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Chapter 2: Problem 11

Calculate the mass in grams of a mole of atoms of the following elements. (a) \(C\) (b) \(\mathrm{Ni}\) (c) \(\mathrm{Hg}\)

Short Answer

Expert verified
(a) 12.01 g (b) 58.69 g (c) 200.59 g

Step by step solution

01

Understanding Molar Mass

Molar mass is the mass of one mole of a substance (atoms, molecules, etc.) and it is expressed in grams per mole (g/mol). The molar mass of an element can be found on the periodic table.
02

Locate the Molar Mass on the Periodic Table

Locate each element on the periodic table and find its molar mass: - For Carbon ( C ), the molar mass is 12.01 g/mol. - For Nickel ( Ni ), the molar mass is 58.69 g/mol. - For Mercury ( Hg ), the molar mass is 200.59 g/mol.
03

Apply the Molar Mass

Since 1 mole of any of these elements corresponds to its molar mass in grams, you simply take those values: - 1 mole of Carbon ( C ) has a mass of 12.01 g. - 1 mole of Nickel ( Ni ) has a mass of 58.69 g. - 1 mole of Mercury ( Hg ) has a mass of 200.59 g.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

periodic table
The periodic table is a critical tool in chemistry, providing essential information about the elements. Each element is systematically arranged based on its atomic number, electron configuration, and recurring chemical properties. This arrangement also allows us to easily determine the molar mass of elements, which is crucial for various calculations in chemistry.
  • The position of each element on the periodic table gives insights into its physical and chemical properties.
  • The periodic table is divided into periods (rows) and groups (columns) that classify elements with similar characteristics.
  • The molar mass for each element can be found right on the periodic table, expressed in grams per mole (g/mol).
By using the periodic table, chemists can readily find the molar masses of Carbon, Nickel, and Mercury, making it an invaluable resource for solving problems like calculating the mass of one mole of these elements.
mole concept
The mole is a fundamental concept in chemistry that bridges the atomic and macroscopic worlds. It allows chemists to convert between the number of atoms or molecules in a sample and its mass.
The mole concept includes some fundamental ideas:
  • One mole is defined as exactly 6.022 x 1023 entities, whether they be atoms, molecules, or ions. This number is known as Avogadro's number.
  • Using the mole concept, chemists can quantify elements in terms of grams easily. Therefore, one mole of an element has a mass equal to its molar mass in grams.
  • This tool is essential for stoichiometric calculations in chemical reactions, allowing for precise predictions of reactants and products.
By understanding the mole concept, one can easily comprehend the process involved in calculating the mass of 1 mole of Carbon, Nickel, and Mercury: simply looking up their molar masses from the periodic table.
elemental mass calculation
Elemental mass calculation involves using the molar masses of elements to determine the mass of a given amount of the substance. The steps are straightforward once you have a grip on finding the molar mass from the periodic table and understanding the mole concept.
  • Start by identifying the element you are interested in and its molar mass using the periodic table.
  • Apply the equation: Mass = Molar Mass x Number of Moles, where Mass is in grams and Molar Mass is in grams/mole.
  • This calculation is easy when working with one mole, as the mass in grams is identical to the molar mass of the element.
For example, the calculation steps in determining the mass of one mole of Carbon, Nickel, and Mercury rely on simply using their respective molar masses: 12.01 g for Carbon, 58.69 g for Nickel, and 200.59 g for Mercury. This underscores the simplicity and utility of accurate elemental mass calculations in chemistry.

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Most popular questions from this chapter

Calculate the number of moles of nitrogen dioxide, \(\mathrm{NO}_{2},\) that could be prepared from \(0.35 \mathrm{~mol}\) of nitrogen oxide and 0.25 mol of oxygen. $$ 2 \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) $$ Identify the limiting reagent and the excess reagent in the reaction. What would happen to the potential yield of \(\mathrm{NO}_{2}\) if the amount of NO were increased? What if the amount of \(\mathrm{O}_{2}\) were increased?

Calculate the volume of \(0.0985 M\) sulfuric acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{4}\right)\) that would be needed to react with \(10.89 \mathrm{~mL}\) of a \(0.01043 M\) aqueous ammonia \(\left(\mathrm{NH}_{3}\right)\) solution. $$ \mathrm{H}_{2} \mathrm{SO}_{4}(a q)+2 \mathrm{NH}_{3}(a q) \longrightarrow\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}(a q) $$

Calculate the volume of \(0.25 \mathrm{M}\) NaI that would be needed to react with all of the \(\mathrm{Hg}^{2+}\) ion from \(45 \mathrm{~mL}\) of $$ \begin{array}{l} \text { a } 0.10 \mathrm{M} \mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2} \text { solution. } \\ \qquad \begin{array}{l} 2 \mathrm{Nal}(a q)+\mathrm{Hg}\left(\mathrm{NO}_{3}\right)_{2}(a q) \\ \longrightarrow \mathrm{HgI}_{2}(s)+2 \mathrm{NaNO}_{3}(a q) \end{array} \end{array} $$

Calculate the molarity of an acetic acid \(\left(\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}\right)\) solution if \(34.57 \mathrm{~mL}\) of the solution are needed to react with \(25.19 \mathrm{~mL}\) of \(0.1025 \mathrm{M}\) sodium hydroxide. $$ \begin{array}{l} \mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}(a q)+\mathrm{NaOH}(a q) \\ \longrightarrow \mathrm{Na}^{+}(a q)+\mathrm{CH}_{3} \mathrm{CO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \end{array} $$

Calculate the mass of \(\mathrm{CO}_{2}\) produced and the mass of oxygen consumed when 10.0 grams of methane \(\left(\mathrm{CH}_{4}\right)\) are burned in oxygen to produce \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\).
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