Question

1. A 0.750-g sample of tin metal reacts with 0.201 g of oxygen gas to form tin oxide. Calculate the empirical formula of the tin oxide. 

2. A 0.565-g sample of cobalt metal reacts with excess sulfur to give 1.027 g of cobalt sulfide. Calculate the empirical formula of the product. 

3. A 1.164-g sample of iron filings reacts with chlorine gas to give 3.384 g of iron chloride. Calculate the empirical formula of the product? 

4. A 0.626-8 sample of copper oxide was reduced to 0.500 g of copper metal by heating in a stream of hydrogen gas. Calculate the empirical formula of the copper oxide.

5. A sample of phosphorus weighing 0.500 g was ignited to the oxide in a stream of oxygen gas. What is the empirical formula of phosphorus oxide if the product has a mass of 1.145 7 What is the molecular formula of phosphorus oxide if the molar mass is approximately 285 pmol? 

6. (optional) Ethylene glycol, the main ingredient in antifreeze, contains 38.7% carbon 9.7% hydrogen, and 51.6% oxygen. Calculate the empirical and molecular formulas for ethylene glycol, given the molar mass is approximately 60 g/mol

Answer 1