An experiment was carried out similar to the one carried out to determine the empirical formula of magnesium oxide. The empirical formula for an oxide of chromium is required. After heating a 3.00 g piece of pure chromium wire in an excess of air, the sample was cooled and weighed. The mass of the compound formed was 5.769 g. The molar masses of Cr and O are 52.00 g mol-1 and 16.00 g mol-1, respectively
Show all calculations and logic for full marks.
1. How many moles of oxygen combined with the chromium
2. Using the information given, how many moles of chromium were used?
3. What is the empirical formula of the oxide formed?