Eudiometer Experiments in Elemental Effervescent Expansions Joe Williamson and Ethan Kang Mar 13, 2023 Purpose: The purpose of the gas laws lab was to calculate the volume of gas produced from a specific mass of magnesium ribbon. It also aims to use gas laws to determine the theoretical yield and volume of hydrogen gas produced at STP. Procedure: Gather Mg ribbon, string, a 2000-mL beaker, a Eudiometer, a 100-mL beaker, 50-60 mL distilled water, and HCl. Measure out 0.035 - 0.045g of magnesium ribbon and tie a string to it and record the mass of the ribbon. Pour 6 mL of HCl into the eudiometer. Carefully pour 50-60 mL of distilled water to fill up the rest of the eudiometer. Fold the Mg ribbon and place about ¼ up the eudiometer. Fill …show more content…
When you collect the gas through the eudiometer, the water inside the eudiometer gets displaced, evaporating until the pressure of the water outside is equal to the pressure inside. To correctly find the pressure of the gas, the pressure of the water vapor must be subtracted, as the two are mixed together. What is the limiting reactant for the reaction? What is the experimental evidence that you are basing it on? Based on the experimental evidence (mostly based on observations), the limiting reactant appeared to be the magnesium strip. As the eudiometer, the magnesium strip began to dissolve, resulting in the formation of Hydrogen gas bubbles. As time went on, the magnesium strip began to quickly break down, forming Hydrogen bubbles, until the magnesium strip fully dissolved. Once the magnesium strip had broken down, the bubbles began to stop forming. Balanced …show more content…
After flipping it upside-down and placing it into the water, it floated outside of the tube and about half of it came into contact with the outside water. As a result, a bit of the hydrogen gas that formed from the magnesium strip did not make it up the eudiometer; instead, it permeated through the beaker. This logically resulted in a lower value of hydrogen gas volume than if all of the gas made it into the eudiometer. The lower volume of hydrogen gas produced could have skewed our results. In order to prevent this in the future, we suggest securing the magnesium further up the
With following the procedure, the experiment was completed very easily. The technique used worked very well. The graduated cylinder were dried after each trial to ensure each water level was equal. The air bubble were risen to the top to ensure the equal amount was measured. Systematic errors can not be eliminated by averaging In principle, they can always be eliminated by changing the way in which the experiment was done.
The eudiometer was placed in a water bath and the magnesium ribbon and hydrochloric acid reacted to form hydrogen gas. The rubber stopper was removed in order to balance the water levels in the eudiometer and the bath. The process was repeated. Chemical theories and concepts used in this experiment includes
CH 204 – Introduction to Chemical Practice Experiment #2 – Gas Laws Jose De Arrigunaga* Robert Gonzalez TA: Ryan Ciufo September 29, 2015 EXPERIMENTAL The power adapter was plugged into the left side of the LabQuest, and the pronged end was plugged into a power outlet. The LabQuest was turned on using the power button on the front of the device near the top left corner.
Equipment: • Different coloured pens/textas • Filter paper • Scissors • 250ml beaker • Pencil or pop stick • Tape • Water Methylated spirits Ruler • Measuring cylinder Method 1. Cut a 10cm length of filter paper 2.
Looking at this value, and comparing the experimentally determined values, the values do not exactly match up, but are close together, as the values are only 0.4 - 0.6 g/mL away from the value of 1 g/mL. One reason why the values may not match up is because of the amount of liquid used. Sometimes, the value of water poured into the graduated cylinder may not be equal to specific volume which was to be used. In order to improve that, making the water volume more precise may allow for more accurate results. Secondly, the type of water used may of affected the value. If we take a look at pure water, the value of it at room temperature is 0.99823 g/mL. If we use this water (by boiling it before hand), and confirming the density is equal to the accepted value, than it will increase the chance of being more accurate.
The experimental density was then compared to the actual value and a percent error was determined. Materials: Equipment and materials used in this experiment were: unknown metal samples (2) 100 mL graduated cylinder electronic balance tap water wire screening weigh dish (Dixie cup) Methods: The mass of five different amounts of an unknown metal sample was determined using an electronic
After the first substance was separated we focused on the other one by getting two beakers of equal mass and filling one up with 50mL of water and taking the mass of the other with the watch glass over it. Once completed we poured the remaining mixture into the beaker and stirred it. We then got another piece of filtration paper and recorded its mass. After that we constructed a filtration setup by placing a pre-massed paper into a funnel supported by a ring stand over a pre massed beaker. Once the setup was complete we poured the water mixed with the mixture into the funnel. Once all the water went through the funnel we took out the filtration paper and set it to dry.
The purpose of this lab experiment is to determine the molar mass of a volatile gas by using the ideal gas law. Procedure: First a 600 mL beaker was filled half way with water and assembled into a boiling water bath. Then 2 stoppers were obtained, one had a hole at the top so that vapor could easily flow out.
Next, is the verification and determination of pure liquids. A clean and dry a 25mL graduated cylinder must be gathered from the lab cart, weigh the dry cylinder to the nearest mg and record the data. Add distilled water to the cylinder making sure the water level is at above the 20mL mark but below the 25mL mark. Determine and record the temperature of the water in the cylinder. Then, reweigh the cylinder to the nearest milligram.
Based on the obtained results from the experiment, the unknown liquid was determined to be methanol. The results were very close to the theoretical values, all within 15.92 % error. In this experiment it showed that the methanol have different intermolecular forces at work and at different vapor pressures implying that the amount of intermolecular forces they exhibit affects the vapor pressure. Possible source of error that occurred throughout the experiment was that the temperature was hard to control leading to the variances between the temperature of the reading in the water bath and the actual temperature causing slight changes in the vapor
It will ultimately measure the absorption of calcium and magnesium for the sample. Next is the usage of the conductivity meter; after filling a well with the sample, place the probe into the well. This will read a total dissolved solid value for the
Then we cut the Sodium metal into small pieces 3. Then we added the cut pieces to water in the beaker and noted the change observed. 4.
Experiment 9: The Molar Volume of a Gas Introduction Description: The purpose of this experiment was to determine the molar volume of a gas by conducting the hydrogen gas producing chemical reaction: Mg(s)+2HCl (aq)→〖MgCl〗_2 (aq)+H_2 (g) A known mass of solid magnesium was reacted with an excess of hydrochloric acid in a sealed vessel, three times, for a total of three trials.
Zero the scale. Pour one of the 4 substances into the plastic container “h”. Record mass of first substance.
• Examine the differences in percentage concentration for each fruit piece. • Wipe the extract water and then measure your pieces. • You will be examining the percentage by weighting the fruit pieces before and after you insert them in the beaker and they have been in there for a day. Table 1: Initial weight of each piece of fruit.