Chemistry Manual 2012-2013 - Edison State College
Chemistry Manual 2012-2013 - Edison State College
Chemistry Manual 2012-2013 - Edison State College
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Blake Schmidt - Unit 1 Page 9<br />
U1 EP2 Unit 1: Example Problems 2<br />
Accuracy/Precision/Significant Figures<br />
1.<br />
Explain how a series of measurements can be precise without being accurate.<br />
2.<br />
Why are significant figures important when reporting measurements?<br />
3.<br />
Suppose a graduated cylinder was not calibrated correctly. How would this effect the results of<br />
a measurement? How would it effect the results of a calculation using this measurement?<br />
4.<br />
5.<br />
6.<br />
How many significant figures are there in each of the following numbers?<br />
a. 0.4004 m<br />
b. 6000 g<br />
c. 1.00030 km<br />
d. 400 mL<br />
Write the following numbers in scientific notation.<br />
a. 0.0006730 g<br />
b. 7500 km<br />
c. 602.2 mm<br />
d. .0094 mg<br />
Calculate the sum of 6.078 g and 0.3329 g.<br />
7.<br />
Subtract 7.11 cm from 8.2 cm.<br />
8.<br />
What is the product of 0.8102 m and 3.44 m?<br />
9.<br />
Divide 94.20 g by 3.16722 mL.<br />
10.<br />
A large building is 1.02 x 10 2 m long, 31 m wide, and 4.25E2 m high. Calculate the volume.
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