3.0 Outline the steps needed to determine the limiting reactant when 30.0 g of propane, C3H8, is burned with 75.0 g of oxygen. Determine the limiting reactant.
3.0 Outline the steps needed to determine the limiting reactant when 30.0 g of propane, C3H8, is burned with 75.0 g of oxygen. Determine the limiting reactant.
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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Educational Chemistry Problems**
4. **Automotive Air Bags:**
- Calculate the mass of sodium azide required to inflate an airbag when a sample is given at a density of 1.25 g/L.
5. **Yield of Carbon Dioxide:**
- Given a sample of 0.53 g of carbon dioxide. Solve for the percent yield of the reaction:
\[
\text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g)
\]
- Reaction involves decomposing calcium carbonate to produce calcium oxide and carbon dioxide.
6. **Theoretical Yield of HI:**
- In a laboratory experiment, calculate the theoretical yield in grams for the reaction producing HI.
7. **Combustion of Propane:**
- Determine the steps to evaluate which reactant limits the reaction when 30.0 g of propane is burned with 75.0 g of oxygen. Identify the limiting reactant.
8. **Lithium Reactant and Theoretical Yield:**
- Calculate the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine, forming lithium nitride:
\[
\text{Li} + \text{N}_2 \rightarrow \text{Li}_3\text{N}
\]
- Also determine the theoretical yield of the product formed.
9. **Burning Phosphorus in Oxygen:**
- Discuss the process of how phosphorus pentoxide is used to produce phosphoric acid. Calculate the limiting reactant when 2.00 mol of phosphorus and 2.00 mol of oxygen react.
---
**Notes on Handwritten Calculations:**
- The handwritten notes show calculations primarily revolving around molar conversions, stoichiometry, and yield determinations. For example, the conversion of grams to moles and use of molar mass to identify yields from provided reactants.
- There are specific figures noted for percentage yield and theoretical yields calculated with standard chemical equations and conversions highlighted, such as calculating with molecular weights like 44.0096 (probably the molar mass of CO₂).
This content is ideal for students learning about chemical reactions, stoichiometry, limiting reactants, and yield calculations in the context of laboratory settings and practical applications, such as airbags or industrial chemical production.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe33c485d-9ded-4ed9-b52c-b6396698c059%2Fb49130ba-ca84-4b76-897f-1ac3bea44f3f%2Fso5p17f.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Chemistry Problems**
4. **Automotive Air Bags:**
- Calculate the mass of sodium azide required to inflate an airbag when a sample is given at a density of 1.25 g/L.
5. **Yield of Carbon Dioxide:**
- Given a sample of 0.53 g of carbon dioxide. Solve for the percent yield of the reaction:
\[
\text{CaCO}_3 (s) \rightarrow \text{CaO} (s) + \text{CO}_2 (g)
\]
- Reaction involves decomposing calcium carbonate to produce calcium oxide and carbon dioxide.
6. **Theoretical Yield of HI:**
- In a laboratory experiment, calculate the theoretical yield in grams for the reaction producing HI.
7. **Combustion of Propane:**
- Determine the steps to evaluate which reactant limits the reaction when 30.0 g of propane is burned with 75.0 g of oxygen. Identify the limiting reactant.
8. **Lithium Reactant and Theoretical Yield:**
- Calculate the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine, forming lithium nitride:
\[
\text{Li} + \text{N}_2 \rightarrow \text{Li}_3\text{N}
\]
- Also determine the theoretical yield of the product formed.
9. **Burning Phosphorus in Oxygen:**
- Discuss the process of how phosphorus pentoxide is used to produce phosphoric acid. Calculate the limiting reactant when 2.00 mol of phosphorus and 2.00 mol of oxygen react.
---
**Notes on Handwritten Calculations:**
- The handwritten notes show calculations primarily revolving around molar conversions, stoichiometry, and yield determinations. For example, the conversion of grams to moles and use of molar mass to identify yields from provided reactants.
- There are specific figures noted for percentage yield and theoretical yields calculated with standard chemical equations and conversions highlighted, such as calculating with molecular weights like 44.0096 (probably the molar mass of CO₂).
This content is ideal for students learning about chemical reactions, stoichiometry, limiting reactants, and yield calculations in the context of laboratory settings and practical applications, such as airbags or industrial chemical production.
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