Processing Lab Data MRS. PAGE 2014-2015. After Collecting Data = Process Data  Raw Data: the data you collect during lab without any calculations  Qualitative.

Slides:



Advertisements
Similar presentations
Accuracy & Precision Date: ________ (you must have a calculator for today’s lesson)
Advertisements

Introduction to Chemistry
Scientific Measurement Chapter The Importance of Measurement Qualitative vs Quantitative Measurement What color vs What mass? Scientific Notation.
MEASUREMENT (A Quantitative Observation) MEASUREMENTS always have 2 things: Number & Unit All measurements have error in them! A measurement consists of.
Using Scientific Measurements.
Measurements: Every measurement has UNITS.
Topic 11: Measurement and Data Processing
Measurements and Calculations
PROPAGATION OF ERROR.  We tend to use these words interchangeably, but in science they are different Accuracy vs. Precision.
Measurements and Calculations
Scientific Measurement What is density? From your experimental data, were the densities of the similar objects the same or different? Why? What does this.
Qualitative vs. Quantitative Qualitative = descriptive, non-numerical. ex. : the mornings are getting very cold. Quantitative = numerical, definite measurement.
The color was brownish The volume was 6 mL The weight was 11.5 g What’s the difference between these three pieces of data?
Math is the language of science Data Analysis Ch. 2.1, 2.2, 2.3.
SCIENTIFIC METHOD NOTES # 1 Table of Contents Lecture/Lab/Activity Date Pg# 1.Scientific Organization 8/24/ Scientific Method 8/25/10 1 Objective:
Measurements: Every measurement has UNITS.
Uncertainty and error Distinguish between precision and accuracy Accuracy is how close to the “correct” value Precision is being able to.
Chapter 2 “Scientific Measurement” Standards for Measurement Accuracy vs. Precision Significant Figures.
Reliability of Measurements Chapter 2.3. Objectives  I can define and compare accuracy and precision.  I can calculate percent error to describe the.
Chapter 2 Section 3 Using Scientific Measurements.
Accuracy and Precision Accuracy refers to the how close you are to the actual value. Precision refers to the how close your measurements are to each other.
Flashback Convert 2.58 m to kilometers. Accuracy and Precision Accuracy- the closeness of measurements to the correct value of the quantity measured.
And Problem Solving in Chemistry Precision and Accuracy Significant Figures % error Measurement Density.
Error Analysis Monday, August 17 th. Do Now  Complete the following calculation. Make sure you use the correct amount of sig figs:  x174.5  Once.
Accuracy and Precision. Since all measurements contain an estimated digit, all measurements contain some uncertainty (error). Scientists try to limit.
 It is the steps someone takes to identify a question, develop a hypothesis, design and carry out steps or procedures to test the hypothesis, and document.
IB Mark Schemes Data Collection and Processing Honors Physical Science 2012.
Uncertainty in Measurement
CHEMISTRY = the study of the composition of matter, its chemical and physical changes, and the changes that accompany these changes.
Scientific Measurement Chpt 3. Units of Measure –general qualitative – describes matter – ex. Rough, shiny, heavy, blue quantitative – measures matter.
Accuracy and Precision. Remember these definitions? ► Accuracy – a description of how close a measurement is to the true value of the quantity measured.
Errors and Uncertainties In Measurements and in Calculations.
Chapter 2 Measurements and Calculations Or It all adds up!
Density and % error. Density Density – Compares mass (amount of matter) of object to its volume (amount of space occupied) mass per unit volume (g/cm.
Errors and Uncertainties
20 pt 30 pt 40 pt 50 pt 10 pt 20 pt 30 pt 40 pt 50 pt 10 pt 20 pt 30 pt 40 pt 50 pt 10 pt 20 pt 30 pt 40 pt 50 pt 10 pt 20 pt 30 pt 40 pt 50 pt 10 pt Those.
Chapter 2 Measurements and Calculations. Sect. 2-1: Scientific Method Scientific Method Scientific Method ▫ Observing and collecting Data ▫ Qualitative.
Experimental Error or Uncertainty: Data Analysis and Presentation
Chemistry Chapter 2D Uncertainty in Measurement. Uncertainty  Represents how well a measurement was made  Science is ‘peer reviewed’  We don’t just.
4 x 10 6 cm 3. Do Now: How may cm 3 in 4 m 3 ?. Experimental Errors & Uncertainty.
Chapter 2 © Houghton Mifflin Harcourt Publishing Company Scientific Method The scientific method is a logical approach to solving problems by observing.
Benchmark1 Investigation & Experimentation Review.
Chapter 2 Measurements & Calculations Pages
Matter and Measurement
Measurement and Significant Figures
Using Scientific Measurements.
Measurements and Calculations
Unit 2- Measurements- Accuracy Precision % Error
Density D= Mass_ Volume Mass: put matter on balance Volume:
Using Scientific Measurements.
Chapter 11 Notes Chapter 11.1 All measurement has a limit of precision and accuracy, and this must be taken into account when evaluating experimental results.
Accuracy vs. Precision.
Errors and Uncertainties
Scientific Measurement
Errors and Uncertainties
Warm-Up Perform the following calculations and write your answer with the proper number of sig figs. (1.79 g) / (3.7 mL) = (432.0 cm) x (120 cm) = (2.
Uncertainty and Significant Figures
Chapter 2 Accuracy vs Precision.
Accuracy vs. Precision.
Errors and Uncertainties
Accuracy, Precision, Percent Error, Significant Figures and Rounding
Section 2.3 Uncertainty in Data
Chapter 2.1: Measurements & Calculations West Valley High School
Measurements.
Uncertainty in Measurement
Accuracy and Precision
Sink Scum You are a plumber with an exceptional background in chemistry and you are asked to look at some ooze building up under a local sink. You collect.
Lab Skills Intro.
Chapter 2A: Measurements & Calculations West Valley High School
Presentation transcript:

