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Questions and Answers
Given the balanced equation N2 + 3H2 → 2NH3, if you start with 0.5 mol of N2, how many moles of NH3 can be produced?
Given the balanced equation N2 + 3H2 → 2NH3, if you start with 0.5 mol of N2, how many moles of NH3 can be produced?
- 2.0 mol
- 1.5 mol
- 0.5 mol
- 1.0 mol (correct)
In the balanced chemical equation N2 + 3H2 → 2NH3, the mole ratio of H2 to NH3 is 3:1.
In the balanced chemical equation N2 + 3H2 → 2NH3, the mole ratio of H2 to NH3 is 3:1.
True (A)
Write the mole ratio of $Al$ to $Al_2O_3$ from this equation: $4Al(s) + 3O_2(g) \rightarrow 2Al_2O_3(s)$
Write the mole ratio of $Al$ to $Al_2O_3$ from this equation: $4Al(s) + 3O_2(g) \rightarrow 2Al_2O_3(s)$
2:1
In the balanced equation N2 + 3H2 → 2NH3, for every mole of N2, ______ moles of H2 are required.
In the balanced equation N2 + 3H2 → 2NH3, for every mole of N2, ______ moles of H2 are required.
Which step is crucial for determining the amount of product formed in a chemical reaction?
Which step is crucial for determining the amount of product formed in a chemical reaction?
Given the balanced chemical equation $4Al(s) + 3O_2(g) \rightarrow 2Al_2O_3(s)$, what is the mole ratio of $O_2$ to $Al_2O_3$?
Given the balanced chemical equation $4Al(s) + 3O_2(g) \rightarrow 2Al_2O_3(s)$, what is the mole ratio of $O_2$ to $Al_2O_3$?
Using the balanced equation $N_2 + 3H_2 \rightarrow 2NH_3$, if 6 moles of $H_2$ are used, how many moles of $NH_3$ will be produced?
Using the balanced equation $N_2 + 3H_2 \rightarrow 2NH_3$, if 6 moles of $H_2$ are used, how many moles of $NH_3$ will be produced?
The coefficients in a balanced chemical equation represent the mass ratio of the reactants and products.
The coefficients in a balanced chemical equation represent the mass ratio of the reactants and products.
In the context of making fish tacos, what does the 'limiting ingredient' primarily determine?
In the context of making fish tacos, what does the 'limiting ingredient' primarily determine?
Excess ingredients affect the maximum yield of a product.
Excess ingredients affect the maximum yield of a product.
Define 'limiting ingredient' in the context of a recipe.
Define 'limiting ingredient' in the context of a recipe.
If you have excess fish, cabbage, cilantro, salsa and lime, but only two tortillas, the ___________ is the limiting ingredient.
If you have excess fish, cabbage, cilantro, salsa and lime, but only two tortillas, the ___________ is the limiting ingredient.
In making sausage sandwiches, if sausages come in packs of 5 and buns come in packs of 8, what is the maximum number of sandwiches you can make with one pack of each?
In making sausage sandwiches, if sausages come in packs of 5 and buns come in packs of 8, what is the maximum number of sandwiches you can make with one pack of each?
The limiting ingredient is always the most expensive ingredient in a recipe.
The limiting ingredient is always the most expensive ingredient in a recipe.
What is the balanced equation for making a sausage sandwich, where S represents sausages and B represents buns?
What is the balanced equation for making a sausage sandwich, where S represents sausages and B represents buns?
What can be inferred if you have excess ingredients after making as many products as possible?
What can be inferred if you have excess ingredients after making as many products as possible?
Which of the following correctly represents the mole ratio needed to convert from moles of a generic substance G to moles of a generic substance W?
Which of the following correctly represents the mole ratio needed to convert from moles of a generic substance G to moles of a generic substance W?
When using the mole-mole flowchart, the coefficients from a balanced chemical equation are used to determine the mole ratios.
When using the mole-mole flowchart, the coefficients from a balanced chemical equation are used to determine the mole ratios.
In the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if 50 moles of $H_2O$ are produced, how many moles of $O_2$ are required?
In the reaction $2H_2 + O_2 \rightarrow 2H_2O$, if 50 moles of $H_2O$ are produced, how many moles of $O_2$ are required?
To ensure proper unit cancellation when applying mole ratios, the units of the 'given' quantity in the numerator should match the units of the same substance in the ______ of the mole ratio.
