Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Chemical Equilibrium and Yield Calculations**
Given the data:
- 2.32 grams of Beryllium Chloride (BeCl\(_2\))
- 0.90 grams of Lithium Hydride (LiH)
- Products are 0.19 grams of Beryllium Hydride (BeH\(_2\)) and 0.92 grams of Lithium Chloride (LiCl)
Answer the following questions:
1. **How many moles of BeCl\(_2\) do you have?**
\[ \text{Moles of BeCl}_2 = \frac{\text{Grams of BeCl}_2}{\text{Molar Mass of BeCl}_2} \]
2. **How many moles of LiH do you have?**
\[ \text{Moles of LiH} = \frac{\text{Grams of LiH}}{\text{Molar Mass of LiH}} \]
3. **What is your limiting reagent?**
- Determine which of the reactants is consumed first in the reaction by comparing the mole ratios.
4. **What is your theoretical yield of BeH\(_2\) in moles?**
\[ \text{Theoretical Yield (moles)} = \text{Moles of Limiting Reagent} \times \frac{\text{Coefficient of BeH}_2 \text{ in balanced equation}}{\text{Coefficient of Limiting Reagent}} \]
5. **What is your theoretical yield of BeH\(_2\) in grams?**
\[ \text{Theoretical Yield (grams)} = \text{Theoretical Yield (moles)} \times \text{Molar Mass of BeH}_2 \]
6. **What is your theoretical yield of LiCl in moles?**
\[ \text{Theoretical Yield (moles)} = \text{Moles of Limiting Reagent} \times \frac{\text{Coefficient of LiCl in balanced equation}}{\text{Coefficient of Limiting Reagent}} \]
7. **What is your theoretical yield of LiCl in grams?**
\[ \text{Theoretical Yield (grams)} = \text{Theoretical Yield (moles)} \times \text{Molar Mass of LiCl} \]
Use the molar masses for the calculations:
- BeCl](https://content.bartleby.com/qna-images/question/19c732c8-efee-414f-84d3-ed7ea6f7d2e9/38fcc1d4-9423-464d-b28b-2e5936f26d5d/0nfl4xa_processed.jpeg)
Transcribed Image Text:**Chemical Equilibrium and Yield Calculations**
Given the data:
- 2.32 grams of Beryllium Chloride (BeCl\(_2\))
- 0.90 grams of Lithium Hydride (LiH)
- Products are 0.19 grams of Beryllium Hydride (BeH\(_2\)) and 0.92 grams of Lithium Chloride (LiCl)
Answer the following questions:
1. **How many moles of BeCl\(_2\) do you have?**
\[ \text{Moles of BeCl}_2 = \frac{\text{Grams of BeCl}_2}{\text{Molar Mass of BeCl}_2} \]
2. **How many moles of LiH do you have?**
\[ \text{Moles of LiH} = \frac{\text{Grams of LiH}}{\text{Molar Mass of LiH}} \]
3. **What is your limiting reagent?**
- Determine which of the reactants is consumed first in the reaction by comparing the mole ratios.
4. **What is your theoretical yield of BeH\(_2\) in moles?**
\[ \text{Theoretical Yield (moles)} = \text{Moles of Limiting Reagent} \times \frac{\text{Coefficient of BeH}_2 \text{ in balanced equation}}{\text{Coefficient of Limiting Reagent}} \]
5. **What is your theoretical yield of BeH\(_2\) in grams?**
\[ \text{Theoretical Yield (grams)} = \text{Theoretical Yield (moles)} \times \text{Molar Mass of BeH}_2 \]
6. **What is your theoretical yield of LiCl in moles?**
\[ \text{Theoretical Yield (moles)} = \text{Moles of Limiting Reagent} \times \frac{\text{Coefficient of LiCl in balanced equation}}{\text{Coefficient of Limiting Reagent}} \]
7. **What is your theoretical yield of LiCl in grams?**
\[ \text{Theoretical Yield (grams)} = \text{Theoretical Yield (moles)} \times \text{Molar Mass of LiCl} \]
Use the molar masses for the calculations:
- BeCl
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