Stoichiometry Mole to Mole Conversions - Molar Ratio Practice Problems

The Organic Chemistry Tutor
15 Jun 201712:11
EducationalLearning
32 Likes 10 Comments

TLDRThis video educates viewers on mole ratios, demonstrating how to balance chemical reactions and solve related problems. It covers examples involving nitrogen and hydrogen gases reacting to form ammonia, propane reacting with oxygen to produce carbon dioxide and water, and ammonia reacting with oxygen to form nitrogen gas and water.

Takeaways
  • 🧪 The video discusses mole ratio and how to solve related problems in chemistry.
  • 🔬 It starts with a balanced chemical reaction: nitrogen gas reacts with hydrogen gas to produce ammonia (NH3).
  • ⚖️ To balance the reaction, 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.
  • 🔄 The mole ratio can be scaled up or down proportionally, for example, 2 moles of nitrogen react with 6 moles of hydrogen to produce 4 moles of ammonia.
  • 🧮 A calculation example shows that 1.5 moles of nitrogen would require 4.5 moles of hydrogen for the reaction.
  • 🔥 Another example involves propane (C3H8) reacting with oxygen gas (O2) to produce carbon dioxide (CO2) and water (H2O).
  • 📝 The balanced equation for this reaction involves 5 moles of oxygen reacting with propane to produce 4 moles of water.
  • 📊 To produce 14 moles of water, 17.5 moles of oxygen are required, as calculated using mole ratios.
  • ⚗️ The video also covers the reaction of ammonia (NH3) with oxygen to produce nitrogen gas (N2) and water, providing the balanced equation and mole ratio.
  • 🔢 It demonstrates how 11 moles of ammonia react completely with 8.25 moles of oxygen and produce 16.5 moles of water.
Q & A

  • What is the balanced chemical equation for the reaction between nitrogen gas and hydrogen gas to produce ammonia?

    -The balanced chemical equation is N2 + 3H2 → 2NH3. This indicates that one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia.

  • What is the mole ratio between nitrogen gas (N2) and hydrogen gas (H2) in the production of ammonia (NH3)?

    -The mole ratio between N2 and H2 is 1:3. This means that for every one mole of N2, three moles of H2 are required to produce ammonia.

  • If you have 1.5 moles of N2, how many moles of H2 will react with it?

    -Using the mole ratio of 1:3, 1.5 moles of N2 will react with 1.5 * 3 = 4.5 moles of H2.

  • What is the balanced chemical equation for the reaction of propane with oxygen gas to produce carbon dioxide and water?

    -The balanced chemical equation is C3H8 + 5O2 → 3CO2 + 4H2O. This shows that one mole of propane reacts with five moles of oxygen gas to produce three moles of carbon dioxide and four moles of water.

  • How many moles of oxygen gas are required to produce 14 moles of water in the reaction involving propane?

    -Using the mole ratio of 5 moles of O2 to 4 moles of H2O, 14 moles of water would require 14 * (5/4) = 17.5 moles of O2.

  • What is the balanced chemical equation for the reaction of ammonia with oxygen gas to produce nitrogen gas and water?

    -The balanced chemical equation is 4NH3 + 3O2 → 2N2 + 6H2O. This indicates that four moles of ammonia react with three moles of oxygen gas to produce two moles of nitrogen gas and six moles of water.

  • How many moles of oxygen gas are required to react completely with 11 moles of ammonia?

    -Using the mole ratio of 4 moles of NH3 to 3 moles of O2, 11 moles of NH3 would require 11 * (3/4) = 8.25 moles of O2.

  • How many moles of water are produced in the reaction of 11 moles of ammonia with oxygen gas?

    -Using the mole ratio of 4 moles of NH3 to 6 moles of H2O, 11 moles of NH3 would produce 11 * (6/4) = 16.5 moles of H2O.

  • Why is it necessary to balance a chemical equation before determining the mole ratios?

