Prepare a chart for recording any observations as you test for the presence of cations in the solution. Set up and label 10 test tubes #1- #10 and place them in order in a test-tube rack. Wash and rinse all of glassware with distilled water. Prepare a hot-water bath in a 250 mL beaker by filling it up to 150 ml and bringing it to a boil. Obtain 2 ml of the solution you want to test and pour it into test tube 1.…
Moles 1.How is molar mass calculated and why is it useful? Molar mass is calculated by going to the periodic table finding each mass of each element in the compound then adding them all up based on how many of those elements are in the compound. 2.Define a mole in chemistry and give 3 examples equivalent units that are used in chemical calculations. Mole is considered the unit for amount in chemistry other units that are equivalent are atoms, formula units, and molecules.…
Procedure: This lab was performed based on the procedure outlined in “Exp #7 Calorimetry.” No changes to the procedure were made. Data and Observations:…
Determining the Percentage Yield of a Chemical Reaction Question: What is the percentage yield of the reaction of sodium carbonate and calcium chloride dihydrate (the dihydrate must be included with the molar mass calculation)? Predictions: Predict the mass of sodium carbonate and calcium chloride dihydrate that will be required to produce 1.90 grams of calcium carbonate: Therefore, the predicted mass of sodium carbonate is 2.0 grams and the predicted mass of calcium chloride dihydrate is 2.8 grams. Materials: 2 Beakers (150 mL) Calcium chloride Sodium carbonate…
To start this laboratory experiment, we first collected all the materials necessary including multiple beakers, samples of each solution, metal strips, a salt bridge, alligator clips, and an abrasive sponge. Then 10 mL of CuSO4(aq) and 10 mL of ZnSO4(aq) were placed into separate 250 mL beakers. A copper strip was then placed in the beaker containing CuSO4(aq) and a zinc strip was placed into the beaker with ZnSO4(aq). The two beakers were connected by a salt bridge that consisted of a string soaked in 0.5 M KI solution and each end was placed into each solution.…
In this method, a solute is dissolved in a solvent at boiling point to increase solubility. The new solution is then cooled to get pure crystals of the solute. Using this technique of an unknown helps one get a pure substance which could be tested for melting point. In Figure A, the red arrows show the series of test the first unknown 64A, was put through to determine what type of substance it was.…
Lab Report #1 Physics 261-001 Author: L. Cason Lab Partners: A. Longo, K. Harrell Date: 3/16/16 Objective: For this lab, the objectives were to learn how to use lab equipment such as the Lab Pro interface and the Logger Pro software and analyze the data collected using Excel. In order to achieve this Newton’s Law of Heating and Cooling was compared to the data collected by a thermometer attached to the Lab Pro. Theory:…
Thermodynamics of Cheetos Purpose: to analyze the caloric content of snack foods, by determining the calories of heat given off by a Cheeto, or other snack foods, as it burns. Procedure: The food sample (Cheeto) was placed on a food holder, and the initial combined mass of the food holder and the Cheeto was measured and recorded. Using a graduated cylinder, 50-100 milliliters (ml) of water was measured and added to an empty soda can that was cut in half and cleaned.…
What do your results tell you? Are there any relationships, patterns or trends in your results? From our [processed] results, we can conclude that the polystyrene cup served as the least effective conductor of heat, the tin mug coming in at a close second. The most effective material for heat conduction was the plastic mug.…
Jessica Vandeventer April 13, 2016 Energy Comparison of Fuels Purpose/Question- The Purpose of the lab is to see a comparison of fuels using a home made calorimeter. Hypothesis– The burner fuel is going to be a better source of fuel than the tea candle. Data Tables/ Graphs – Data Table 1.…
Based on the results of the control experiments, the interaction between the Calcium Chloride and phenol red are responsible for the high temperature change in the overall reaction. After doing a control experiment with Sodium Bicarbonate and phenol red and noticing that the temperature got colder, only one other chemical mixed with phenol red could be responsible for the warm temperature change that chemical being Calcium Chloride. There was a temperature change that was observed during the individual control labs as seen when calcium chloride was mixed with water it became hotter and when calcium chloride was mixed with the phenol red it also grew hotter in temperature. Though during the lab which mixed phenol red with baking soda the temperature…
The most common is a Styrofoam cup. And a more complicated one is called a bomb calorimeter which has the substance in the middle surrounded by water, and the substance is ignited and the change in temperature of the water is measured. (Cal …) The measurements as well as the mass and the specific heat, “which is the amount of heat required to raise an objects temperature by one degree Celsius” (Chem …), are used in the calorimetery equation. Which is specific heat multiplied by the mass in grams multiplied by the change in temperature.…
The purpose of this lab was to determine if a change in mass occurs during a chemical reaction in a closed system. To conduct this experiment, the mass of the test tube, rubber cover, and other materials must be measured. To prevent the test tube from rolling off of the balance, a plastic cup was used to hold it in place, but the group had to remember to zero out the cup on the balance so the cup’s mass will not affect the masses of the objects the group was trying to measure. During this investigation, it was determined that there is a 0% change in mass after a chemical change in a closed system, because the mass of the copper and sulfur before heating did not change after being heated. Although the substances had changed in appearance and could no longer be considered…
Afterwards, the flask was filled with distilled water to the mark, so that the bottom of the meniscus is aligned with the ring in the neck of the flask. The filled flask was then weighted and the measure was recorded. Then, the distilled water was poured from the flask into a 50 ml beaker and its temperature was recorded. Once that was done, the flask was cleaned with an unknown solution provided by the instructor and then the flask was filled with the same unknown solution up to the mark. The flask was weighted and its mass recorded.…
Cool water was placed into the calorimeter and its temperature recorded, while an equal weight of water was heated to 35.3 ⁰C. The heated water was immediately poured into the water in the calorimeter and the temperature was recorded. The water equivalent of the calorimeter could then be calculated. Approximately 100 g of cool distilled water was placed into the calorimeter and the initial temperature recorded. Solid sodium sulphate decahydrate crystals of 4.00 g were added to the water in the calorimeter and stirred until it dissolved.…