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Ch.3 - Molecules and Compounds
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.3 - Molecules and CompoundsProblem 89a
Chapter 3, Problem 89a

Determine the number of moles of hydrogen atoms in each sample. a. 0.0885 mol C4H10 b. 1.3 mol CH4

Verified step by step guidance
1
Step 1: Identify the molecular formula of the compound. In this case, it's C4H10, which means there are 4 atoms of Carbon (C) and 10 atoms of Hydrogen (H) in one molecule of the compound.
Step 2: Understand that a mole of a substance contains Avogadro's number (6.022 x 10^23) of entities (atoms, molecules, etc.). Therefore, one mole of C4H10 contains 10 moles of Hydrogen atoms.
Step 3: Use the given amount of moles of C4H10 to find the moles of Hydrogen atoms. Since one mole of C4H10 contains 10 moles of Hydrogen atoms, multiply the given moles of C4H10 by 10.
Step 4: The result from step 3 will give you the number of moles of Hydrogen atoms in the sample.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Mole Concept

The mole is a fundamental unit in chemistry that quantifies the amount of substance. One mole contains approximately 6.022 x 10^23 entities, such as atoms or molecules. This concept allows chemists to convert between the mass of a substance and the number of particles it contains, facilitating stoichiometric calculations.
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Chemical Formula

A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. For example, C4H10 (butane) consists of 4 carbon (C) atoms and 10 hydrogen (H) atoms. Understanding the chemical formula is essential for determining the number of moles of specific atoms within a compound.
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Stoichiometry

Stoichiometry is the area of chemistry that deals with the relationships between the quantities of reactants and products in chemical reactions. It allows for the calculation of moles of different substances based on their ratios in a balanced equation. In this case, stoichiometry helps determine the number of moles of hydrogen atoms from the given moles of butane.
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