# Silver Oxide Lab

Determination of the Empirical Formula of Silver Oxide
College Chemistry
9/12 – 9/13
9/17
The purpose of this lab is to use one of the ways to identify different compounds and be able to tell them apart. Based off of experimentation, the empirical formula of the given silver oxide will be determined. Materials:

Chemicals:
Silver Oxide, 0.5g
Equipment:
Balance, 0.001-g or 0.0001-g precision
Bunsen Burner
Clay pipestem triangle
Crucible and cubicle lid, 15- or 30-mL
Crucible tongs
Ring stand and ring clamp
Watch glass
Wire gauze with ceramic center

Pre Lab Questions

1. Use molar mass of iron to convert the mass of iron to moles. 85.65g/55.9g 1.534 moles of Iron were used
2. According to the law of conservation of mass, what is the mass of oxygen that reacts with the iron? 118.37g – 85.65g = 32.72 grams of Oxygen reacted with Iron 3. Calculate the number of moles of oxygen in the product. 32.72g/15.99g = 2.045 moles is the amount of moles of Oxygen produced 4. Use the ratio between the number of moles of iron and the number of moles of oxygen to calculate the empirical formula of iron oxide. Fe3O2

Procedure:
Set up a Bunsen burner on a ring stand beneath a ring camp holding a clay pipestem triangle. Place the crucible in the clay triangle. Do NOT light the Bunsen burner. Adjust the height of the ring clamp so that the bottom of a crucible sitting in the clay triangle is about 1 cm above the burner. This will ensure that the crucible will be in the hottest part of the flame when the Bunsen burner is lit. Light the Bunsen burner and brush or gently heat the bottom of the crucible with the burner flame for about one minute. Turn off the Bunsen burner and allow the crucible to cool. Using crucible tongs to handle the crucible, measure the mass of a clean, dry, empty crucible and its lid to the nearest 0.001 g. Record the mass in the Data Table. Using proper transfer techniques, add approximately 0.5...