Combustion of Methane Quiz

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Questions and Answers

How much oxygen is needed to react with 1.20 mol of CH₄?

  • 64.0 g
  • 2.40 mol
  • 1.20 mol (correct)
  • 76.8 g

In a reaction involving CH₄ and O₂, which reactant is considered limiting?

  • O₂ (correct)
  • CO₂
  • H₂O
  • CH₄

If 16.0 g of CH₄ reacts with 48.0 g of O₂, what is the mass of CO₂ produced?

  • 22.0 g
  • 16.0 g
  • 33.0 g (correct)
  • 44.0 g

What is the mole ratio of CH₄ to O₂ in the balanced reaction?

<p>1:2 (B)</p> Signup and view all the answers

What is the molar mass of O₂ used for calculations in the examples?

<p>32.0 g/mol (A)</p> Signup and view all the answers

In the combustion of methane, which molecule is produced in the greatest quantity?

<p>Water (H₂O) (D)</p> Signup and view all the answers

What is indicated by the coefficients in a balanced chemical equation?

<p>The proportions of reactants and products (A)</p> Signup and view all the answers

In the given equation CH₄ + 2O₂ → CO₂ + 2H₂O, how many total molecules of reactants are present?

<p>4 (D)</p> Signup and view all the answers

What role do the substances to the left of the reaction arrow play in a chemical equation?

<p>They are the reactants participating in the reaction. (C)</p> Signup and view all the answers

Which of the following best describes the products in the reaction CH₄ + 2O₂ → CO₂ + 2H₂O?

<p>They are created from the reactants after the reaction has occurred. (B)</p> Signup and view all the answers

How many O₂ molecules are required to react with 25 CH₄ molecules?

<p>50 O₂ molecules (A)</p> Signup and view all the answers

If 4 moles of CH₄ react, how many moles of CO₂ are produced?

<p>4 moles of CO₂ (B)</p> Signup and view all the answers

What is the total mass of products formed from 32.0 g of O₂ reacting with an excess of CH₄?

<p>80.0 g (C)</p> Signup and view all the answers

What is the molar mass of methane (CH₄)?

<p>16.0 g/mol (C)</p> Signup and view all the answers

According to the balanced equation, how many moles of H₂O are produced from 5 moles of CH₄?

<p>10 moles (C)</p> Signup and view all the answers

What is the limiting reactant in the reaction between CH₄ and O₂ based on the given mass?

<p>O₂ (A)</p> Signup and view all the answers

How many moles of CO₂ are produced from 1.50 moles of O₂?

<p>0.750 moles (D)</p> Signup and view all the answers

What is the mass of CO₂ produced from 0.750 moles of CO₂?

<p>33.0 g (B)</p> Signup and view all the answers

What is the ratio of reactants needed to produce 1 mole of Ni(OH)₂ based on the balanced equation?

<p>1:2 (D)</p> Signup and view all the answers

If you have more NiCl₂ than NaOH, which reactant determines the amount of Ni(OH)₂ produced?

<p>NaOH (C)</p> Signup and view all the answers

What is the purpose of using the smallest whole-number coefficients in a balanced chemical equation?

<p>To follow the law of conservation of mass (A), To accurately represent the actual quantities in the reaction (B)</p> Signup and view all the answers

Why can subscripts in chemical formulas not be changed when balancing equations?

<p>Changing subscripts alters the identity of the compound (A)</p> Signup and view all the answers

In the balanced equation C₂H₆O + 3O₂ → 2CO₂ + 3H₂O, how many total moles of products are produced?

<p>5 (B)</p> Signup and view all the answers

What does the law of conservation of matter imply about a balanced chemical equation?

<p>The total number of each type of atom must be equal on both sides (A)</p> Signup and view all the answers

What is represented by the equation C₂H₆O + O₂ → CO₂ + H₂O before balancing?

<p>An unbalanced chemical reaction (D)</p> Signup and view all the answers

What is the calculated amount of Ni(OH)₂ formed when 0.250 moles of NaOH are used?

<p>0.125 moles (D)</p> Signup and view all the answers

What mass of NiCl₂ was used in the reaction calculations?

<p>129.6 g (B)</p> Signup and view all the answers

Identify the limiting reactant in the given reaction.

<p>NaOH (D)</p> Signup and view all the answers

What is the theoretical yield of Ni(OH)₂ in grams?

<p>11.6 g (C)</p> Signup and view all the answers

What is the theoretical yield of Nitrobenzene from the given amount of Benzene?

<p>24.6 grams (B)</p> Signup and view all the answers

Which factor is NOT a reason for a lower actual yield compared to the theoretical yield?

<p>Using excessive amounts of reactants (A)</p> Signup and view all the answers

What percent yield was achieved in the experiment?

<p>73.2% (A)</p> Signup and view all the answers

Which step is NOT involved in calculating the theoretical yield of Nitrobenzene?

<p>Determine the actual yield from an experimental setup (A)</p> Signup and view all the answers

What is the molar mass of Benzene used in the calculation?

<p>78.1 g/mol (C)</p> Signup and view all the answers

What assumption is made when calculating the percent yield in this reaction?

<p>Side reactions do not occur (B)</p> Signup and view all the answers

Flashcards

Conservation of Matter

In a chemical reaction, the total mass of the reactants equals the total mass of the products.

Balanced Equation

A chemical equation with the same number of atoms of each element on both sides.

Mole Ratio

The ratio of moles of one substance to moles of another in a balanced chemical equation.