To ensure proper unit cancellation when applying mole ratios, the units of the 'given' quantity in the numerator should match the units of the same substance in the ______ of the mole ratio.
For the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if you start with 1.20 mol of $N_2$, how many moles of $NH_3$ can be produced, assuming sufficient $H_2$?
For the reaction $N_2 + 3H_2 \rightarrow 2NH_3$, if you start with 1.20 mol of $N_2$, how many moles of $NH_3$ can be produced, assuming sufficient $H_2$?
Which step is essential when using stoichiometry to calculate the amount of a product formed from a given amount of reactant?
Which step is essential when using stoichiometry to calculate the amount of a product formed from a given amount of reactant?
In a chemical reaction, what is the significance of the limiting reagent?
In a chemical reaction, what is the significance of the limiting reagent?
If a reaction has a 1:1 mole ratio between reactant A and product B, and you start with 3 moles of A, how many moles of B can theoretically be produced?
If a reaction has a 1:1 mole ratio between reactant A and product B, and you start with 3 moles of A, how many moles of B can theoretically be produced?
If the amount of $R_2$ calculated is less than the amount of $R_2$ needed, then $R_2$ is the excess reagent.
If the amount of $R_2$ calculated is less than the amount of $R_2$ needed, then $R_2$ is the excess reagent.
If the mole ratio from a balanced equation is $\frac{1 \text{ mol A}}{2 \text{ mol B}}$, then 4 moles of B are required to react completely with 2 moles of A.
If the mole ratio from a balanced equation is $\frac{1 \text{ mol A}}{2 \text{ mol B}}$, then 4 moles of B are required to react completely with 2 moles of A.
Briefly explain how the mole ratio is utilized in determining whether a reactant is limiting or in excess.
Briefly explain how the mole ratio is utilized in determining whether a reactant is limiting or in excess.
The ___________ reagent limits the reaction and is used in a mole-mass calculation with the mole ratio to determine the mass of the product.
The ___________ reagent limits the reaction and is used in a mole-mass calculation with the mole ratio to determine the mass of the product.
In the reaction $aR_1 + bR_2 → cW$, how do you determine the moles of $R_2$ needed for a complete reaction with a given amount of $R_1$?
In the reaction $aR_1 + bR_2 → cW$, how do you determine the moles of $R_2$ needed for a complete reaction with a given amount of $R_1$?
If you are given the masses of reactants $R_1$ and $R_2$, what is the first step in determining which reactant is limiting?
If you are given the masses of reactants $R_1$ and $R_2$, what is the first step in determining which reactant is limiting?
The excess reagent is completely consumed during a chemical reaction.
The excess reagent is completely consumed during a chemical reaction.
Match the following terms with their descriptions in the context of chemical reactions:
Match the following terms with their descriptions in the context of chemical reactions:
In stoichiometric calculations involving gases, what is used to convert from moles to liters?
In stoichiometric calculations involving gases, what is used to convert from moles to liters?
When 2 mol of NO2 are produced for each 1 mol of O2 that reacts, the volume of NO2 should be half the volume of O2.
When 2 mol of NO2 are produced for each 1 mol of O2 that reacts, the volume of NO2 should be half the volume of O2.
What volume of oxygen is required to completely burn 3.86 L of carbon monoxide according to the following reaction: 2CO(g) + O2(g) → 2CO2(g)?
What volume of oxygen is required to completely burn 3.86 L of carbon monoxide according to the following reaction: 2CO(g) + O2(g) → 2CO2(g)?
In stoichiometric problems, _________ can be measured easily for solids and liquids, while __________ can be measured easily for gases.
In stoichiometric problems, _________ can be measured easily for solids and liquids, while __________ can be measured easily for gases.
What does the roadmap for solving stoichiometric problems involving mass-volume calculations use to relate the mass of a solid or liquid reactant to the volume of a gaseous product?
What does the roadmap for solving stoichiometric problems involving mass-volume calculations use to relate the mass of a solid or liquid reactant to the volume of a gaseous product?
In the context of stoichiometric calculations, what is the primary purpose of the 'mole ratio' step?
In the context of stoichiometric calculations, what is the primary purpose of the 'mole ratio' step?
When solving stoichiometric problems, it is generally unnecessary to evaluate if the result makes sense in the context of the chemical reaction.
