Your task is to find the density of a liquid. You mistakenly fill the 10 mL...
Your task is to find the density of a liquid. You mistakenly fill the 10 mL volumetric flask all the way to the top, to overflowing, and find the mass of the overfull flask. Then you subtract the mass of the empty flask to get the mass of the liquid. In your calculations, you use 10 mL as your volume; will your result (the calculated density) be too high or too low? Explain.
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Your task is to find the density of a liquid. You mistakenly
fill the 10 mL...
What is the effect on the calculated density of the unknown metal or liquid under the...
What is the effect on the calculated density of the unknown metal or liquid under the following conditions? After the flask was filled with unknown liquid the cover slip was placed on top. In doing so a small air bubble was trapped under the cover slip. When determining the density of the unknown metal, the flask was filled less than one quarter way with the metal instead of halfway. When determining the volume of the flask, the student did not...
A student was given a 10 mL sample of a clear, colorless liquid. She was assigned...
A student was given a 10 mL sample of a clear, colorless liquid. She was assigned the task of identifying the unknown liquid and was told that the sample could be methanol (CH_3OH), acetone (C_3H_6O), or ethanol (C_2H_5OH). She decided to attempt to determine the molar mass of the liquid by the vapor density method, which involves completely vaporizing a small sample of the liquid, cooling it and determining the mass of the condensed vapor. She also collects the volume...
You are checking the accuracy of a volumetric flask marked 10.00 mL . To calculate the...
You are checking the accuracy of a volumetric flask marked 10.00 mL . To calculate the volume of water contained in the flask, you first measure the mass of the empty flask and the mass of the flask filled with water and take the difference. Then, you correct for the buoyancy factor and divide by the density of the water. The result of 8 such measurements is given in the table. Calculate the mean and the 95% confidence interval for...
For the Unknown Liquid, suppose the first three measurements (empty, w/ 5mL, and w/ had no...
For the Unknown Liquid, suppose the first three measurements (empty, w/ 5mL, and w/ had no major error, but then you chipped your cylinder and the mass was too low for 10mL the last 3 measurements (w/ 15mL, w/ 20mL, and w/ 25mL). Briefly explain whether this would cause your calculated density to be too High or too Low (think about slope).
2. In attempting to calculate the density of chloroform, CHCl3, Riley determines the following densities: 1.30...
2. In attempting to calculate the density of chloroform, CHCl3, Riley determines the following densities: 1.30 g/mL, 1.35 g/mL, 1.32 g/mL, 1.23 g/mL, 1.13 g/mL, and 1.39 g/mL. a. Calculate the average density of chloroform from his data. b. If the accepted density of chloroform is 1.48 g/mL, calculate the percent error. C. Was Riley's data accurate? Was the data precise? Explain your reasoning. Experiment 1: Determination of the Density of Water and nft page 14 3. For each of...
Part B: Density of a liquid. unknown number #118 First add 10 ml of the unknown...
Part B: Density of a liquid. unknown number #118 First add 10 ml of the unknown liquid...... Erlenmeyer Flask + stopper = 32.3540 g Erlenmeyer Flask + stopper + unknown liquid (10.00ml) = 41.3460 g Then add another 10.00 ml of unknown liquid into the flask, so that the sample is 20.00 ml Erlenmeyer Flask + stopper + unknown liquid (10.00 ml + 10.00 ml = 20.00 ml) = 49.9595 g Find the density of unknown liquid?
You are checking the accuracy of a volumetric flask marked 10.00 mL. Measurement| Volume (mL) You...
You are checking the accuracy of a volumetric flask marked 10.00 mL. Measurement| Volume (mL) You measure the volume of water contained in the flask by measuring the mass of the empty flask, the mass of the flask filled with water, taking the difference, correcting for the buoyancy factor, and dividing by the density of the water. The results of eight such measurements are given in the table 10.064 10.063 10.017 10.049 10.020 10.025 10.045 10.008 2 3 4 5...
#13-#14 13. When you finish your calculations for the previous experiment, you find the density of...