    -Balancing a chemical equation ensures that the number of atoms of each element is the same on both sides of the equation, which is essential for accurately determining the mole ratios and the stoichiometry of the reaction.

  • What is the significance of the mole ratio in stoichiometry problems?

    -The mole ratio is crucial in stoichiometry problems as it provides the proportional relationship between the reactants and products in a chemical reaction. It helps in determining the amounts of substances needed or produced in a reaction.

  • Can the mole ratios be altered by multiplying the coefficients in a balanced chemical equation?

    -Yes, the mole ratios can be altered by multiplying the coefficients in a balanced chemical equation. However, the relative ratios between the reactants and products remain the same, which is what is used in stoichiometry calculations.

Outlines
00:00
🧪 Mole Ratio in Chemical Reactions

This paragraph introduces the concept of mole ratio in chemical reactions, using the example of nitrogen gas reacting with hydrogen gas to produce ammonia. The balanced chemical equation is discussed, highlighting the coefficients that represent the mole ratio between the compounds. The paragraph explains that these ratios can be scaled up or down, and a specific example is given where 1.5 moles of nitrogen gas reacts with 4.5 moles of hydrogen gas. Additionally, a problem involving propane reacting with oxygen to produce carbon dioxide and water is presented, with a challenge to determine the moles of oxygen required for 14 moles of water.

05:03
🔍 Calculating Moles of Oxygen for Water Production

This paragraph focuses on solving the problem of determining the moles of oxygen gas required to produce 14 moles of water from propane and oxygen. The balanced chemical equation for the reaction is first established, showing the mole ratio of 5 moles of oxygen to 4 moles of water. The paragraph guides through a step-by-step calculation, using the mole ratio to find that 17.5 moles of oxygen are needed. The explanation includes a methodical approach to scale the ratio and perform the necessary calculations to arrive at the answer.

10:04
🚀 Ammonia Reaction with Oxygen: Mole Ratio Analysis

This paragraph discusses another chemical reaction involving ammonia reacting with oxygen to produce nitrogen gas and water. The paragraph begins by writing and balancing the chemical equation, establishing the mole ratio between ammonia, oxygen, and water. The main focus is on calculating the moles of oxygen required to react completely with 11 moles of ammonia, using the mole ratio of 4 moles of ammonia to 3 moles of oxygen. Additionally, the paragraph calculates the moles of water produced in the process, showing that 11 moles of ammonia yield 16.5 moles of water. The explanation emphasizes the importance of understanding and applying mole ratios in stoichiometry problems.

