CHEMISTRY 121 MIDTERM #1B OCTOBER 25, 2013 2.54 cm = in, 946mL=qt, 454g=lb, 5280 ft = mi, 12in=ft 1. Convert the following measurements into scientific notation and provide the number of significant figures. a. 100 b. 101.0 c. 0.01101 d. 45400.0 2. What is the empirical formula of glucose C6H12O6. 3. Give names for the following formulas: Name the Following Give Formulas a. Fe2S3 a. Hypochlorus acid b. Mn2O7 b. SO3 c. S4N2 c. Hydrogen oxide d. HCN (aq) d. Chromium(VI) oxide e. HCl (g) e. Carbon tetrachloride f. H2S (aq) f. Zinc acetate 4. What does the atomic number tell us about an element? 5. What does the mass number describe about an isotope? 6. What is the difference between an ionic compound and a molecular compound? 7. How many elements are in period 2 of the periodic chart? 8. A compound contains 52.0 % Cr and 48.0% O. Determine the empirical and molecular formulas if the molar mass is 200.0 g/mole. 9. Give an appropriate unit for each of the following. a. Time b. Specific heat c. Mass d. Volume e. Density f. Energy 10. Convert 72.3 x 10-16 km3 to cm3. 11. Label the following changes as chemical or physical a. Folding of paper b. Milk turning sour c. Magnetizing a piece of steel d. Healing of a wound e. Diamonds burning f. Melting of a diamond g. Dry ice subliming 12. Find the number of atoms of hydrogen in a 16.2 g sample of glucose C6H12O6. 13. A 1.33 g sample of metal absorbs 2.31 j of heat causing its temperature to increase from 25.0 °C to 33.6°C. Calculate the specific heat of the metal. 14. What mass of water contains the same number of oxygen atoms as a 33.4 g sample of glucose C6H12O6 15. Mercury has a density of 13.6 g/mL. Find the volume in quarts of 5.00 lbs of mercury. 16. A 5.94 g sample of aluminum oxide contains 3.66 g of Al contains 3.14 g of aluminum. Give the % composition of this sample of aluminum oxide.