#13-#14
13. When you finish your calculations for the previous experiment, you find the density of your piece of metal to be 10.72 g/mL. Your instructor says that the metal you have has a true density of 11.34 g/mL. What is your percent error? 14. You are instructed to make up a solution that is 0.25 M NaCI(aq). You are provided with table salt (Molar mass = 54.443 g/mol); a supply of water; a balance, and a 1000-mL volumetric flask....
i dont understand why the molecular weight i calculated (42.012 g/mol) for my unknown liquid (acetone)...
i dont understand why the molecular weight i calculated
(42.012 g/mol) for my unknown liquid (acetone) is less than the
actual molecular weight (58.08 g/mol). what errors could i have
made in my lab that would account for the difference.
Molecular Weight of a Volatile Liquid In this experiment, an amount of liquid more than sufficient to fill the flask when vaporized is placed in a flask of measured volume and mass. The flask is then heated in a boiling...
im stuck on 3 and 4... data on second sheet raye 2 3. You carelessly remove...
im
stuck on 3 and 4...
data on second sheet
raye 2 3. You carelessly remove the stopper from Flask #1 after the water has been sucked back in and allow the water in the rubber tubing to flow into Flask #1. How does that mistake affect the calculated value of the ratio in Equation 4 (too high or too low)? Explain your answer. 4. When you determine the volume of air in Flask #1 (Steps 21 & 22), you...
A student was given a 10 mL sample of a clear, colorless liquid. She was assigned the task of identifying the unknown liquid and was told that the sample could be methanol (CH_3OH), acetone (C_3H_6O), or ethanol (C_2H_5OH). She decided to attempt to determine the molar mass of the liquid by the vapor density method, which involves completely vaporizing a small sample of the liquid, cooling it and determining the mass of the condensed vapor. She also collects the volume...
For the Unknown Liquid, suppose the first three measurements (empty, w/ 5mL, and w/ had no major error, but then you chipped your cylinder and the mass was too low for 10mL the last 3 measurements (w/ 15mL, w/ 20mL, and w/ 25mL). Briefly explain whether this would cause your calculated density to be too High or too Low (think about slope).
2. In attempting to calculate the density of chloroform, CHCl3, Riley determines the following densities: 1.30 g/mL, 1.35 g/mL, 1.32 g/mL, 1.23 g/mL, 1.13 g/mL, and 1.39 g/mL. a. Calculate the average density of chloroform from his data. b. If the accepted density of chloroform is 1.48 g/mL, calculate the percent error. C. Was Riley's data accurate? Was the data precise? Explain your reasoning. Experiment 1: Determination of the Density of Water and nft page 14 3. For each of...
You are checking the accuracy of a volumetric flask marked 10.00 mL. Measurement| Volume (mL) You measure the volume of water contained in the flask by measuring the mass of the empty flask, the mass of the flask filled with water, taking the difference, correcting for the buoyancy factor, and dividing by the density of the water. The results of eight such measurements are given in the table 10.064 10.063 10.017 10.049 10.020 10.025 10.045 10.008 2 3 4 5...
#13-#14
13. When you finish your calculations for the previous experiment, you find the density of your piece of metal to be 10.72 g/mL. Your instructor says that the metal you have has a true density of 11.34 g/mL. What is your percent error? 14. You are instructed to make up a solution that is 0.25 M NaCI(aq). You are provided with table salt (Molar mass = 54.443 g/mol); a supply of water; a balance, and a 1000-mL volumetric flask....
i dont understand why the molecular weight i calculated
(42.012 g/mol) for my unknown liquid (acetone) is less than the
actual molecular weight (58.08 g/mol). what errors could i have
made in my lab that would account for the difference.
Molecular Weight of a Volatile Liquid In this experiment, an amount of liquid more than sufficient to fill the flask when vaporized is placed in a flask of measured volume and mass. The flask is then heated in a boiling...
im
stuck on 3 and 4...
data on second sheet
raye 2 3. You carelessly remove the stopper from Flask #1 after the water has been sucked back in and allow the water in the rubber tubing to flow into Flask #1. How does that mistake affect the calculated value of the ratio in Equation 4 (too high or too low)? Explain your answer. 4. When you determine the volume of air in Flask #1 (Steps 21 & 22), you...
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