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Writing a Lab Report

Writing a Lab Report. Introduction. Background Information What you already know, research, related information, etc. Observations Feel, Touch, Appearance, etc. Be Consistent Problem Experimental question. Hypothesis Possible explanation for a set of observations.

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Writing a Lab Report

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  1. Writing a Lab Report

  2. Introduction • Background Information • What you already know, research, related information, etc. • Observations • Feel, Touch, Appearance, etc. • Be Consistent • Problem • Experimental question. • Hypothesis • Possible explanation for a set of observations. • Your statement must relate to the problem and why you feel that way (Experience, Background Information, and Observations.

  3. Procedure • Materials • Equipment and anything else used to carry out the present experiment. • Do not write “Pen” or “Paper” • Methods • Experimental design, exact procedure followed. • Someone else should be able to do precisely what you did.

  4. Results and Discussion • Data Collected • Graphs, Data Table and Text reporting findings. • You need to have a TABLE, a GRAPH, and PARAGRAPHS reporting your data. • Discussion and explanation of findings. • Interpret data and explain HOW and WHY your data was as it is. • Explain Everything!

  5. Conclusions • Brief Summary of Important Data. • Was your hypothesis proved? Why? • Support your answer • Causes of possible error or uncertainty regarding any portion of the experiment. • If there is none, say that. • Your expert opinion of Why and How the results were as you found them to be. • Take some guesses, Go out on a limb. • Recommendations for future researchers and other related studies that should be done. • What else needs to be studied to gain a better understanding of the current material?

  6. Paper Towel Absorbency Test

  7. Paper Towel Absorbency Test

  8. Scientific Notation

  9. Scientific Notation • 299,800,000 m/sec is the speed of light in a vacuum • 602,000,000,000,000,000,000,000 is the number of atoms in 1 mol Carbon • 0.000000000000000000000001674 g is the mass of one hydrogen atom

  10. Scientific Notation it is extremely cumbersome to do calculations with very large and small numbers so… c x 10n where c is the coefficient and n is the exponent

  11. Scientific Notation • 2.998 x 108m/sec (the speed of light in a vacuum)    • 6.02 x 1023atoms (the number of atoms in 1 mol of carbon) • 1.674 x 10-24g (the mass of one hydrogen atom)

  12. Scientific Notation 1. Move the decimal point so that there is only one digit to the left of the decimal. 2. Count the number of places the decimal moves. 3. If the decimal moves to the left, the exponent on 10 is equal to the number of places the decimal was moved and has a positive sign. 4. If the decimal moves to the right, the exponent on 10 is equal to the number of places the decimal was moved and  has a negative sign.

  13. Practice Problems 7,910,000 .00000000345 1,200,000,000.0 .000098

  14. Practice Problems 0.00416 x 106 24.8 x 10-3 0.716 x 10-4 3410 x 102

  15. Significant Figures Sig Figs

  16. Significant Figures Used to convey the confidence we have in the accuracy of our measuring methods and measurements 8 ± 1 mL (beaker) 8.0 ± 0.1 mL (graduated cylinder) 8.00 ± 0.01 mL (buret)

  17. Significant Figures How many sig figs are in the following??? 23.4g 555001.0100 atoms 200mL 74.221g 3.100mm 0.001201kg

  18. Rules for Sig Fig Rule 1 Zeros between other nonzero digits are significant. Examples • 50.3 m has three significant figures • 3.0025 s has five significant figures

  19. Rules for Sig Fig Rule 2 Zeros in front of nonzero digits are not significant. Examples • 0.892 has three significant figures • 0.0008 s has one significant figure

  20. Rules for Sig Fig Rule 3 Zeros that are at the end of a number and also to the right of a decimal point are significant. Examples • 57.00 g has four significant figures • 2.000 000 kg has seven significant figure

  21. Rules for Sig Fig Rule 4 Zeros that are at the end of a number but left of the decimal point are not significant. Examples • 100 m has ONE significant figure • 20 m has ONE significant figure

  22. Rules for Sig. Fig. Extra Rule Zeros that are at the end of a number but left of the decimal point that are measured to be significant are indeed significant. Examples • A scale measures 1200. kg has four significant figures and is written in scientific notation: • 1.200 x 10 kg so Rule 3 applies 3

  23. Rules for Sig Fig

  24. Significant Figures Put the following into scientific notation… 23.4g 555001.0100 atoms 200mL 74.221g 3.100mm 0.001201kg

  25. Significant Figures Round the following to the indicated number of significant figures. 23.4 g (2 sig figs) 555001.0100 atoms (3 sig figs) 2001.0345mL (5 sig figs) 74.221g (3 sig figs) 3.100mm (3 sig figs) 0.001201kg (3 sig figs)

  26. Rules for Calculating with Significant Figures

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