When solving stoichiometric problems, it is generally unnecessary to evaluate if the result makes sense in the context of the chemical reaction.
Match each step in solving stoichiometric problems with its description:
Match each step in solving stoichiometric problems with its description:
In a chemical reaction, what primarily determines the amount of product that can be formed?
In a chemical reaction, what primarily determines the amount of product that can be formed?
The excess reagent is completely used up in a chemical reaction.
The excess reagent is completely used up in a chemical reaction.
What happens to a reaction once the limiting reagent is used up?
What happens to a reaction once the limiting reagent is used up?
In the balanced reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$, if you start with 1 mole of $N_2$ and 4 moles of $H_2$, the ______ is the limiting reagent.
In the balanced reaction $N_2(g) + 3H_2(g) \rightarrow 2NH_3(g)$, if you start with 1 mole of $N_2$ and 4 moles of $H_2$, the ______ is the limiting reagent.
Match each scenario to the reagent that is most likely the limiting reagent:
Match each scenario to the reagent that is most likely the limiting reagent:
Consider a scenario where 2 moles of $N_2$ react with 5 moles of $H_2$ to produce $NH_3$. Which of the following statements is correct?
Consider a scenario where 2 moles of $N_2$ react with 5 moles of $H_2$ to produce $NH_3$. Which of the following statements is correct?
A chemist mixes 2.0 mol of $H_2$ with 1.0 mol of $O_2$ which react according to the equation: $2H_2 + O_2 \rightarrow 2H_2O$. What is the limiting reactant?
A chemist mixes 2.0 mol of $H_2$ with 1.0 mol of $O_2$ which react according to the equation: $2H_2 + O_2 \rightarrow 2H_2O$. What is the limiting reactant?
If 4.0g of $H_2$ is allowed to react with 14.0g of $N_2$, producing 16.4g of $NH_3$, determine the theoretical yield of ammonia in grams.
If 4.0g of $H_2$ is allowed to react with 14.0g of $N_2$, producing 16.4g of $NH_3$, determine the theoretical yield of ammonia in grams.
Flashcards
Chemical Equation Format
Chemical Equation Format
aR1 + bR2 → cW represents a chemical reaction
Mass to Moles Conversion
Mass to Moles Conversion
Using the mass of a reactant to find the moles.
Given Quantities
Given Quantities
The experimentally available amount of each reactant is known.
Mole Ratio
Mole Ratio
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Limiting Reagent
Limiting Reagent
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Excess Reagent
Excess Reagent
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Determining Limiting Reagent
Determining Limiting Reagent
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Mass from Limiting Reagent
Mass from Limiting Reagent
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Balanced Reactants
Balanced Reactants
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Unbalanced Reactants
Unbalanced Reactants
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Balanced Chemical Equation
Balanced Chemical Equation
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Theoretical Yield
Theoretical Yield
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Actual Yield
Actual Yield
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Percent Yield
Percent Yield
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Limiting Ingredient
Limiting Ingredient
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Excess Ingredients
Excess Ingredients
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Taco Production
Taco Production
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Reactant Amounts
Reactant Amounts
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Balanced Equation
Balanced Equation
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Sausage Sandwich Production
Sausage Sandwich Production
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Sausage Sandwich Limiting Ingredient
Sausage Sandwich Limiting Ingredient
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Sausage Sandwich Excess Ingredient
Sausage Sandwich Excess Ingredient
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Balanced Equation Importance
Balanced Equation Importance
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What is a Mole Ratio?
What is a Mole Ratio?
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Using Mole Ratio
Using Mole Ratio
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N2 to NH3 Mole Ratio
N2 to NH3 Mole Ratio
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What does 'Calculate' mean?
What does 'Calculate' mean?
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Calculating Moles of NH3
Calculating Moles of NH3
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What does 'Evaluate' mean?
What does 'Evaluate' mean?
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4Al(s) + 3O2(g) → 2Al2O3(s)
4Al(s) + 3O2(g) → 2Al2O3(s)
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Mole-Mole Conversion
Mole-Mole Conversion
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Mole-Mole Flowchart
Mole-Mole Flowchart
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Balanced Equation Example
Balanced Equation Example
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Applying Mole Ratio
Applying Mole Ratio
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O2 required to produce 25 mol of H2O
O2 required to produce 25 mol of H2O
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H2 required to produce 25 mol of H2O
H2 required to produce 25 mol of H2O
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Calculating Moles of Product
Calculating Moles of Product
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Molar Volume
Molar Volume
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Evaluate the Result
Evaluate the Result
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CO Combustion Equation
CO Combustion Equation
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Measuring Reactants
Measuring Reactants
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Stoichiometry Roadmap
Stoichiometry Roadmap
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Mass-Volume Calculations
Mass-Volume Calculations
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Mass-Volume Process
Mass-Volume Process
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Study Notes
- Mole ratios are conversion factors from balanced chemical equations in terms of moles.
