INDIVIDUAL ACCOMPLISHED REPORT Name \( \qquad \) Course \( \qquad \) lustructor \( \qquad \) \( \qquad \) Nate Peffarme \( \qquad \) Date Subruitted \( \qquad \) Experiment No. 1 MEASUREMENTS I. Data and Results a Measurements of Temperature Temperature 1. Tee water \( \qquad \) \( \circ \) 1.a before stiring \( \qquad \) \( { }^{\circ} \mathrm{C} \) 1.b atter stiming 2. fce "?ate ?ith satt ?dded \( \qquad \) \( { }^{\circ} \mathrm{C} \) b. Measurements of Voiume Volume \( \qquad \) \( \mathrm{ml} \) \( \qquad \) \( \mathrm{ml} \) \( \qquad \) \( m l \) \( \qquad \) \( \mathrm{ml} \) 1. test tuke 2. \( 125 \mathrm{ml} \) Erlecumeyer flask with CusO, 3. Height of \( 5.0 \mathrm{ml} \) Water in the test tube 4. Height of \( 10 \mathrm{ml} \) water in the test tube \( \qquad \) c. Measurement of Density C. Solid Sample \begin{tabular}{|l|l|l|l|l|l|} \hline Thal & Mass & Volume & Yolume ( \( \mathrm{H}_{2} \mathrm{O} \) displacement) & Densilyl & Density( \( \mathrm{H}_{2} \mathrm{O} \) displacement) \\ \hline 1 & & & & & \\ \hline 2 & & & & & \\ \hline Alc & & & & & \\ \hline \end{tabular} 11
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In this experiment you will measure the density of a liquid and a solid object. Be sure to record all of your measurements with the correct degree of precision and perform your calculations properly, according to the rules of arithmetic for measured values. A. Measurement of the density of water. 1. Weigh a small beaker (degree of precision?). Place about 25 mL of water in a 50 mL graduated cylinder and record its volume (degree of precision?). Pour the water into the beaker and weigh the beaker and water together. From these data, calculate the density of the water, giving your answer with the proper number of significant figures. Volume of water in cylinder 26.7 mL Mass of empty beaker 78.013 g Mass of beaker with water 104.735 g Mass of water in beaker ____ g Density of water ______g/mL Show calculations: 2. After pouring out the water from your beaker, add a second 25 mL of water to the graduated cylinder. As before, record the volume of water in your graduated cylinder. Pour the water into the beaker and weigh the beaker after adding the water. From these data, calculate the density of the water a second time. You need not dry the beaker before performing this second experiment. Why? Volume of water in cylinder 24.2 mL Mass of empty beaker 78.013 g Mass of beaker with water 102.181 g Mass of water in beaker ____g Density of water _____g/mL Show calculations: What do you notice about the two values of density obtained in these two experiments? How close are your two values? If there is variation, in what decimal place to you see the variation? Why should you expect variation in the last decimal place of your recorded values? 3. Calculate the average density you determined for this unknown liquid and record below. [ ___g/mL + ____g/mL] / 2 = _____g/mL
Danielle A.
Finding the volume of a flask. A student obtained a clean dry glass-stoppered flask. She weighed the flask and stopper on an analytical balance and found the total mass to be 31.601 g. She then filled the flask with water and obtained a mass for the full stoppered flask of 60.735 g. From these data, and the fact that at the temperature of the laboratory the density of water was 0.9973 g/cm $^{3}$, find the volume of the stoppered flask. a. First we need to obtain the mass of the water in the flask. This is found by recognizing that the mass of a sample is equal to the sum of the masses of its parts. For the filled stoppered flask: Mass of filled stoppered flask = mass of empty stoppered flask + mass of water, so mass of water = mass of filled flask - mass of empty flask Mass of water $=$ _____ g $-$ _____ g$=$ ____ g Many mass and volume measurements in chemistry are made by the method used in la. This method is called measuring by difference, and is a very uscful one. b. The density of a pure substance is equal to its mass divided by its volume: Density $=\frac{\text { mass }}{\text { volume }}$ or volume $=\frac{\text { mass }}{\text { density }}$ The volume of the flask is equal to the volume of the water it contains. Since we know the mass and density of the water, we can find its volume and that of the flask. Make the necessary calculation. Volume of water $=$ volume of flask $=$ _____ $\mathrm{cm}^{3}$
(a) To identify a liquid substance, a student determined its density. Using a graduated cylinder, she measured out a 45 -mL. sample of the substance. She then measured the mass of the sample, finding that it weighed 38.5 $\mathrm{g}$ . She knew that the substance had to be either isopropylalcohol (density 0.785 $\mathrm{g} / \mathrm{mL}$ )or toluene (density 0.866 $\mathrm{g} / \mathrm{mL} ) .$ What are the calculated density and the probable identity of the substance? (b) An experiment requires 45.0 $\mathrm{g}$ of ethylene glycol, a liquid whose density is 1.114 $\mathrm{g} / \mathrm{mL}$ . Rather than weigh the sample on a balance, a chemist chooses to dispense the liquid using a graduated cylin-der. What volume of the liquid should he use? (c) Is a graduated cylinder such as that shown in Figure 1.21 likely to afford the accuracy of measurement needed? (d) A cubic piece of metal measures 5.00 $\mathrm{cm}$ on each edge. If the metal is nickel, whose density is $8.90 \mathrm{g} / \mathrm{cm}^{3},$ what is the mass of the cube?
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