3) In a chemical reaction between nitrogen and hydrogen, 5.0 moles of hydrogen are reacted with excess nitrogen. To determine how many moles of ammonia are produced, what conversion factor should be used?

Use this balanced equation for the Haber process: N₂ (g) + 3 H₂ (g) → 2 NH₃

 

_4) In a chemical reaction shown in the equation below, ammonia reacts with nitrogen monoxide to produce nitrogen and water.

4 NH₃ + 6 NO → 5 N₂ + 6 H₂O

How many moles of NH₃ are necessary to produce 0.824 mol N₂?

 

5) Magnesium metal reacts with a solution of silver nitrate in a single-replacement reaction, producing aqueous magnesium nitrate and silver metal. 

If a reaction starts with 0.480 mol Mg, how many moles of silver are produced?

You must show a proper set up for the calculation, the answer with a proper unit, and the proper significant figures. 

 

6) Aluminum reacts with sulfur to form aluminum sulfide according to the following reaction:

2 Al (s) + 3 S (s) → Al₂S₃ (s)

How many grams of aluminum sulfide will be produced if 5.00 grams of aluminum is reacted with excess sulfur?

 

7)If 2.75 grams of calcium react with 1.10 grams of oxygen in the following reaction, what mass of calcium oxide will be produced?

2 Ca (s) + O2 (g) → 2 CaO (s)

 

8) Ethane gas (C₂ H₆) burns to produce carbon dioxide and water according to the following chemical equation. All gases are measured at the same temperature and pressure:

2 C₂ H₆ (g) + 7 O₂ (g) → 4 CO₂ (g) + 6 H₂O (g) 

How many liters of oxygen are required to react with 2.50 liters of ethane? 

 

9) Sodium chloride reacts with silver nitrate in a water solution, producing aqueous sodium nitrate and solid silver chloride. 

1) Write a balanced chemical equation for the reaction. Include the phases for all reactants and products. 

2) What mass of sodium chloride is needed if 3.00 moles of silver nitrate are reacted? Show all of your work. 

To receive full credit, show all of your work, including ratios and molar mass calculations.

 

10) 26.7 g of nickel metal reacted with 178 g of silver nitrate in the following chemical reaction:

Ni (s) + 2 AgNO3 (aq) → Ni(NO3)2 (aq) + 2 Ag (s)

 

1) What is the limiting reactant? You must show:

1. how you find out the molar mass of AgNO₃,
2. how you find out the amount of AgNO₃ needed for the reaction including the calculation with a proper set up
3. how you know what the limiting reactant is with a proper reasoning.

2) What mass of silver metal will be produced?

You must show all your work including a proper set up, calculations, and proper significant figures.

SuperTutor

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Status NEW Posted 15 May 2017 12:05 AM My Price 12.00

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