Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question
What is the balanced equation for this reaction (in lowest multiple integers)?
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**H₂(g) + I₂(s) → 2HI(g)**
1. **Mass of HI Produced**
Given an initial mass of 17.8 g H₂, an excess of I₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction.
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
2. **Mass of H₂ Consumed**
Determine the mass (g) of the reactant, H₂, consumed by the reaction.
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
3. **Moles of H₂ Consumed**
The entire mass, 17.8 g, of the reactant H₂ is consumed by the reaction. Calculate the amount (mol) of H₂ in this mass.
**Molar mass = 2.02 g/mol**
**Input:**
- Enter amount in moles (mol): [Input box]
**Action:**
- Submit [Button]
4. **Moles of HI Formed**
Given that 8.8294 mol H₂ was consumed, calculate the amount of HI formed.
**Input:**
- Enter amount in moles (mol): [Input box]
**Action:**
- Submit [Button]
5. **Mass of HI Formed**
Complete consumption of H₂ yields 17.6587 mol of HI. Calculate the mass of this quantity of HI.
**Molar mass = 127.91 g/mol**
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
---
This transcription elaborates on the chemical reaction process, guiding students through calculations involving mass and mole conversions within this specific chemical context.](https://content.bartleby.com/qna-images/question/41533dd6-be05-40da-a627-190380aa1e53/95ddd29b-1043-4154-8640-e5ad14007853/fy82z6k_processed.png)
Transcribed Image Text:---
**H₂(g) + I₂(s) → 2HI(g)**
1. **Mass of HI Produced**
Given an initial mass of 17.8 g H₂, an excess of I₂, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of HI produced by the reaction.
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
2. **Mass of H₂ Consumed**
Determine the mass (g) of the reactant, H₂, consumed by the reaction.
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
3. **Moles of H₂ Consumed**
The entire mass, 17.8 g, of the reactant H₂ is consumed by the reaction. Calculate the amount (mol) of H₂ in this mass.
**Molar mass = 2.02 g/mol**
**Input:**
- Enter amount in moles (mol): [Input box]
**Action:**
- Submit [Button]
4. **Moles of HI Formed**
Given that 8.8294 mol H₂ was consumed, calculate the amount of HI formed.
**Input:**
- Enter amount in moles (mol): [Input box]
**Action:**
- Submit [Button]
5. **Mass of HI Formed**
Complete consumption of H₂ yields 17.6587 mol of HI. Calculate the mass of this quantity of HI.
**Molar mass = 127.91 g/mol**
**Input:**
- Enter mass in grams (g): [Input box]
**Action:**
- Submit [Button]
---
This transcription elaborates on the chemical reaction process, guiding students through calculations involving mass and mole conversions within this specific chemical context.
Transcribed Image Text:**Chemical Reaction Worksheets**
**1. Balancing Chemical Equations:**
- **Reaction:** \( \_\_\_ \text{MnO}_2(s) + \_\_\_ \text{Al}(s) \rightarrow \_\_\_ \text{Mn}(s) + \_\_\_ \text{Al}_2\text{O}_3(s) \)
- *Enter the balanced equation in lowest multiple integers.*
**2. Stoichiometry Calculations:**
a. **Calculating Moles of MnO₂:**
- *Question:* How many moles are present in 53.9 g of MnO₂?
- *Enter moles of MnO₂:*
b. **Mole Ratio Determination:**
- **Reaction:** \( 3 \text{MnO}_2(s) + 4 \text{Al}(s) \rightarrow 3 \text{Mn}(s) + 2 \text{Al}_2\text{O}_3(s) \)
- *Enter the mole ratio of Al to MnO₂:*
c. **Reacting Moles of Al:**
- *Question:* How many moles of Al are required to completely react with 0.620 mol MnO₂?
- *Enter moles of Al:*
d. **Mass of Al Required:**
- *Question:* What is the mass of Al required?
- *Enter mass of Al in grams:*
e. **Formation of Iron(III) Chloride:**
- **Reaction:** \( \text{Fe}(s) + \text{Cl}_2(g) \rightarrow \text{FeCl}_3(s) \)
- *Question:* How many milligrams of iron(III) chloride result when 20.00 mg of iron is reacted with excess chlorine gas?
- *Enter mass in mg of FeCl₃:*
**3. Limiting Reagent Analysis:**
a. **Amount of Acetic Acid Formed:**
- *Question:* What amount of HC₂H₃O₂ can be formed from the amount of each reactant?
- If all of the CH₃CHO was used up in the reaction, how many moles of HC₂H₃O₂ would be produced?
- *Enter moles of HC₂
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