Density/Scientific Notation/Significant Digits Name______

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 ______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 x 45.2 cm =

9. 125.5 kg + 52.68 kg + 2.1 kg =

52.8 Pa + 3.0025 Pa 10. = 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)) =

78.26 - 89.50 15. = 678.2 + 9511

16. Calculate the % error for the density of silver from #4 above if the actual density is 10.49 g/cm3.