- Mole ratios convert between moles of a given reactant/product and moles of a different reactant/product.
- Mole ratios are determined from balanced chemical equations.
- For the ammonia production equation, N2(g) + 3H2(g) → 2NH3(g), mole ratios can be determined.
Mole-Mole Graph
- The graph displays NH3 moles versus N2 and H2 moles.
- Coefficients in chemical equations show proportionality between reactants/products.
- The mole ratio can also be used to compute the ratio between any reactants and/or products.
- Slope for NH3 vs N2 line is 2 mol NH3 / 1 mol N2.
- Slope for NH3 vs H2 line is 2 mol NH3 / 3 mol H2.
Mole-Mole Calculations
- Mole ratios facilitate mole-mole conversions between reactants/products.
- For a given number of moles (G), the mole ratio calculates the moles of the wanted substance (W).
- Choose the right mole ratio ensuring the moles of the wanted substance are in the numerator.
- To apply the mole-mole flowchart multiply the moles given by the right mole ratio.
Applying the Mole-Mole Flowchart
- To produce 25 mol H2O, the process involves using the balanced equation 2H2 + O2 → 2H2O.
- Use coefficients to derive mole ratios including H2O and O2.
- Select the ratio enabling mol H2O cancellation.
- 25 mol H2O x (1 mol O2 / 2 mol H2O) = 12.5 mol O2
Calculating Moles of a Product
- To analyze, list knowns and unknowns, then solve
- For the balanced chemical equation for the formation of ammonia.
- You must cancel mol N2 in the known.
- Multiply the given mol N2 by the mole ration in order to find the moles of NH3, as the final step.
- As a result, if 0.60 mol of nitrogen reacts with hydrogen, 1.2 mol of ammonia is produced.
Calculating the Mass of Product
- The mass-mass calculation converts mass from one reactant/product to another.
- First, convert the mass of the given component to moles using molar mass.
- Then, use the mole ratio to find the number of moles in the wanted component.
- Finally, convert moles of the wanted component into mass using its molar mass.
- Mass ratio for ammonia reaction is approximately 1.21 NH3:1 N2.
Calculating Volume of a Product
- Volume-volume calculation convert between volumes of reactants/products.
- Only gases at STP (standard temperature and pressure) can use this specific volume-volume calculations.
- Convert the volume of the known component into moles with molar volume, this is the first stpe.
- Then, use the mole ration in order to determine what are the moles of the component you want to find.
- To finish, convert moles of the component you the molar volume.
A Roadmap for Solving Stoichiometric Problems
- Mass measurement is easiest for solids/liquids.
- Volume measurement is easiest for gases.
- Mass-volume calculations apply to both combinations of solids and gases.
Limiting Ingredients
- In recipes, insufficient ingredient amounts limit product formed from the limiting ingredient.
Limiting and Excess Reagents
- The limiting reagent in chemical equations restricts product amount.
- The reaction ceases upon depletion of this reagent, leaving other reactants as excess reagents.
- Balanced chemical equation: N₂(g) + 3H2(g) → 2NH3(g)
- Any reactant not fully used is the excess reagent.
Mass of Products and Reactants
- Quantities in stoichiometric problems need conversion to moles.
- Mole ratio application determines the limiting reagent using the mass to moles conversion.
- The limiting reagent is used next to determine the final mass of products or reactants.
Percent Yield
- Percent yield compares actual yield to theoretical yield of a reaction.
- Actual yield: product amount from the reaction.
- Theoretical yield: maximum product amount from calculation.
- Percent Yield = (actual yield / theoretical yield) x 100
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Description
Learn about mole ratios as conversion factors derived from balanced chemical equations. Explore mole-mole graphs and calculations to understand the quantitative relationships in chemical reactions. Understand how coefficients in equations indicate proportionality between reactants and products and how to perform mole-mole conversions.
