Empirical Formula: SnO2

Mass of tin oxide formed: 1.2665g

The overall reaction is represented in the following unbalanced equation: aSn(s) + b HNO₃ (aq) c Sn_xOy (s) + d H₂O(g) + e NO₂ (g)

1. Having determined the empirical formula of the tin oxide, re-write and balance the overall reaction representing the formation of the oxide.

2. Based on the balanced chemical equation above, calculate the theoretical mass of tin oxide that could have been produced in each determination. Show your work.

3. How do these theoretical amounts compare to the actual amounts obtained? Explain your answer.

4. What is the mass percent of tin and oxygen in the synthesized product? Show your work.

5. How would the loss of some of the metastannic acid during the evaporation of water affect the determination of the empirical formula of the product tin oxide? Explain your answer.

6. What is the Theoretical Yield?