The Determination Of Molar Mass Of Volatile Liquids And Calorimetry Lab Report

What about converting a given volume of gas to mass or a given mass to volume? Once again you have to get to that common ground first, which is the mole.

Copied the observations table in our notebook. Then recorded the mass of the beaker using the balance and wrote down the measured mass in the observation

If the NaOH managed to absorb water before measured, then the measured mass of the NaOH

3. The volume of a fixed mass of a liquid sample increases as the temperature rises from 20 to

In the third stage of this experiment, the density of a liquid was determined and compared to known standards. A 100ml beaker was filled to about half-full with room-temperature distilled water. The temperature of the water in ◦C was recorded in order to compare to known standards later. A 50ml beaker was then weighed on a scale in order to determine mass and recorded. A sample of the distilled water with an exact volume of 10ml was then placed in the 50ml beaker using a volumetric pipette. The 50ml beaker with the 10ml of water was then weighed again and the initial mass of the beaker was subtracted from this mass to obtain the mass of the 10ml of water. With the volume and the mass of the water now known, density was calculated using d = m/V and recorded in g/ml. This process was then repeated to check for precision and compared to standard values to check for accuracy. Standard values were obtained from CRC Handbook, 88th Ed.

In this lab, the molar mass of a volatile liquid is determined based on its physical properties in the vapor state. In order to calculate the molar mass, the mass, temperature, pressure, and volume is measured independently and then converted to the correct units. Sample C was obtained at the beginning of the experiment, which was later informed to be ethanol. Based on the calculations made, the molar mass of the volatile liquid was 95.9 g/mol. However, compared to the known value of 46.1 g of ethanol, the value measured had a 108% error. Unfortunately, this was a very big percent error and may have been caused by incorrectly measuring the volume of the gas. Using the ideal gas law, the molar mass of a volatile compound was calculated in order

The table above displayed the data we figured out concerning the mass of each substance. First, we weighed the cup alone that contained the unknown substance. It weighed 3.5 g. Then, weighed the cup with the unknown substance. It weighed 32.5 g. The final mass was determined by subtracting the cup mass (3.5 g) from the cup mass with the unknown substance (32.5 g). I figured out the final mass was 29 g. Next, we weighed the cup alone that contained the aluminum. It weighed 3.5 g. Then, weighed the cup with the aluminum. It weighed 17 g. The final mass was determined by subtracting the cup mass (3.5 g) from the cup mass with the aluminum (17 g). I figured out the final mass was 13.5 g. After that, we weighed the cup alone that contained zinc. It weighed 3.5 g. Then, weighed the cup with the zinc. It weighed 19.7 g. The final mass was determined by subtracting the cup mass (3.5 g) from the cup mass with the zinc (19.7 g). I figured out the final

15. Determine the mass of the water by using the water’s density (specific to the initial temperature) and the volume of the water. Remember, density = mass/volume. You can look up the density of the water at your specific temperature at

Obtain the mass of two dry and empty 125mL or 250mL Erlenmeyer flasks on a milligram balance and then number it. Record the mass in your data table.

Determine the weight of the water by subtracting the weight of the vial with water by the weight of the vial on its own.

The purpose of this experiment is to identify an unknown substance by measuring the density and boiling point. I will be able to conclude which substance is my own from a list of known options stating what its real boiling point and density is.

The hydrochloric acid is put into a calorimeter and then the zinc is added after. The lid is closed after the zinc is added and a thermometer is inserted through the lid in order to check the temperature as the reaction takes place . The temperature is measured until the reaction has completed and the highest temperature is used as the final temperature. ∆T is then found by the equation ∆T=Tfinal-Tinitial. Then according using the equation ∆H=mc ∆T+PV. In this lab the pressure remains constant while the volume is changing. In order to calculate the volume the same reaction with the same amount of zinc and hydrochloric acid is used. However, instead of a calorimeter, an erhlenmeyer flask with a balloon put over the top is used. The hydrochloric acid is placed into a flask, the zinc is placed inside the balloon and then sealed over the flask. By dropping the zinc into the flask the reaction occurs. This allows the H₂ gas to be captured in the balloon. The circumference of the balloon is then found. The circumference can then be applied to the equation C=2πr and the radius is determined. Using the radius of the balloon, in the equation V=(4/3)πr³ the volume taken up by the hydrogen gas can be found. The pressure is the pressure of the air which is measured with a barometer. ∆H can be found by multiplying the mass of hydrochloric acid, the specific heat of HCl, and ∆T of the hydrochloric

2. Calculate the mass of the reaction mixture in each reaction first by determining the volume of the solution and then assuming that the density of the solution is the same as pure water (1.0g/ml). Show work here and record your answer in Data Table 2.

For Table 1 the difference between the reactants and the product was zero grams. One possible explanation as to why the mass stayed the same, was that there was a rubber stopper covering the top of the Erlenmeyer flask. This resulted in the mass to staying the same because it stopped the gas that was formed from

4. Determine the mass of the mixture by subtracting the mass of the empty evaporating dish from the mass of the evaporating dish containing the mixture and record the calculated mass onto the data sheet.