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Ch.6 Chemical Reactions: Mole and Mass Relationships
McMurry - Fundamentals of General, Organic, and Biological Chemistry 8th Edition
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.6 Chemical Reactions: Mole and Mass RelationshipsProblema 57b
Capitolo 6, Problema 57b

When table sugar (sucrose, C12H22O11) is heated, it decomposes to form C and H2O.
b. How many grams of carbon are formed by the breakdown of 60.0 g of sucrose?

Guida verificata passo dopo passo
1
Step 1: Write the balanced chemical equation for the decomposition of sucrose (C₁₂H₂₂O₁₁) into carbon (C) and water (H₂O). The equation is: C₁₂H₂₂O₁₁ → 12C + 11H₂O.
Step 2: Calculate the molar mass of sucrose (C₁₂H₂₂O₁₁) by summing the atomic masses of its elements: (12 × atomic mass of C) + (22 × atomic mass of H) + (11 × atomic mass of O). Use the periodic table to find the atomic masses: C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol.
Step 3: Determine the number of moles of sucrose in 60.0 g by using the formula: \( \text{moles of sucrose} = \frac{\text{mass of sucrose}}{\text{molar mass of sucrose}} \).
Step 4: Use the stoichiometry of the balanced equation to find the moles of carbon produced. From the equation, 1 mole of sucrose produces 12 moles of carbon. Multiply the moles of sucrose by this ratio: \( \text{moles of carbon} = \text{moles of sucrose} \times 12 \).
Step 5: Convert the moles of carbon to grams using the molar mass of carbon (12.01 g/mol). Use the formula: \( \text{mass of carbon} = \text{moles of carbon} \times \text{molar mass of carbon} \).

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Chemical Decomposition

Chemical decomposition is a reaction where a single compound breaks down into two or more simpler substances. In this case, sucrose (C12H22O11) decomposes when heated, resulting in carbon (C) and water (H2O). Understanding this process is crucial for calculating the products formed from a given amount of the reactant.
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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using balanced chemical equations to determine the proportions of substances involved. For the decomposition of sucrose, stoichiometry allows us to calculate how much carbon is produced from a specific mass of sucrose.
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Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is essential for converting between grams and moles in chemical calculations. For sucrose and carbon, knowing their molar masses enables the determination of how many grams of carbon can be obtained from the decomposition of a given mass of sucrose.
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Nitrobenzene (C6H5NO2) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C6H6) with nitric acid:

C6H6(l) + HNO3(aq) → C6H5NO2(l) + H2O(l)

b. Calculate the theoretical yield for this reaction.

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Although Cu is not sufficiently active to react with acids, it can be dissolved by concentrated nitric acid, which functions as an oxidizing agent according to the following equation:

Cu(s) + 4 HNO3(aq) → Cu(NO3)2(aq) + 2 NO2(g) + 2 H2O(l)

b. Is 35.0 g of HNO3 sufficient to dissolve 5.00 g of copper?

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Nitrobenzene (C6H5NO2) is used in small quantities as a flavoring agent or in perfumes but can be toxic in large amounts. It is produced by reaction of benzene (C6H6) with nitric acid:

C6H6(l) + HNO3(aq) → C6H5NO2(l) + H2O(l)

a. Identify the limiting reagent in the reaction of 27.5 g of nitric acid with 75 g of benzene.

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When table sugar (sucrose, C12H22O11) is heated, it decomposes to form C and H2O.

a. Write a balanced equation for the process.

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Ethyl alcohol is formed by enzyme action on sugars and starches during fermentation.

C6H12O6 → 2 CO2 + 2 C2H6O

If the density of ethyl alcohol is 0.789 g/mL, how many quarts can be produced by the fermentation of 100.0 lb of sugar?

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Acetylsalicylic acid, the active ingredient in aspirin, is prepared from salicylic acid by reaction with acetic anhydride.

C7H6O3 (salicylic acid) + C4H6O3 (acetic anhydride) → C9H8O4 (acetylsalicylic acid) + C2H4O2 (acetic acid)

a. Calculate the theoretical yield if 47 g of salicylic acid is reacted with 25 g of acetic anhydride.

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