ENGR 1540 Worksheet 13 Chapter 4
1. Magnesium nitride forms in a side reaction when magnesium metal burns in air. This reaction may also be carried out in pure nitrogen.
If 18.4 g of Mg3N2 forms from the reaction of 20.0 g of magnesium with excess nitrogen, what is the percentage yield?
2. Industrial production of hydrogen gas uses the reaction shown below. If 1.00 metric ton of propane reacting with excess water yields 270 kg of H2, what is the percentage yield?
3. If 21 g of H2S is mixed with 38 g of O2 and 31 g of SO2 forms, what is the percentage yield?
4. A mixture of 10.0 g of NO and 14.0 g of NO2 results in the production of 8.52 g of N2O3. What is the percentage yield?
5. Small quantities of hydrogen gas can be prepared by the following reaction:
How many grams of H2 can be prepared from 25.0 mL of 6.00 M H2SO4 and excess zinc?
6. Aluminum hydroxide can be dissolved in hydrochloric acid to form aluminum chloride and water. Write a balanced chemical equation for this reaction. How many mL of 3.37 M HCl is needed to react with 10.0 g of Al(OH)3?
7. What volume of 0.812 M HCl, in milliliters, is required to titrate 1.45 g of NaOH to the equivalence point?
8. What volume, in milliliters, of 0.512 M NaOH is required to react completely with 25.0 mL 0.234 M H2SO4?
9. What is the molarity of a solution of nitric acid if 0.216 g of barium hydroxide is required to neutralize 20.00 mL of nitric acid?
10. Hydrazine, N2H4, is a weak base and can react with an acid such as sulfuric acid:
What mass of hydrazine can react with 250. mL 0.225 M H2SO4?
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