Essay on Vapor Pressure and Enthalpy of Vaporization of Water

Pick up each test tube, tap the bottom/ swirl the contents and then using your ruler record in Table 1 the bubble height (if any) that is produced. Remember to include this table (with a strong title) in your lab report.

1. Fill the graduated cylinder nearly to the top with water, with a tall glass tube open at both ends (the water level with act as the closed end).

C) Again, rinse the saucepan and then add 250 grams of sugar to your 250ml graduated cylinder and then add water up to the 250ml mark. You will place a small piece of plastic wrap over the top of the graduated cylinder (or parafilm if you have that), and mix the sugar with the water. Then pour the contents into a small saucepan over the stove. You will fill the graduated cylinder up to the 250ml mark again and then pour the tap water into the saucepan as well. You will now heat the mixture on the stove and stir until the sugar has dissolved. Once this has happened, you will remove the solution from the saucepan, pour the solution into a container and label that container 50% sugar solution.

I took the graduated cylinder and started filling it up with water until the bottom of the meniscus was to the the 100.0 mL mark with the assistance of a dropper pipet. I then took the 13 x 100 mm test tube and slowly poured the water from the graduated cylinder into the test tube until it was full to the top. I then poured the water in the test tube out into the sink and put the graduated cylinder on the counter so I can get an accurate measurement of the lower meniscus to record on my data table. I once again followed the same procedure again filling a second test tube with water from the graduated cylinder then setting it on a straight surface to get an accurate measure of the volume to

1. Carefully measure the volume of the trapped gas using the graduations (markings) on the side of the container.

A. Water boils at 100°C at sea level. If the water in this experiment did not boil at 100°C, what could be the reason?

The control experiment for this investigation will be the experimental setup of 5 trials using 5oC as the temperature. All the steps in the method will be followed.

28) A basketball is inflated to a pressure of 1.90 atm in a 24.0°C garage. What is the pressure of the basketball outside where the temperature is -1.00°C? A) 2.08 atm B) 1.80 atm C) 1.74 atm D) 2.00 atm 29) The density of a gas is 1.43 g/L at STP. What is the gas? A) Cl2 B) O2 C) S 30) Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) In an experiment, 201 mL of wet H2 is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is __________ atm. A) 1.00 B) 706 C) 0.929 D) 0.964 E)

Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring

1) Separate the solid from the liquid in the beaker by decanting the liquid. Ask your instructor to demonstrate the correct procedure.

The second step involves taking the measuring cup and pouring two cups of water into both glasses. When you have finished filling the glasses take a marker and mark where the water line falls on both glasses. Before you put the glasses in their respective places you should cover both of with the foil. Making sure the foil is wrapped tightly around both of the glasses place one in the freezer and the other one on a counter, so that it is room temperature. Leave both glasses in their set places for twenty-four hours. When the twenty-four period is over using a ruler compare the initial line we drew to the line of the water now too see if the water height has increased, decreased, or stayed the

In this experiment, The purpose of this experiment is to investigate the measurement of the actual volume contents of volumetric glassware. In the beginning of the experiment, the volumetric glassware should be clean and dry before used. The volumetric glassware, measuring cylinder and pipette should be handled with care and all the precautions were be taken during the experiment was held. This was to ensure to avoid any errors such as parallax error especially while reading water meniscus. This experiment must be repeated three times or more and take the average reading to get more

The Joule-Thomson apparatus (Leybold Didactic, Huerth, Germany) consisted of a glass cylinder with five outlets and a glass filter subdivision. One side of the division was connected to the helium or carbon dioxide gas pressure cylinder that was supplied in the laboratory, a pressure sensor, and a NiCr-Ni thermocouple, which measures the temperature inside that chamber. The other chamber contained outlets for another thermocouple and for the transferred gas. A temperature controlled water bath was used to set the system to the

To achieve this, the final value from each thermocouple was set to be equal to the warm water bath temperature (370C), and the initial reading was set equal to the ice water bath temperature. Thus, for each thermocouple an equation was obtained using the two points to convert voltage readings to temperature. An example of the calibration for one of the thermocouples is shown in Appendix II.

Vapor pressure thermometers are founded on the saturated vapor pressure in a two-phase system. The behavior of a liquid-vapor system in equilibrium is described in the tC curve. Beside the curve for a pure substance, the pressure differs on the temperature and not on the quantity of substance vaporized. The temperature range related with vaporization is limited to temperatures between the critical point and the triple point of the substance. The range is even further reduced if the extreme pressures to