Textbook Question
What is meant by the rate of a reaction?
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Ch.7 Chemical Quantities and Reactions
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249
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Table of contents
- Ch.1 Chemistry in Our Lives19
- Ch.2 Chemistry and Measurements80
- Ch.3 Matter and Energy53
- Ch.4 Atoms and Elements58
- Ch.5 Nuclear Chemistry42
- Ch.6 Ionic and Molecular Compounds57
- Ch.7 Chemical Quantities and Reactions38
- Ch.8 Gases30
- Ch.9 Solutions50
- Ch.10 Acids and Bases and Equilibrium64
- Ch.11 Introduction to Organic Chemistry: Hydrocarbons77
- Ch.12 Alcohols, Thiols, Ethers, Aldehydes, and Ketones82
- Ch.13 Carbohydrates54
- Ch.14 Carboxylic Acids, Esters, Amines, and Amides91
- Ch.15 Lipids61
- Ch.16 Amino Acids, Proteins, and Enzymes84
- Ch.17 Nucleic Acids and Protein Synthesis86
- Ch.18 Metabolic Pathways and ATP Production73
Timberlake14thChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9781292472249Not the one you use?Change textbook
Chapter 7, Problem 79c
Using the models of the molecules (black = C, white = H, yellow = S, green = Cl), determine each of the following for models of compounds 1 and 2:
d. number of moles in 10.0 g
Verified step by step guidance1
Step 1: Identify the molecular formulas of the compounds based on the models provided. For compound 1 (top model), the molecule consists of two yellow spheres (sulfur) and one red sphere (oxygen), indicating the formula is likely SO2. For compound 2 (bottom model), the molecule consists of four black spheres (carbon) and eight white spheres (hydrogen), indicating the formula is likely C4H8.
Step 2: Determine the molar mass of each compound. For SO2, calculate the molar mass by summing the atomic masses of sulfur (32.07 g/mol) and oxygen (16.00 g/mol × 2). For C4H8, calculate the molar mass by summing the atomic masses of carbon (12.01 g/mol × 4) and hydrogen (1.008 g/mol × 8).
Step 3: Use the formula for moles: \( \text{moles} = \frac{\text{mass}}{\text{molar mass}} \). Substitute the given mass (10.0 g) and the molar mass calculated for each compound into the formula.
Step 4: Perform the calculation for each compound separately to determine the number of moles in 10.0 g of SO2 and C4H8. Ensure units are consistent (grams for mass and g/mol for molar mass).
Step 5: Interpret the results to understand the number of moles present in 10.0 g of each compound. This will provide insight into the quantity of each substance in terms of moles.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molecular Composition
Molecular composition refers to the types and numbers of atoms that make up a molecule. In the context of the question, understanding the molecular formulas of the compounds represented in the models is essential. For example, the black spheres represent carbon (C), white spheres represent hydrogen (H), yellow represents sulfur (S), and green represents chlorine (Cl). Identifying these components allows for the calculation of moles based on the molecular weight.
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Mole Concept
The mole concept is a fundamental principle in chemistry that relates the mass of a substance to the number of particles it contains. One mole of any substance contains Avogadro's number of entities (approximately 6.022 x 10²³). To determine the number of moles in a given mass (like 10.0 g), one must divide the mass by the molar mass of the substance, which is derived from its molecular composition.
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Molar Mass Calculation
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. For the compounds in the question, determining the molar mass is crucial for calculating the number of moles in 10.0 g. This involves using the periodic table to find the atomic weights of carbon, hydrogen, sulfur, and chlorine, and applying them to the molecular formulas.
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Related Practice
Textbook Question
How would each of the following change the rate of the reaction shown here? 2SO2(g) + O2(g) → 2SO3(g)
a. adding more SO2(g)
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Textbook Question
How would each of the following change the rate of the reaction shown here?
2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
c. removing some H2(g)
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Textbook Question
Using the models of the molecules (black = C, white = H, yellow = S, red = O), determine each of the following for models of compounds 1 and 2:
c. number of moles in 10.0 g
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Textbook Question
Balance each of the following by adding coefficients, and identify the type of reaction for each:
a.
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Textbook Question
If red spheres represent oxygen atoms, blue spheres represent nitrogen atoms, and all the molecules are gases,
a. write the formula for each of the reactants and products.
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