Report

Basic Chemical Praktium Report 1


EVENTS IV
DETERMINATION OF GAS AND OXYGEN MOLAR VOLUME

A. IMPLEMENTATION OF PRKATIKUM
1. Practical Objectives: To learn how to determine gas constant and oxygen molar volume as well as to study gas laws such as boyle, charles, gay lusac, dalton's laws, about partial pressure and Avogadro's law.
2. Practicum Time: Monday, 8 Mei 2017
3. Place Practicum: Basic Chemistry Laboratory I, Faculty of Mathematics
  And Natural Sciences Jambi University.

B. THEORY OF THEORY
The physical properties of the substance affect by its form, ie solid, liquid or gas. Among these three forms, gas properties are simpler than others. There are four important variables that affect the physical properties of the gas ie temperature, pressure, volume and amount of gas. Gas has the following characteristics: its shape and volume follow the container, can be utilized, the lowest speed, and can be mixed perfectly in one container (Purwoko, 2006: 136
The gas consists of molecules that move according to straight roads in all directions, at very high speeds. These gas molecules always collide with other molecules or with vessel walls. Plants against walls. This is the cause of the pressure. The volume of the gas molecule is very small when compared to the volume occupied by the gas, so there is actually a lot of empty space between the molecules. This causes the gas to have a smaller density than liquid or solid, thereby causing the gas to be compressible or easily suppressed, in gas talk, all gases are divided into two types:

A. The ideal gas is gas that follows perfectly.
Gas laws (Boyle, gay lussac, etc.)
B. Non ideal gas is a gas that only follows the laws of gas at low pressure.
The ideal gas does not actually exist, so it is just a gas hypothesis. All gas is not real. In the ideal gas is considered, that the molecule is not attractive and the volume of the molecule can be ignored against the volume of the gas itself or occupied space. This ideal is only approached by the one-mat gas at low pressure and at relatively high temperatures. When used the STP price (1 atm 00C or 273 k) and we take 1 mole of gas, the gas volume can be measured which we call molar volume in STP, since it is the voluem of 1 mole of gas at the pressure of 1 atm and o0C. If we do this for different gas looks different because the real gas is not "ideal gas". Of the various measurements of the average volume occupied by one mole of gas at STP = 24 L. then this price is taken for the molar volume of the ideal gas using those prices, can be calculated by R.

The R constant may vary depending on the unit used in expressing pressure and volume (Brady, 1999: 483).
The laws relating to gas include:
1. Boyle's Law
Boyle said that if the temperature is kept constant then the volume (v) of the gas sample decreases with increasing external pressure, ie atmospheric pressure plus pressure from the addition of mercury. Boyle's Law Statement The volume of gas at a fixed temperature is inversely proportional to the pressure. The pressure and volume of a gas at a fixed temperature is constant.
2. Charles and Gay Lussac's Law
Jeagues Charless and Gay Lussac observe that pressure remains a task that will expand when heated and otherwise shrink when cooled. Charless and Gay Lussac's law reads "the volume of a gas at a pressure remains proportional to its absolute temperature".
3. Avogadro's Law
Based on the results of Boyle's investigation, Charless and Gay Lussac Amedeo Avogadro proposed the hypothesis that "at the same temperature and pressure, all gases contain the same number of molecules (atoms)." Common gas equations: four complete (quantity) quantities of gas: M, V, T and P. The number of available can also be expressed in the number of moles (n) in place of their mass. The volume of a gas is directly proportional to the number of moles present. The number of moles of n at an absolute temperature is inversely proportional to P. The combination in a statement of Boyle, Charless, Gay Lussac and Avogadro's laws is called the ideal gas law, mathematically (Pudjaatmaka 1998: 263):
P.V = n.R.T
 Gas mix: eg a mixture occupies a container at a certain temperature. We can define the partial pressure of a gas as if the pressure of the gas is self-generated if it is in the container. Dalton's law probably states that total pressure is the sum of the partial pressures of each gas. This law applies under the same conditions as the ideal gas law itself with a moderate pressure approach, but be careful if the pressure is lowered (Oxtoby, 2001: 106).
The reaction coefficient represents the mol ratio of the substances present in the reaction. In the case of a gas reaction, the reaction coefficient also states the ratio of gas volume involved in the initial reaction to the same P, T (according to Gay-Lussac Law). The relationship between standard gas volume and the number of moles. The relationship of the molar volume of the gas shows the volume of 1 mole of gas at the standard state (Wahyuni, 2003: 23).

C. PROCEDURES AND MATERIALS
1. Practicum Tools
A. Bunsen
B. Jack
C. 250 ml erlenmeyer glass
D. 250 ml measuring cup
E. Watch glass
F. Clamp
G. 500 ml round bottom flask
H. Pipe
I. Hose
J. Spatula
K. Statif
L. Test tube
M. thermometer
N. Analytical Scales

2. Practicum Materials
A. Aquades
B. KClO3 (s) (Potassium chlorate)
C. MnO2 (s) (Manganese Oxide)

D. PROCEDURES OF EXPERIMENT
1. Weighed one clean and dry reaction tube.
2. Inserted 1.2 gr of KClO3 / MnO2 into the test tube, then weigh it more thoroughly.
3. Fill the flask with water and put a little water into the erlenmeyer flask.
4. Contains water into a measuring flask with measuring glass and erlenmeyer by blowing from the end of the pipe connected to the test tube.
5. Issued air bubbles contained between the measuring flask and erlenmeyer by raising or lowering the measuring flask or erlenmeyer.
6. Clipped the test tube with a clamp that will connect the measuring flask and the erlenmeyer flask.
7. Installed test tube.
8. The opening is opened and the erlenmeyer rises to the surface of the water in the measuring flask and the erlenmeyer is the same height. Pinch more with a clamp.
9. Moved erlenmeyer with hati2 so that water does not drip.
10. Cleaned erlenmeyer and placed carefully pipe in the erlenmeyer vessel.
11. Heat the test tube carefully so that oxygen flows into the measuring flask. Heated kikra - about 5 minutes so all KClO3 decomposes.
12. If oxygen is not decomposed again, move the burner and leave it until all the equipment reaches room temperature.
13. If it is cool, the hose is clamped and removed erlenmeyer.
14. Measured gas temperature in measuring flask with thermometer with care and thermometer not to be exposed to water.
15. Measured water volume in erlenmeyer with measuring cup.
16. Recorded thermometer position and KClO3 / MnO2 already heated, recalculated and recorded.

E. OUTCOME RESULTS
NO

PROCEDURES OF EXPERIMENT

OBSERVATION RESULT
1.The empty reaction tube is weighed by the analytical balance
Weight test tube
= 7.87 grams
2.KClO3 and MnO3 are weighed
Tube + KClO3 + MnO2
= 9.06 grams
3.Incorporated water into a circular round flask and erlenmeyer glass
4.Installed sets of molar volume determinations, connected hoses with round bottom flask, hose with Erlenmeyer glasses dipemangkn klem, blown until no bubbles.
5.Connected the hose with a test tube in which MnO3 and KClO3.
5.Heated with Bunsen for 5 minutes
7.Clamps open, allow water to flow until it stops flowing
T = 32
8.Measured water volume in measuring flask with measuring cup
Water volume = 55 ml
9.The reaction tube is weighed again
KclO3 + MNO3 (after heating) = 8.83 grams