1. 

Consider the reaction I₂O_5(g) + 5 CO_(g) → 5CO_2(g) + I_2(g)

 80.0 grams of iodine pentoxide, I₂O₅ (molar mass = 333.80g/mol), reacts with 38.0 grams of carbon monoxide (molar mass 28.01g/mol). Determine the mass of iodine that could be produced.

2.  

If, in the above question, only 32.0g I2 was produced, what percent yield of iodine was produced?

 You must use your answer from the question above.

3. 

Use the balanced equation. CaCO3  +  SO2 → CaSO3 + CO2

 In a particular experiment, 255 g of CaCO3 (molar mass = 100.09g/mol) was exposed to 135 g of SO2 (molar mass = 64.07g/mol).What is the maximum number of CaSO3 (molar mass = 120.15g/mol) in grams that can be produced?

4. If only 198 g of CaSO3 was isolated from the products in the question above, what was the percentage yield in grams of CaSO3 in this experiment?

5. 

If after completing the experiment from problem 3 above (do not take any information from problem 4 above), your percent yield was 88.20%, what must the actual yield have been?

6. 

Would 26.5g sodium or 32.5g sulfur be the limiting reagent in the following formula when solving for moles:

 12Na + S6 → 6Na2S ?

7. 

CS2 + 3O2 → CO2 + 2SO2  

If 6.0mol of CS2 and 6.0 mol of O2 react to form moles of the products.

8. In the reaction 2Al + 3F2 → 2AlF3, what would be the actual yield if 50.0g of fluorine reacts with 50.0g of aluminum and the percent yield was 75.20% moles AlF3?

9.  

5O2 + P4 → P4O10

If 45.0g of phosphorus is reacted with 75.0g of oxygen to produce .21mol of P4O10 what is the percent yield? (Be careful, there is an easy molar mass mistake in this one)