about.com/od/chemistryglossary/a/vaporpressdef.htm [Accessed: 7 Mar 2014].

Conservation of Mass

Mass is always conserved. As Lavoisier’s law states, mass is neither created nor destroyed in chemical reactions (Nature.com, 2012). The data we obtained in the lab corroborates this. Some other examples would be:

(Amrita Olabs, 2011)

As shown by our data, unlike mass volume is not conserved. Especially in the case of gases, that don’t have a constant volume (Lohninger H., 2014).

Molarity is the relationship between the number of moles of solvent in a solution and the weight in Kg.

Molality is the relationship between the number of moles of solvent in a solution and the volume in L.

References

Amrita Olabs. 2011. The Law of Conservation of Mass in a Chemical Reaction (Theory) : Class 9 : Chemistry : Amrita Online Lab. [online] Available at: http://amrita.olabs.co.in/?sub=73&brch=2&sim=118&cnt=1 [Accessed: 13 Mar 2014].

Lohninger, H. 2014. Volume Relationships in Chemical Reactions. [online] Available at: http://www.vias.org/genchem/atommasses_12431_03.html [Accessed: 13 Mar 2014].

Nature.com. 2012. The Conservation of Mass | Learn Science at Scitable. [online] Available at: http://www.nature.com/scitable/knowledge/library/the-conservation-of-mass-17395478 [Accessed: 13 Mar 2014].

The properties of materials

Why do ionic compounds dissolve in water?

Because the oxygen in water molecules is electronegative, so when ionic compounds are mixed in it, the molecules are easily pulled apart as they're both charged.

Why do covalent compounds dissolve in acetone (a covalent compound)?

Because acetone is non-polar, as well covalent compounds. Non-polar substances dissolve other non polar substances.

Why do metals conduct electricity?

The metallic bond allows electrons to move freely between the atoms, this allows electricity to be transferred.

Why do covalent compounds NOT conduct electricity?

In order for electricity to be transferred, there must be a charged part that can move freely in the compound. There's no charge in covalent compounds.

Why do ionic compounds have such a high boiling points?

Ionic bonds are very strong and a lot of energy is required to break them.

Why do metals have such high boiling points?

Metallic bonds are quite strong, in order to break them a lot of energy is needed.

Relationship between volume and pressure

Boyle-Marriote Law: 

Gas Equation: Pi·Vi = Pf·Vf

Initial Pressure(Pi) = Pf·Vf / Vi

Initial Volume(Vi) = Pf·Vf / Pi

Final Pressure(Pf) = Pi·Vi / Vf

Final Volume(Vf) = Pi·Vi / Pf

Conclusion: The lower the volume the higher the pressure. This is because when the same amount of particles are together in a big place there is plenty of space between them, but when they are all together in a smaller place the particles have a smaller space between them. When this happens the pressure is higher.

Hello physics fanatics, this here is our first How-To video. This will show you how to prepare a Schlenk Flask for the lab. Hope you like it.
Enjoy! :D

Schlenk flask How-To