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When a solution containing 1.4 g of Ba(NO3)2 and 2.4 g of NH,SO3H is boiled, a precipitate forms. This precipitate may be Ba(NH,SO3)2, BaSO4, or Ba(NH2)2. You can find these products in the reactions whose equations you balanced in the first question. 2. a. Calculate the number of moles of each reactant.

When a solution containing 1.4 g of Ba(NO3)2 and 2.4 g of NH,SO3H is boiled, a precipitate forms. This precipitate may be Ba(NH,SO3)2, BaSO4, or Ba(NH2)2. You can find these products in the reactions whose equations you balanced in the first question. 2. a. Calculate the number of moles of each reactant.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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### Experiment: Precipitation Reaction **Objective:** Determine the precipitate formed when mixing solutions of barium nitrate and ammonium sulfamate. **Materials:** - Barium nitrate, Ba(NO₃)₂ - Ammonium sulfamate, NH₂SO₃H **Procedure:** 1. A solution containing 1.4 g of Ba(NO₃)₂ and 2.4 g of NH₂SO₃H is boiled. 2. Observe the formation of a precipitate. **Analysis:** - The precipitate may be one of the following compounds: - Ba(NH₂SO₃)₂ - BaSO₄ - Ba(NH₂)₂ **Calculation:** a. **Calculate the number of moles of each reactant:** - Use the molar masses of Ba(NO₃)₂ and NH₂SO₃H to convert grams to moles. *Note: Detailed equations and molar mass calculations can be referenced from general chemistry resources.* **Conclusion:** Determining the identity of the precipitate through balanced equations helps understand reaction outcomes. --- This guide should assist in conducting the experiment and understanding the reactions involved.
Transcribed Image Text:### Experiment: Precipitation Reaction **Objective:** Determine the precipitate formed when mixing solutions of barium nitrate and ammonium sulfamate. **Materials:** - Barium nitrate, Ba(NO₃)₂ - Ammonium sulfamate, NH₂SO₃H **Procedure:** 1. A solution containing 1.4 g of Ba(NO₃)₂ and 2.4 g of NH₂SO₃H is boiled. 2. Observe the formation of a precipitate. **Analysis:** - The precipitate may be one of the following compounds: - Ba(NH₂SO₃)₂ - BaSO₄ - Ba(NH₂)₂ **Calculation:** a. **Calculate the number of moles of each reactant:** - Use the molar masses of Ba(NO₃)₂ and NH₂SO₃H to convert grams to moles. *Note: Detailed equations and molar mass calculations can be referenced from general chemistry resources.* **Conclusion:** Determining the identity of the precipitate through balanced equations helps understand reaction outcomes. --- This guide should assist in conducting the experiment and understanding the reactions involved.
### Experiment Instructions **b.** Determine the limiting reactant in each of the following three reactions. The limiting reactant that you determine here will be used directly in this experiment. - **Reaction producing Ba(NH<sub>2</sub>SO<sub>3</sub>)<sub>2</sub>:** - **Reaction producing BaSO<sub>4</sub>:** - **Reaction producing Ba(NH<sub>2</sub>)<sub>2</sub>:** **c.** What conclusion can you reach about the limiting reactant in this experiment?
Transcribed Image Text:### Experiment Instructions **b.** Determine the limiting reactant in each of the following three reactions. The limiting reactant that you determine here will be used directly in this experiment. - **Reaction producing Ba(NH<sub>2</sub>SO<sub>3</sub>)<sub>2</sub>:** - **Reaction producing BaSO<sub>4</sub>:** - **Reaction producing Ba(NH<sub>2</sub>)<sub>2</sub>:** **c.** What conclusion can you reach about the limiting reactant in this experiment?
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