After ten (10) measurements using your weighing scale at home, you realize that you were not measuring at a level surface. Instead you discover that your balance has been sitting at a 4° incline all this time. Given the nature of how a balance works, you know that there will be some error introduced into all ten of your readings. O systematic O random

After ten (10) measurements using your weighing scale at home, you realize that you were not measuring at a level surface. Instead you discover that your balance has been sitting at a 4° incline all this time. Given the nature of how a balance works, you know that there will be some error introduced into all ten of your readings. O systematic O random

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter3: Measurement And Chemical Calculations

Section: Chapter Questions

Problem 128E: In Active Example 3-29 you calculated that you would have to work six weeks to earn enough money to...

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In Active Example 3-29 you calculated that you would have to work six weeks to earn enough money to buy a 1082.49 television. You would be working five shifts of four hours each at 9.25/hr. But, alas, when you received your first pay check, you found that exactly 23 of your earnings had been withheld for social security, federal and state income taxes, and workers compensation insurance. Taking these into account, how many weeks will it take to earn the 1082.49?
To identify a liquid substance, a student determined itsdensity. Using a graduated cylinder, she measured out a 45-mLsample of the substance. She then measured the mass of thesample, finding that it weighed 38.5 g. She knew that the substancehad to be either isopropyl alcohol 1density 0.785 g>mL2or toluene 1density 0.866 g>mL2. What are the calculated densityand the probable identity of the substance?
Why should the selected rule(s) be followed? A residue left on the balance will contaminate the balance pan surface and anything that comes into contact with it afterwards. There may be discrepancies in accuracy between individual balances. Objects at any temperature other than room temperature can create air currents which can affect the balance pan, causing the measured mass to be higher or lower than the true mass. Weighing wet items will cause the displayed mass to be greater than the actual mass of the object.
1. A piece of metal was weighed on a laboratory balance five times and gave the following values: 15.75, 15.73, 15.77, 15.76and 15.74 grams.Determine the average mass andstandard deviation from the mean mass.(b) An object weighs 0.0930 gramson an analyticalbalance. Indicate theaccuracy of the balance and the number of significant figures in this weight.
One student calibrated a 50-mL burette by using the mass of water delivered. The student used an analytical balance which was previously calibratedby STEEL (density = 7.8 g/mL). During calibration, the temperature of water was found to be 19.0oC. The density of water at this temperature is0.9984 g/mL. The results of the calibration by the student is shown in the table below: Apparent burette reading, mL A-10.05 ml, B- 20.04ml, C- 30.08ml, D- 40.07 ml, E- 49.98ml Weight H2O delivered, g A -10.03g, B- 20.09g, C- 30.05g, D- 40.02g, E- 49.83g
The mass of a glass beaker is known to be 24.4 gg. Approximately 5 mLmL of water are added, and the mass of the beaker and water is measured on an analytical balance to be 30.625 gg. How many significant figures are there in the mass of the water?
Using the relative uncertainty for these densities, which used the balance. Balance Density A 0.7834 g/mL B 0.7836 g/mL C 0.781 g/mL In addition, these approximate uncertainities using the buret. Balance A: ± 0.001 Balance B: ± 0.01 Balance C: ± 0.1 In each case, does the uncertainty associated with using the balance or the buret contributemore of the uncertainty in the density? (Answer "balance," "buret," or "the same" if applicable) A: B: C:
Please answer this question as fast as you can please and tahnk you. I will afterwards write an wonderful review on solving the question. Thank you. For each piece of glassware measure the density of water in triplicate (three times). Why repeat the procedure multiple times for each piece of glassware? Running the measurement in triplicate increases the precision of our results and reduces the impact of a single outlier result. The experiment would be too short if you only ran each trial once The first two trials act as practice, and the final trial will give you the true result. Running the measurement in triplicate increases the accuracy of our results and reduces the impact of a single outlier result.
1.) A dense plastic-like shape has a mass of 42.985 g and has a volume of 41.96 mL. What is the density of the substance? 2.) Another plastic-like piece has a mass of 65.389 grams and displaces 53.652 grams of water (measured at 24.6 ⁰C). Is this piece likely to be composed of the same material as the sample in problem 1? Explain using the Claim-Evidence-Reasoning process.
The pharmacist attempts to weigh 0.375 g o morphine sulfate on a balance of dubious accuracy. When checked on a highly accurate balance, the weight is found to be 0.400 g. Calculate the percentage of error in the first weighing.
The pharmacist weight 800 mg of a substance on a balance of dubious accuracy. When checked on a balance of high accuracy, the weight was found to be 785mg. calculate the percentage error in the first weighing.
(a) To identify a liquid substance, a student determined itsdensity. Using a graduated cylinder, she measured out a 45-mLsample of the substance. She then measured the mass of thesample, finding that it weighed 38.5 g. She knew that the substancehad to be either isopropyl alcohol (density 0.785 g/mL)or toluene (density 0.866 g/mL). What are the calculated densityand the probable identity of the substance? (b) An experimentrequires 45.0 g of ethylene glycol, a liquid whose densityis 1.114 g/mL. Rather than weigh the sample on a balance, achemist chooses to dispense the liquid using a graduated cylinder.What volume of the liquid should he use? (c) Is a graduatedcylinder such as that shown in Figure 1.21 likely to afford theaccuracy of measurement needed? (d) A cubic piece of metalmeasures 5.00 cm on each edge. If the metal is nickel, whosedensity is 8.90 g/cm3, what is the mass of the cube?