Mindmap
Keywords
💡Mole Ratio
Mole ratio is a fundamental concept in chemistry that describes the relationship between the amounts of reactants and products in a chemical reaction. It is typically expressed as a ratio of moles. In the video, the mole ratio is used to determine how many moles of one substance will react with another. For example, the script discusses the mole ratio in the reaction between nitrogen gas and hydrogen gas to produce ammonia, which is 1:3 for N2 to H2.
💡Nitrogen Gas
Nitrogen gas (N2) is a diatomic molecule consisting of two nitrogen atoms bonded together. It is a major component of Earth's atmosphere, making up about 78% of the air. In the video, nitrogen gas is a reactant in the reaction with hydrogen gas to form ammonia, illustrating the concept of mole ratio in chemical reactions.
💡Hydrogen Gas
Hydrogen gas (H2) is a diatomic molecule consisting of two hydrogen atoms. It is the most abundant element in the universe and is a key reactant in many chemical processes. In the video, hydrogen gas reacts with nitrogen gas in a balanced chemical equation to produce ammonia, demonstrating the mole ratio of 3:1 for H2 to N2.
💡Ammonia
Ammonia (NH3) is a compound of nitrogen and hydrogen with a characteristic pungent smell. It is a significant compound used in various industrial applications, including the production of fertilizers. In the video, ammonia is the product of the reaction between nitrogen gas and hydrogen gas, and the mole ratio of reactants to ammonia is used to solve stoichiometry problems.
💡Balanced Chemical Equation
A balanced chemical equation is an equation that accurately represents a chemical reaction, with the same number of atoms of each element on both sides of the equation. In the video, the script emphasizes the importance of balancing equations, such as the reaction between propane and oxygen to produce carbon dioxide and water, to determine the correct mole ratios.
💡Propane
Propane (C3H8) is a hydrocarbon gas that is commonly used as a fuel. It is a component of natural gas and is also used in propane-fueled vehicles. In the video, propane is a reactant in a reaction with oxygen gas to produce carbon dioxide and water, illustrating the use of mole ratios in stoichiometry calculations.
💡Oxygen Gas
Oxygen gas (O2) is a diatomic molecule that is essential for life on Earth. It is a major component of the atmosphere and is involved in many biological and chemical processes. In the video, oxygen gas is a reactant in the reactions discussed, such as the combustion of propane and the oxidation of ammonia.
💡Carbon Dioxide
Carbon dioxide (CO2) is a compound consisting of one carbon atom and two oxygen atoms. It is a byproduct of combustion and respiration and is a significant greenhouse gas. In the video, carbon dioxide is a product of the combustion of propane, and the mole ratio is used to calculate the amount of oxygen gas required to produce a certain amount of water.
💡Water
Water (H2O) is a compound of hydrogen and oxygen and is essential for all known forms of life. It is the most abundant substance on Earth. In the video, water is a product of the combustion of propane and is also involved in the reaction with ammonia and oxygen, demonstrating the use of mole ratios in stoichiometry.
💡Stoichiometry
Stoichiometry is the quantitative aspect of chemistry that deals with the relationships between reactants and products in chemical reactions. It involves using balanced chemical equations and mole ratios to determine the amounts of substances involved in reactions. In the video, stoichiometry is the central theme, as it is used to solve problems involving mole ratios and chemical reactions.
💡Conversion Factor
A conversion factor is a ratio used to convert units from one scale to another. In chemistry, it is often used to relate the amounts of reactants and products in a chemical reaction. In the video, conversion factors derived from mole ratios are used to calculate the amounts of substances needed in various reactions, such as the reaction between ammonia and oxygen.
Highlights

Introduction to mole ratio and its significance in solving chemical problems.

Explanation of how to balance the chemical reaction of nitrogen gas and hydrogen gas to produce ammonia.

Illustration of how coefficients in a balanced chemical equation represent the mole ratio between compounds.

Example of how to calculate the moles of hydrogen gas reacting with a given amount of nitrogen gas using mole ratio.

Demonstration of how to adjust mole ratios by multiplying all coefficients to maintain the balance in a chemical equation.

Introduction to the problem of determining the moles of oxygen gas required to produce a certain amount of water from propane.

Step-by-step process of writing and balancing the chemical reaction for propane reacting with oxygen to form carbon dioxide and water.

Use of mole ratio to estimate the moles of oxygen gas needed for a given amount of water production.

Calculation of the exact moles of oxygen gas required to produce 14 moles of water using the balanced chemical equation.

Introduction to the problem of determining the moles of oxygen gas required to react completely with ammonia.

Balancing the chemical reaction of ammonia reacting with oxygen to produce nitrogen gas and water.

Explanation of how to use the mole ratio between ammonia and oxygen to calculate the moles of oxygen gas needed.

Introduction to the problem of calculating the moles of water produced in the reaction of ammonia with oxygen.

Use of the mole ratio between ammonia and water to determine the moles of water produced from a given amount of ammonia.

Final calculation showing that 11 moles of ammonia will produce 16.5 moles of water and react completely with 8.25 moles of oxygen.

Summary of the importance of understanding mole ratios in solving stoichiometry and chemical equilibrium problems.

Transcripts

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Mole RatioChemistryNitrogen GasHydrogen GasAmmoniaReaction BalancePropaneOxygen GasCarbon DioxideWater ProductionStoichiometry