# 2.3 Practice Name_________________________________ Density/Scientific Notation/Significant Digits ```2.3 Practice
Name_________________________________
Density/Scientific Notation/Significant Digits
Date _______________ Period ____________
Directions: Complete the following density problems. You must show all work to receive credit. Remember
to include your units and don’t forget significant digits!
1. A block of aluminum has a mass of 36.40 g and a volume of 13.5 cm3. What is the block’s density?
2. The density of CCl4 (carbon tetrachloride) is 1.58 g/mL. What is the mass of 95.7 mL of CCl4?
3. What is the volume of 227 g of olive oil if its density is 0.92 g/mL?
4. Calculate the density of silver if a student measured a mass of 201.0 g and volume of 18.9 cm3?
5. The density of a block of ice is 0.917 g/cm3. How much volume does 52.3 g of ice occupy?
6. Express the following numbers in scientific notation or regular form:
a. 8960
_______________
f. 4.563 x 107
__________________
b. 0.000 23
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g. 2.53 x 10-3
__________________
c. 86,000
_______________
h. 6.805 x 108
__________________
d. 36,000,000
_______________
i. 5.6 x 10-2
__________________
e. 0.000 000 025 3
_______________
j. 3.29 x 104
__________________
7. Identify and write the number of significant digits in each of the following measurements:
a. 520 mL
__________
e. 10.002 ns ___________
b. 0.0102 ns
__________
f. 0.451 Pa
___________
c. 0.230 kg
__________
g. 0.001 cm
___________
d. 25,600 L
__________
h. 0.0010010 ___________
Perform the following calculations and round off the answer to the correct number of significant digits.
8. 0.3287 cm
9.
10.
x
45.2 cm =
125.5 kg + 52.68 kg + 2.1 kg =
52.8 Pa + 3.0025 Pa

253.4 Pa
11. (0.12 cm + 5.16 cm) x (93.0 cm - 45.56 cm) =
12. 68.32 ns + (-1.001 ns) + (-0.00367 ns) + (-678.1 ns) =
13. 0.258 mL  0.36105 mL =
14. (1250 - (234.207  52.69)) =
15.
78.26 - 89.50
=
678.2 + 9511
16.
Calculate the % error for the density of silver from #4 above if the actual density is 10.49 g/cm3.
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