Limiting Reactant

The reactant that is completely used up in a chemical reaction, thus limiting the amount of product formed.

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Excess Reactant

The reactant that is not completely used up in a chemical reaction.

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Mass of Oxygen

The mass in grams of oxygen required for a reaction.

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Mass of Product

The mass in grams of a substance produced in a chemical reaction.

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Chemical Equation

A representation of a chemical reaction showing reactants and products and their relative amounts.

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Reactants

The substances that are consumed during a chemical reaction.

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Products

The substances that are formed during a chemical reaction.

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Chemical Reaction

A process where one or more substances are transformed into different substances.

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Combustion of Methane

The chemical reaction of methane (CH4) with oxygen, producing carbon dioxide and water.

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Balanced Chemical Equation

A chemical equation where the number of atoms of each element in the reactants equals the number of atoms of that element in the products.

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Limiting Reactant

The reactant that is completely used up in a chemical reaction, limiting the amount of product formed.

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Balanced Equation

A chemical equation with the same number of atoms of each element on both sides.

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Calculate Moles

Converting a mass of a substance into the number of moles using its molar mass.

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Molar Mass (Example)

The mass in grams of one mole of a substance.

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Mole Ratio

Ratio of moles of reactants and products in a balanced equation.

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Mass of CO₂ (Problem 1)

Determining the mass of carbon dioxide (CO₂) produced in a reaction given the mass of reactants (CH₄ and O₂).

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Limiting Reactant Identification (Problem 1)

Determining which reactant is completely consumed in a chemical reaction with given masses of reactants

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Mole Ratio in Equation

The ratio of moles of substances according to a balanced chemical equation.

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Balanced Chemical Equation

A chemical equation where the quantities of each element are equal on both sides of the equation.

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Conservation of Matter

The principle that matter is neither created nor destroyed in a chemical reaction.

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Calculate O₂ for CH₄

Determine how many O₂ molecules react with a given amount of CH₄ according to a balanced equation.

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Calculate H₂O from CH₄

Find the moles of water produced from a known amount of methane (CH₄), assuming sufficient oxygen.

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Chemical Formula

A symbolic representation of a substance showing the elements and their ratios.

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Subscripts in Formulas

These numbers tell you how many atoms of each element are in a molecule.

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Molar Mass - CH₄

Mass of one mole of methane (CH₄).

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Molar Mass - O₂

Mass of one mole of oxygen (O₂)

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Coefficients

Numbers before the formula that tell you the moles/number of molecules of each substance involved in the reaction.

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Balancing Chemical Equation

Adjusting the coefficients of a reaction to equal the number of atoms of each element in reactants and products.

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Molar Mass - CO₂

Mass of one mole of carbon dioxide (CO₂)

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Molar Mass - H₂O

Mass of one mole of water (H₂O).

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Law of Conservation of Mass

Total mass of reactants equals the total mass of products in a chemical reaction.

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Limiting Reactant

The reactant that is completely used up in a chemical reaction, determining the maximum amount of product that can be formed.

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Theoretical Yield

The maximum amount of product that can be produced in a chemical reaction, assuming all the limiting reactant reacts.

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Moles of Reactant

The amount of a substance (reactant) expressed in moles, reflecting the quantity of individual atoms in the reactant.

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Balanced Chemical Equation

An equation where the number of atoms of each element is equal on both sides of the equation, reflecting conservation of mass.

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Moles of Product

The amount of the product formed in a reaction, expressed in moles(mol).

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Percent Yield

The ratio of actual yield to theoretical yield, often expressed as a percentage.

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Actual Yield

The amount of product produced in a reaction in real-world conditions.

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Incomplete Reaction

A reaction where the reactants fail to convert to expected products entirely.

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Percent Yield

The percentage of the desired product obtained compared to the maximum possible yield.

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Actual Yield

The amount of product actually obtained in a reaction.

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Theoretical Yield

The maximum amount of product possible based on the amount of reactants.

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Molar Ratio

The ratio of moles of one substance to moles of another in a balanced equation.

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Balanced Chemical Equation

An equation showing the reactants & products with the same number of each atom on both sides.

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Calculation of Theoretical Yield

Finding the maximum product from given reactant amounts following the balanced chemical equation.

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Calculating Percent Yield

Comparing actual yield to theoretical yield expressed as a percentage.

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Nitrobenzene

An organic compound produced from benzene and Nitric acid.

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Benzene

A hydrocarbon used in the chemical reaction process.

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Study Notes

Chemical Equations and Reaction Stoichiometry

  • Chemical reactions involve changing one or more substances into one or more different substances.
  • Chemical equations are used to describe chemical reactions, showing reactants and products.
  • Reactants are written to the left of an arrow, and products to the right.
  • The relative amounts of reactants and products are shown by the coefficients in the equation.
  • A balanced chemical equation has the same number of each kind of atom on both sides of the equation..
  • Coefficients in chemical equations represent the number of moles of substances.
  • In real-world situations, reactions may not proceed to completion, this could be due to multiple reasons:
    • Some reactions do not proceed to completion because the reactants are not completely converted to products.
    • Multiple reactions are occurring simultaneously
    • Products are difficult to isolate from the reaction mixture.

Limiting Reactants

  • The limiting reactant is the reactant that is completely used up first in a reaction.
  • The limiting reactant determines the amount of product that can be formed.
  • Calculations are often based on the limiting reactant to evaluate the maximum product formed.

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