Download presentation

Presentation is loading. Please wait.

Published byAaron Gill Modified over 4 years ago

1
**Errors and uncertainties in chemistry internal assessment**

The consideration and appreciation of the significance of the concepts of errors and uncertainties helps to develop skills of inquiry and thinking that are not only relevant to the group 4 experimental sciences The treatment of errors and uncertainties is directly relevant in the internal assessment criteria of: data collection and processing, (recording raw data and presenting processed data) conclusion and evaluation, aspects 1, 2 and 3 (concluding, evaluating procedure(s), and improving the investigation).

2
**Within internal assessment students should be able to do the following:**

make a quantitative record of uncertainty range (±) state the results of calculations to the appropriate number of significant figures. propagate uncertainties through a calculation so as to determine the uncertainties in calculated results and to state them as absolute and/or percentage uncertainties.

3
**Random and systematic errors**

Systematic errors arise from a problem in the experimental set-up that results in the measured values always deviating from the “true” value in the same direction, that is, always higher or always lower. Examples of causes of systematic error are miscalibration of a measuring device or poor insulation in calorimetry experiments.

4
**Random uncertainties or errors arise from the inadequacies or limitations in the instrument.**

5
**Random uncertainties What is the length of the object?**

The ruler has scale markings every inch. You must divide each inch to 10 equal parts w/ your eyes and estimate the length of the object to the nearest 1/10 of an inch. ANSWER: 1.5 or 1.4 or 1.6. We’re not certain about the first place after the decimal place. Hence we should record this value as 1.5 ± 0.1.

6
**1.5 ± 0.1 Random uncertainties**

uncertainty of the measurement due to the limitation of the instrument

7
**1.5 ± 0.1 in Random uncertainties**

Means that the true value can be in between 1.4 and 1.6

8
**No, you can estimate only ONE DIGIT, NOT TWO!**

Random uncertainties What is the length of the object? 1.52 in ??? No, you can estimate only ONE DIGIT, NOT TWO!

9
**Uncertainties in measurements…**

form the random errors in the investigations will always be determined as 1/10th of the LEAST CERTAIN DIGIT on the MANUAL EQUIPMENTS!!!

10
**Uncertainties in measurements…**

For uncertainties of the digital equipments, ± the smallest digit that could be measured on that equipment. 2.000 ±0.001 g

11
**While making measurements…**

always remember to estimate ONE MORE DIGIT!!!

12
**total # of significant figures in that measurement**

Random uncertainties in digit we’re certain of digit we estimated 2 sf Total # of digits that we’re certain of + the # of the digit estimated (1)= total # of significant figures in that measurement

13
**Significant figures(carry meaning contributing to its precision)…**

Total # of digits that we’re certain of # of the digit estimated (1) +

14
**Can we eliminate the random errors?**

No, we can only reduce them. the uncertainty is reduced, but it can never be completely eliminated. When recording raw data, estimated uncertainties should always be indicated for all measurements

15
**How can we reduce the random errors?**

repeat measurements, 5 TRIALS AT LEAST! use more precise measuring equipment (?????) MOST EFFECTIVE!!!

16
**Learning check What is the length of the object on both rulers?**

top Ruler: ± 0.1 in bottom Ruler: ± 0.01in Which ruler is more precise?

17
**More precise equipment is…**

the one that gives more digits to the right of the decimal point in measurements.

18
**Precision vs Accuracy in measurements**

19
**Precision vs Accuracy in measurements**

The theoretical value of R (ideal gas law constant)=8.314 J/molK Student A found it as 8.34 ± 0.03 J/molK Student B found it as ± J/molK Which one is more accurate and which one is more precise?

20
**Precision vs Accuracy in measurements**

Student A found it as 8.34 ± 0.03 J/molK (more accurate) Student B found it as ± J/molK (more precise)

21
Accuracy is usually calculated as “PERCENTAGE ERROR.”

22
Accuracy Let’s determine the accuracy of the student A’s and B’s results by calculating the % errors: 8.314 = % 8.314 = 2.39 % (less accurate)

23
**Precision vs Accuracy in measurements**

24
**C. Estimating the uncertainity ( propogation of errors )**

Device Example Uncertainity Analogue scale Ruler,voltmeter,ammeter ,graduated cylinder, thermometer, watch, stopwatch,meters with moving pointers. 1/10th of the smallest scale division Digital scale Top-pan balances , digital meters,voltmeter,pH meter the smallest scale division Reflex time of a person 0.2 seconds Hand out 1) the worksheet about determining uncert 2) the sig fig papers. 3) the calculations about sf

Similar presentations

OK

Uncertainty & Errors in Measurement. Waterfall by M.C. Escher.

Uncertainty & Errors in Measurement. Waterfall by M.C. Escher.

© 2018 SlidePlayer.com Inc.

All rights reserved.

To make this website work, we log user data and share it with processors. To use this website, you must agree to our Privacy Policy, including cookie policy.

Ads by Google