Processing Lab Data MRS. PAGE

After Collecting Data = Process Data  Raw Data: the data you collect during lab without any calculations  Qualitative Data: Descriptive data – observed with senses, (i.e. what does it look like, sound like, feel like)  Quantitative Data: Measured data using tools. Will be number values.  Processed Data: data as a result of performing calculations AFTER all data has been collected  Raw Data & Processed Data are kept on SEPARATE DATA TABLES!!!

DENSITY

Practice Calculating Density  If you measure an object that has a mass of 8.47 g and a volume of 3.1 cm 3. Calculate the density of the object. Remember Sig. Fig. Rules

YOU TRY  What is the density of an g sample of an unknown substance if the sample occupies 49.6 mL?  What volume would be occupied by 7.75 g of the same substance? (Use the density from the first problem)

Accuracy vs. Precision  Accuracy : how close a measurement is to an accepted value (literature value)  Precision: how close the measurements are to each other

Percentage Error

Practice Calculating Percentage Error  What is the percentage error for a mass measurement of 17.8 g, given that the correct value is 21.2 g? Remember Sig. Fig. Rules

YOU TRY…  A volume is measured experimentally as 4.26 mL. What is the percentage error, given that the correct value is 4.15 mL?  A student measures the mass and volume of a substance and calculates its density as 1.40 g/mL. The correct, accepted, value of the density is 1.30 g/mL. What is the percentage error of the student’s measurement?

Experimental Errors  2 Types: Random & Systematic  Random Errors: unpredictable, chance variations that experimenter has little control over– using many trials and averaging results helps alleviate this type of error. (ex: parallax error)  Systematic Errors: caused by the way in which the experiment was conducted (design). Systematic errors can not be eliminated by averaging. Must change how experiment is conducted. (ex: not calibrating instruments)  Human Error: should not occur if you are focused and careful

HOMEWORK  Read/review pages in your textbook.  Complete questions 1-8 on page 57. SHOW ALL WORK.