Trial 3 Trial 1 Trial 2 Density Unknown Average Density Absolute bevtion 0.C03 .
ID: 1881008 • Letter: T
Question
Trial 3 Trial 1 Trial 2 Density Unknown Average Density Absolute bevtion 0.C03 .oos M- M Average Deviation (AD) Relative Average Deviation (RAD), ppt S.902 RAD X 1000 determined (in parts per thousand, or ppt) is one measure of precision. The closer this is to zero, the closer the data points are to each other, and therefore the higher level 4. The RAD z umber precision associated with the data. Generally, a ppt value of 20 or less represents precise data Based on this, and the value calculated in Data Table 2, can your data be considered precise? 2 Accuracy is a measure of how close and experimental value is to a substance's actual value. Therefore, in order to determine accuracy, the identity (or property of interest) of the substance tested must be known. Based on this, can accuracy be determined with the data collected frorm Part 4? 5. Accuracy is often calculated by determining the percent error between the experimental and actual (or theoretical) value. The lower the percent error (closer to zero), the more accurate the experimental data is. The formula for calculating percent error is: 6. Actual Experimentall Actual Calculate the percent error of the data obtained assuming that the identity of your unknown i Percent Error X 100 a. Dichloromethane (d 1.33 g/mL) b. Water (d 1.00 g/mL) c. Aqueous KCI (d 1.06 g/mL)Explanation / Answer
soln 4.)
Considering the data provided for the column 'trial 2', RAD (relative average deviation) is the closeness of one digits value to the other. For example, 5 and 6 are closest, 5 and 7 are still close. but 5 and 9 or 5 and 1 can be called as not so close.
closer the digits to each other, more precise is the result.
Here the RAD value is given in ppt (parts per thousand) is coming out to be 5.982, which is way below the 20 mark. So, we can definitely call it a precise result.
soln 5)
For accuracy, we need a true value of the property or the identity, but we don't have a true value.
Accuracy is the closeness of a result to the actual value. But here since the actual result is not provided in the table, we can't assure whether the result is accurate or not.
soln 6)
In all the three cases we will use the average density as the experimental value
Experimental value = 1.003 g/mL
a. The actual value of the density of Dichloromethane = 1.33 g/mL
percentage error = (|actual - experimental|/ actual)* 100
= (|1.33-1.003|/1.33)* 100
=24.586 %
b. percentage error for water (1 g/mL)
= (|1-1.003|/1)*100
=0.3 %
c. percentage error for Aqueous KCl (1.06 g/mL)
= (|1.06-1.03|/1.06)*100
=2.83 %
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