Measurement/Density Lab Purpose: The purpose of this lab was to practice measurements, obtain calculations with significant figures, and calculate density of different substances with various methods. Procedure: Part A: Densities of Rectangular Solids/Cubes 1) Obtain a rectangular solid/cube and measure the three dimensions. 2) Determine volume and mass, recording mass to the nearest .01g. 3) Determine the density and percent error. Part B: Density of a Cylindrical Solid 1) Obtain a cylindrical solid and measure its mass.
AP Physics C Lab Report i. Purpose: To use derivatives to investigate the various characteristics of cardboard ii. Materials: Compass, Cardboard, mass balance, ruler, meter stick iii. Procedure: 1. Measure and record the diameter of each of the disks in meters.
The following mistakes were made when carrying out the experiment. What effect does each have on the calculated molar mass? Be specific. For example, too large because… Only part of the pipet was immersed in the boiling water, so the temperature in part of the pipet was less than that of the water bath. If the temperature was less than the water bath in some places because only part of the pipet was immersed in the boiling water, the molar mass calculated would become lower.
Calculate the percent by mass of NaClO in the commercial bleach. (Start with molarity of concentrated NaClO found in part 4. Determine the molarity per mL instead of liter. Next, divide by the density (you’ll have a label of mole/g at this point). Then multiply this by the molar mass of NaClO which has a label of g/mol so all labels cancel.
They were basic. Conclusion: It was experimentally determined that elements in the same families react similarly, after observing the reaction of calcium, and later, potassium. These experiments could have been affected by error such as contamination of chemicals, improper amounts of chemicals, lack of reactions, as well as
Use the report pages below to record your data. Answer questions A-G found on pages 46 and 47. Name: _________________________ Lab 2 Report Data: Data Table 1: Length Measurements | Object | Length (cm) | Length (mm) | Length (m) | CD or DVD | 12.1 cm | 121 mm | .121 m | Key | 5.1 cm | 51 mm | .051 m | Spoon | 16.1 cm | 161 mm | .161 m | Fork | 18.5 cm | 185 mm | .185 m | NOTE: The instructions indicate to measure the objects to “one degree of uncertainty.” The degree of uncertainty is a property of the instrument used. All three recorded values will have the same precision. On page 29 is the explanation of uncertainty.
Pre Lab Objective: The purpose of this lab is to obtain the mass and volume of two different metal samples, to graph data, to obtain the slope of graphed data and to display a best fit curve of experimental data in order to graphically determine the density of each metal Background: Understanding the relationship that exists between a substance’s mass and its volume. This relationship is expressed by the physical property called density. (D = M/V). In order to determine the volume of solids, a technique called water displacement is used. A fixed amount of water is added to a graduated cylinder and the volume of water is recorded.
Possible experimental errors include not properly removing all the iron/salt/benzoic acid from sand. Residue in beaker and cups not completely removed for accurate mass weight. Another error could have been not properly drying the benzoic acid filter paper or sand mixture before weighing. Questions: A. How did your proposed procedures or flow charts at the beginning of this experiment compare to the actual procedures of this lab exercise?
There was a low efficiency rate for this experiment; energy was most likely wasted into the surrounding environment when the burner was alight. Possible ways to improve this experiment would be to possibly do the experiment in a more enclosed space, so as to disallow any heat escaping into the surrounding atmosphere. A fume cupboard would be suitable (when it is not turned on) as there is less movement in the air to move the energy from its intended target. The thermal energy was not only going into the water, but the can of the calorimeter became hot too, meaning that the thermal energy was transferred into the metal surrounding the water, and not just the
Also, there is a limit of how much solute you can put in the solvent and you should not exceed that certain percentage. If you put too much solute and end up having more solute than the water, the freezing point will start going back up again because the solute won’t be able to dissolve within the solvent at such a big quantity. Another limitation is that the concentration of the solvent in the mixture should be at least 10% and if it’s lower, the freezing point depression might not be affected because the amount of solute used will be too low. Lastly, the solution must be cooled to a lower temperature than the pure solvent in order to freeze. If water was used as the solvent, it has a freezing point of 0 °C and the solution will freeze at even a lower temperature so you have to put it somewhere cool like a freezer.