Lab Report
Kiley O’Toole
Lab Report 3
Purpose
The purpose of this lab was to uncover the number of layers of zinc atoms around a piece of galvanized iron. This was done by pouring the hydrochloric acid onto the galvanized iron, thus removing the zinc from the piece of metal.
Laboratory Procedure 1. Measured and recorded the mass of a piece of galvanized iron using a centigram balance and a ruler 2. Measured and recorded the length and width of the galvanized iron using the ruler 3. Put the piece galvanized iron into a 400-ml beaker 4. Added 25mL of hydrochloric acid to the beaker 5. Observed the reaction between the piece of galvanized iron and the hydrochloric acid for five minutes 6. Added 200mL of tap water to the beaker 7. Poured the hydrochloric acid and tap water from the beaker into the sink 8. Removed galvanized iron with forceps 9. While still holding the galvanized iron, rinsed it with tap water 10. Dried metal on paper towel 11. Repeated steps 1 and 2 with the galvanized iron
Observations
Pouring the Hydrochloric Acid on the Galvanized Metal: * Lots of bubbles/fizz * Steam rose from the metal * Metal rose slightly off the bottom of the beaker * Bits of metal fell off
Data and Results | Trial One | Mass of galvanized iron, initial | 3.26g | Length of galvanized iron | 3.4cm | Width of galvanized iron | 3.0cm | Mass of galvanized iron, final | 3.13g | Mass of zinc removed | .13g | Volume of zinc coating | 1.8 x 10-2 g | Volume of zinc coating per side | 9 x 10-3 g | Thickness of coating per side | 9 x 10-4 cm | Number of zinc atoms layers per side | 3.3 x 104 |
Sample Calculations * Mass / Density = Volume * .13g / 7.13g/cm3 = .018cm3 * Number of layers of zinc atoms = Thickness of zinc coating per side(cm) / Diameter of zinc atom (cm) * .0090 / .000000027 = 33,000 or 3.3 x 104 * Volume of Rectangular Solid = length x width x height *
Lab Report 3
Purpose
The purpose of this lab was to uncover the number of layers of zinc atoms around a piece of galvanized iron. This was done by pouring the hydrochloric acid onto the galvanized iron, thus removing the zinc from the piece of metal.
Laboratory Procedure 1. Measured and recorded the mass of a piece of galvanized iron using a centigram balance and a ruler 2. Measured and recorded the length and width of the galvanized iron using the ruler 3. Put the piece galvanized iron into a 400-ml beaker 4. Added 25mL of hydrochloric acid to the beaker 5. Observed the reaction between the piece of galvanized iron and the hydrochloric acid for five minutes 6. Added 200mL of tap water to the beaker 7. Poured the hydrochloric acid and tap water from the beaker into the sink 8. Removed galvanized iron with forceps 9. While still holding the galvanized iron, rinsed it with tap water 10. Dried metal on paper towel 11. Repeated steps 1 and 2 with the galvanized iron
Observations
Pouring the Hydrochloric Acid on the Galvanized Metal: * Lots of bubbles/fizz * Steam rose from the metal * Metal rose slightly off the bottom of the beaker * Bits of metal fell off
Data and Results | Trial One | Mass of galvanized iron, initial | 3.26g | Length of galvanized iron | 3.4cm | Width of galvanized iron | 3.0cm | Mass of galvanized iron, final | 3.13g | Mass of zinc removed | .13g | Volume of zinc coating | 1.8 x 10-2 g | Volume of zinc coating per side | 9 x 10-3 g | Thickness of coating per side | 9 x 10-4 cm | Number of zinc atoms layers per side | 3.3 x 104 |
Sample Calculations * Mass / Density = Volume * .13g / 7.13g/cm3 = .018cm3 * Number of layers of zinc atoms = Thickness of zinc coating per side(cm) / Diameter of zinc atom (cm) * .0090 / .000000027 = 33,000 or 3.3 x 104 * Volume of Rectangular Solid = length x width x height *