2) As an example of precision and accuracy of data, suppose the % carbon in a single compound has beenmeasured thrce separate times by 2 different students. The theoretical % carbon is 21.34%.Student 1: trial 1:26.11%,trial 2: 26.24%trial 3: 25.92 %,Avg - 26.09Student 2: trial 1: 20.35%.trial 2: 22.64 %trial 3: 19.79 %.Avg = 20.93a) Which student had the more precise data and how can you tell?b) Which student had the more accurate data and how can you tell?3a) Calculate the % error of Student 1 data in problem 2 above. Show all work below. WATCH SIG FIGS

Accuracy means the value comes close to actual true value and Precision means all the trial values…

Answered: 2) As an example of precision and…

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter11: Intermolecular Forces And Liquids

Section11.6: Properties Of Liquids

Problem 1.2ACP

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(8) Identify whether the following are examples of systematic or random error or are mistakes: a. Using an inaccurately calibrated buret. b. An uncertainty of 1 mg in the weight of your sample.∓ c. Overshooting the endpoint on your first sample, then hitting the endpoint on the remaining samples.d. Failing to let your volumetric pipet drain for a few seconds have most of the liquid has been delivered.
Example 2: You prepared a 0.250 M NH3 solution by diluting 8.45 (±0.04) mL of 28.0 (10.5) wt% NH3 [density = 0.899 (+0.003) g/mL] up to 500.0 (±0.2) mL. Find the uncertainty in 0.250 M. The molecular mass of NH3, 17.0306 g/mol, has negligible uncertainty relative to other uncertainties in this problem.
aur X Macmilla X 2/ Course X 50 ~ T Sections X Submit Answer evo/index.html?deploymentid=5735112480241329813180832311&elSBN=9781305862883&id=1707786042&snapshot! References lancing Molecular Equations: This is group attempt 2 of 10 HOMEW X Use the References to access Important values if needed for this question. When the following molecular equation is balanced using the smallest possible Integer coefficients, the values of these coefficients are: Na (s) + H₂0 (1). NaOH (aq) + H₂ (8) ≡く □ □ A MindTap ㅁ Autosaved at 5:51 PM MacBook Air Gatoms to When the following molecular equation is balanced using the smallest possible Integer coefficients, the values of these coeffi Br₂(g) + Cl₂(g) →BrCl(g) X Dom
EXAMPLE Significant Figures in Laboratory Work You prepared a 0.250 M NH, solution by diluting 8.46 (0.04) mL of 28.0 (10.5) wt% NH, [density=0.899 (+0.003) g/mL] up to 500.0 (+0.2) mL. Find the uncertainty in 0.250 M. The molecular mass of NH3, 17.031 g/mol, has negligible uncertainty relative to other uncertainties in this problem.
My answer here is 18.5 % and 1.98 ft3 please verify
9) The following results were obtained in the determination of Vitamin E mass in tablet samples. Sample 1 2 3 4 5 6 Weight of Vitamin E (mg) 249.1 249.9 251.2 250.2 244.8 251.0 i. Determine whether any data should be rejected or not at 90 % confidence level. ii. Calculate the mean and standard deviation of the data set above. ii. Express the mean weight of vitamin C at 99 % confidence interval.
What is the absolute uncertainty and relative uncertainty of the molarity of the solution? M = = 0.078376462 = 0.078 M Pb2+
Analysis was run on samples from a known CRM with 8.85% Fe. The following results for %Fe were obtained by an analyst: 8.75, 8.51, 8.25, 8.61. Which of the following statements is true assuming none of the data points are outliers? Group of answer choices Tcalc = 63.15 The analysis is not accurate at the 95% confidence interval. Tcalc = 3.03 The analysis is accurate at the 95% confidence interval. Not enough information to determine Tcalc = 63.15 The analysis is accurate at the 95% confidence interval. Tcalc = 3.03 The analysis is not accurate at the 95% confidence interval.
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Sample IdentificationCodeConcentration of M%TA=2-log(%T)Q50004.00 x 10-417.90.75Q50013.20 x 10-425.00.6Q50022.40 x 10-435.70.46Q50031.60 x 10-450.20.3Q50048.000 x 10-570.80.15SampleIdentificationCode%TA=2-log(%T)AMQ0210150143.70.359518560.360.000192Q0210150244.10.355561410.360.00018Q0210150343.80.358525890.360.00017Q0210150444.10.355561410.360.00018Q0210150543.80.358525890.360.00017What was their percent error?43%Does Batch 021015 meet legal requirements?No, because it is not between 2.85 * 10(4) and 3.15 * 10(4)Well #DropsBluedye1234567891012345678910Drops 9Distilled water876543210Concne 0.26tration0.52Test Tube #0.781.041.3Solutions3Concentration (M)2.082.32.6Concentration (ppm)1:1 dilution11.82Starting Dilution21.562:1 dilution0A.Zero standard0Was your calibration curve as linear as you expected?B.Did you experience any â€œdriftâ€ of the resistance readings?C.What is the equation of your best-fit line?D.What commercial drink did you analyze?E.Assuming…
I. GRAVIM ETRIC CALCULATIONS Complete the table below. Calculate the % (w/w) BaSO4 and the statistical analysis needed in the table. Show your complete solution and indicate your final answer in proper significant figures. Trial 1 Trial 2 Trial 3 Weight of Sample 0.6020 g 0.5021 g 0.5018 g 24.8405 g 22.8165 g 22.8169 g Weight of Crucible and BaS04 24.8451 g 22.8165 g 22.8169 g 24.8422 g 24.8422 g Constant Weight of Crucible & Sample 24.8422 g 22.8165 g 22.8169 g W eight of Crucible 24.3181 g 22.3593 g 22.3641 g 24.3160 g 22.3523 g 22.3612 g 24.3142 g 22.3534 g 22.3605 g 24.3142 g 22.3532 g 22.3605 g 24.3142 g 22.3532 g 22.3605 g 24.3142 g 22.3532 g 22.3605 g Constant Weight of Crucible Weight of BaSO4 % SO,2- A verage Standard deviation Relative standard deviation
1. How many milliliters of 53.40(±0.06) (w/w) % NaOH with a density of 1.52(±0.01)g/mL will you need to prepare 1.000 L of 0.200 M NaOH? Keep 1 extra sig fig in your answer (4). 2. If the uncertainty in delivering NaOH is ±0.01 mL, calculate the absolute uncertainty in molarity (0.200 M). Assume there is negligible uncertainty in the formula mass of NaOH and in the final volume (1.000 L) Hint: You will need to calculate the molarity of the 53.40% NaOH. One way to solve this is to assume that you have 100.00 grams of the initial NaOH solution. Determine how many grams are NaOH. Convert that value to moles NaOH. Using the density, determine the volume of your 100.00 grams of solution.

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