Question

5. Under a high-pressure atmosphere of oxygen, the compound C7H11O4NS2 is burned.

A. Write the balanced equation for this reaction. You may assume all the nitrogen is converted to NO2 and the sulfur is converted to SO3. Coefficients should represent the smallest whole number ratio of all reactants and products – no fractional coefficients. (7.5 pts.)

B. If 77.6 g of the compound is burned, what is the mass of each product? (7.5 pts

6. Consider the reaction: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g)

Molar masses (g/mol): Fe2O3 = 159.7 CO = 28.01 Fe = 55.85 CO2 = 44.01

A. What is the theoretical yield of iron if 16.0 g of iron (III) oxide is reacted with 7.25 g of carbon monoxide? (7.5 pts.)

B. What mass of the excess reagent remains if a complete reaction occurs? (7.5 pts.)