Textbook Question
Balance the following equation, and tell how many moles of nickel will react with 9.81 mol of hydrochloric acid.
Ni(s) + HCl(aq) → NiCl2(aq) + H2(g)
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Ch.6 Chemical Reactions: Mole and Mass Relationships
McMurry8th EditionFundamentals of GOBISBN: 9780134015187
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Table of contents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
Chapter 6, Problem 6
Which weighs more, 5.00 g or 0.0225 mol of acetaminophen (C8H9O2)?
Verified step by step guidance1
Step 1: Calculate the molar mass of acetaminophen (C8H9O2). Add the atomic masses of all the atoms in the molecular formula: (8 × atomic mass of C) + (9 × atomic mass of H) + (2 × atomic mass of O). Use the periodic table to find the atomic masses of C, H, and O.
Step 2: Multiply the molar mass of acetaminophen by the given number of moles (0.0225 mol) to find the mass of 0.0225 mol of acetaminophen. Use the formula: mass = moles × molar mass.
Step 3: Compare the calculated mass of 0.0225 mol of acetaminophen to the given mass of 5.00 g. Determine which value is greater.
Step 4: Conclude which quantity weighs more based on the comparison in Step 3.
Step 5: Ensure all units are consistent and properly labeled throughout the calculations to avoid errors.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). For acetaminophen (C8H9O2), the molar mass can be calculated by summing the atomic masses of its constituent elements: carbon (C), hydrogen (H), and oxygen (O). This value is essential for converting between grams and moles, allowing us to determine the weight of a given amount of substance.
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01:10
Calculating Molar Mass
Conversion Between Grams and Moles
To compare weights in grams and moles, one must convert moles to grams using the molar mass. The formula used is: mass (g) = number of moles × molar mass (g/mol). This conversion is crucial for answering the question, as it allows for a direct comparison between the given weight of 5.00 g and the weight of 0.0225 mol of acetaminophen.
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01:29Mole Concept
Comparative Weight Analysis
Comparative weight analysis involves evaluating two or more quantities to determine which is greater. In this context, after converting 0.0225 mol of acetaminophen to grams using its molar mass, one can directly compare the resulting weight to the fixed weight of 5.00 g. This analysis is fundamental to answering the question accurately.
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Related Practice
Textbook Question
How many moles of NiCl2 can be formed in the reaction of 6.00 mol of Ni and 12.0 mol of HCl?
Ni(s) + HCl(aq) → NiCl2(aq) + H2(g)
1650
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Textbook Question
The reaction of ethylene oxide with water to give ethylene glycol (automobile antifreeze) occurs in 96.0% actual yield. How many grams of ethylene glycol are formed by reaction of 35.0 g of ethylene oxide? (For ethylene oxide, MW = 44.0 amu; for ethylene glycol, MW = 62.0 amu.)
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