Ch.3 - Chemical Reactions and Reaction Stoichiometry

Problem 32

Chapter 3, Problem 32

Without doing any detailed calculations (but using a periodic table to give atomic weights), rank the following samples in order of increasing numbers of atoms: 42 g of NaHCO3,1.5molCO2,6.0×1024 Ne atoms.

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Identify the number of atoms in each sample: NaHCO3, CO2, and Ne.

For NaHCO3, calculate the molar mass using the atomic weights from the periodic table: Na (22.99 g/mol), H (1.01 g/mol), C (12.01 g/mol), O (16.00 g/mol).

Determine the number of moles of NaHCO3 by dividing the given mass (42 g) by its molar mass.

Calculate the total number of atoms in NaHCO3 by multiplying the number of moles by Avogadro's number (6.022 x 10^23 atoms/mol) and the number of atoms per formula unit (6 atoms: 1 Na, 1 H, 1 C, 3 O).

Compare the number of atoms in each sample: 42 g of NaHCO3, 1.5 mol of CO2 (3 atoms per molecule), and 6.0 x 10^24 Ne atoms, and rank them in order of increasing number of atoms.

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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). It is calculated by summing the atomic weights of all the atoms in a molecule. For example, sodium bicarbonate (NaHCO3) has a molar mass of approximately 84 g/mol, which is essential for determining the number of moles in a given mass.

Avogadro's Number

Avogadro's number, approximately 6.022 x 10^23, is the number of atoms, ions, or molecules in one mole of a substance. This constant allows chemists to convert between moles and the number of individual particles. For instance, knowing the number of moles of CO2 can help determine the total number of CO2 molecules present in a sample.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the conservation of mass. It involves using molar ratios derived from balanced chemical equations to relate quantities of different substances. In this context, stoichiometry helps compare the number of atoms in different samples by converting masses or moles into a common unit.

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