Take home exam 3 copy

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Take Home Exam
1. Balance the following reactions
1. I2O5 + CO ↔ I2 + CO2
2. NO2 + O3 ↔ N2O5 + O2
3. CS2 + CL2 ↔ CCL4 + S2Cl2
4. NaCl + H2SO4 ↔ Na2SO4 + HCl
5. WO3 + H2 ↔ W + H2O
6. CO2 + H2O ↔ C6H12O6 + O2
7. P4O10 + H2O ↔ H3PO4
8. C5H12 ↔ C5H8 + H2
9. As2O3 + C ↔ CO2 + As
10. Al2O3 ↔ Al + O2
2. N2 (g) + 3H2 ↔ 2 NH3
1. How many moles of NH3 can be produced from 5.25 mol of N2?
2. How many moles of N2 will react with .7 moles of H2?
3. 9.0 moles of NH3 can be produced from how many moles of N2?

3. CaC2 (g) + 2 H2O (l) ↔ C2H2 (g) + Ca(OH)2 (s)
1. Calculate the formula mass for each chemical in the reaction.
2. 62.4 g CaC2 reacts with excess water to yield how many grams of Ca(OH)2?
3. 62.4 g CaC2 reacts with excess water to yield how many liters of C2H2?
4. How many ml of water is consumed in the above reaction? (the density of water

is .98 g/ml for this problem)

4. Fe2O3 (s) + 3 C (s) ↔ 2 Fe (s) + 3 CO (g)
1. 92.7 g Fe2O3 reacts with 16 g C. Identify the limiting reactant and give the theoretical
yield (in moles) of each product.
2. 215.6 g Fe2O3 reacts with 94.7 g C. Identify the limiting reactant and calculate the
theoretical yield of CO in liters.
3. If the percent yield of CO is 85.2% calculate the actual yield of CO (in liters) from #2.
4. If 82.7 liters CO of were actually recovered in problem #2 calculate the percent yield.