If you have 2.32 grams of BeCl, and 0.90 grams of LiH and make .19 grams of BeH, and .92 grams of LiCl. a. How many moles of BeCl, do you have? b. How many moles of LiH do you have? c. What is your limiting reagent?
If you have 2.32 grams of BeCl, and 0.90 grams of LiH and make .19 grams of BeH, and .92 grams of LiCl. a. How many moles of BeCl, do you have? b. How many moles of LiH do you have? c. What is your limiting reagent?
Chemistry
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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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![**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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19c732c8-efee-414f-84d3-ed7ea6f7d2e9%2F38fcc1d4-9423-464d-b28b-2e5936f26d5d%2F0nfl4xa_processed.jpeg&w=3840&q=75)
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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