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1. 10.2 Mass And The Mole Study Guide Answers

1. Mar 8, 2017 - The molar mass of a substance is the mass of one mole of the substance. This collection of ten chemistry test questions deals with calculating it. The answers appear after the final question. Continue Reading.
2. Answer to: 4.00 moles of sodium have a mass of By signing up, you'll get thousands of step-by-step solutions to your homework questions.

Learning Objectives By the end of this section, you will be able to:. Calculate formula masses for covalent and ionic compounds. Define the amount unit mole and the related quantity Avogadro’s number Explain the relation between mass, moles, and numbers of atoms or molecules, and perform calculations deriving these quantities from one another We can argue that modern chemical science began when scientists started exploring the quantitative as well as the qualitative aspects of chemistry. For example, Dalton’s atomic theory was an attempt to explain the results of measurements that allowed him to calculate the relative masses of elements combined in various compounds.

Understanding the relationship between the masses of atoms and the chemical formulas of compounds allows us to quantitatively describe the composition of substances. Formula Mass In an earlier chapter, we described the development of the atomic mass unit, the concept of average atomic masses, and the use of chemical formulas to represent the elemental makeup of substances. These ideas can be extended to calculate the formula mass of a substance by summing the average atomic masses of all the atoms represented in the substance’s formula. Formula Mass for Covalent Substances For covalent substances, the formula represents the numbers and types of atoms composing a single molecule of the substance; therefore, the formula mass may be correctly referred to as a molecular mass. Consider chloroform (CHCl 3), a covalent compound once used as a surgical anesthetic and now primarily used in the production of the “anti-stick” polymer, Teflon. The molecular formula of chloroform indicates that a single molecule contains one carbon atom, one hydrogen atom, and three chlorine atoms.

There are 6.02 x 10 23 atoms in a mole of an element or 6.02 x 10 23 molecules in a compound. 6.02 x 10 23 is known as Avogadro's number. Answer and Explanation: 4.00 moles of sodium has a mass of 91.96 grams. To find an element's molar mass, you can use its atomic weight. Sodium's molar mass is 22.99 g/mole.

The average molecular mass of a chloroform molecule is therefore equal to the sum of the average atomic masses of these atoms. Outlines the calculations used to derive the molecular mass of chloroform, which is 119.37 amu. Example 1 Computing Molecular Mass for a Covalent Compound Ibuprofen, C 13H 18O 2, is a covalent compound and the active ingredient in several popular nonprescription pain medications, such as Advil and Motrin. What is the molecular mass (amu) for this compound? Solution Molecules of this compound are comprised of 13 carbon atoms, 18 hydrogen atoms, and 2 oxygen atoms. Following the approach described above, the average molecular mass for this compound is therefore: Check Your Learning Acetaminophen, C 8H 9NO 2, is a covalent compound and the active ingredient in several popular nonprescription pain medications, such as Tylenol. What is the molecular mass (amu) for this compound?

10.2 Mass And The Mole Study Guide Answers

Answer: 151.16 amu Formula Mass for Ionic Compounds Ionic compounds are composed of discrete cations and anions combined in ratios to yield electrically neutral bulk matter. The formula mass for an ionic compound is calculated in the same way as the formula mass for covalent compounds: by summing the average atomic masses of all the atoms in the compound’s formula. Keep in mind, however, that the formula for an ionic compound does not represent the composition of a discrete molecule, so it may not correctly be referred to as the “molecular mass.” As an example, consider sodium chloride, NaCl, the chemical name for common table salt. Sodium chloride is an ionic compound composed of sodium cations, Na +, and chloride anions, Cl −, combined in a 1:1 ratio. The formula mass for this compound is computed as 58.44 amu (see ).

Table salt, NaCl, contains an array of sodium and chloride ions combined in a 1:1 ratio. Its formula mass is 58.44 amu. Note that the average masses of neutral sodium and chlorine atoms were used in this computation, rather than the masses for sodium cations and chlorine anions.

This approach is perfectly acceptable when computing the formula mass of an ionic compound. Even though a sodium cation has a slightly smaller mass than a sodium atom (since it is missing an electron), this difference will be offset by the fact that a chloride anion is slightly more massive than a chloride atom (due to the extra electron). Moreover, the mass of an electron is negligibly small with respect to the mass of a typical atom. Even when calculating the mass of an isolated ion, the missing or additional electrons can generally be ignored, since their contribution to the overall mass is negligible, reflected only in the nonsignificant digits that will be lost when the computed mass is properly rounded.

The few exceptions to this guideline are very light ions derived from elements with precisely known atomic masses. Example 2 Computing Formula Mass for an Ionic Compound Aluminum sulfate, Al 2(SO 4) 3, is an ionic compound that is used in the manufacture of paper and in various water purification processes. What is the formula mass (amu) of this compound? Solution The formula for this compound indicates it contains Al 3+ and SO 4 2− ions combined in a 2:3 ratio.

For purposes of computing a formula mass, it is helpful to rewrite the formula in the simpler format, Al 2S 3O 12. Following the approach outlined above, the formula mass for this compound is calculated as follows: Check Your Learning Calcium phosphate, Ca 3(PO 4) 2, is an ionic compound and a common anti-caking agent added to food products. What is the formula mass (amu) of calcium phosphate? Answer: 310.18 amu The Mole The identity of a substance is defined not only by the types of atoms or ions it contains, but by the quantity of each type of atom or ion. For example, water, H 2O, and hydrogen peroxide, H 2O 2, are alike in that their respective molecules are composed of hydrogen and oxygen atoms. However, because a hydrogen peroxide molecule contains two oxygen atoms, as opposed to the water molecule, which has only one, the two substances exhibit very different properties.

Today, we possess sophisticated instruments that allow the direct measurement of these defining microscopic traits; however, the same traits were originally derived from the measurement of macroscopic properties (the masses and volumes of bulk quantities of matter) using relatively simple tools (balances and volumetric glassware). This experimental approach required the introduction of a new unit for amount of substances, the mole, which remains indispensable in modern chemical science. The mole is an amount unit similar to familiar units like pair, dozen, gross, etc. It provides a specific measure of the number of atoms or molecules in a bulk sample of matter. A mole is defined as the amount of substance containing the same number of discrete entities (such as atoms, molecules, and ions) as the number of atoms in a sample of pure 12C weighing exactly 12 g.

One Latin connotation for the word “mole” is “large mass” or “bulk,” which is consistent with its use as the name for this unit. The mole provides a link between an easily measured macroscopic property, bulk mass, and an extremely important fundamental property, number of atoms, molecules, and so forth. The number of entities composing a mole has been experimentally determined to be 6.02214179 × 10 23, a fundamental constant named Avogadro’s number ( N A) or the Avogadro constant in honor of Italian scientist Amedeo Avogadro. This constant is properly reported with an explicit unit of “per mole,” a conveniently rounded version being 6.022 × 10 23/mol. Consistent with its definition as an amount unit, 1 mole of any element contains the same number of atoms as 1 mole of any other element. The masses of 1 mole of different elements, however, are different, since the masses of the individual atoms are drastically different. The molar mass of an element (or compound) is the mass in grams of 1 mole of that substance, a property expressed in units of grams per mole (g/mol) (see ).

Each sample contains 6.022 × 10 23 atoms —1.00 mol of atoms. From left to right (top row): 65.4 g zinc, 12.0 g carbon, 24.3 g magnesium, and 63.5 g copper. From left to right (bottom row): 32.1 g sulfur, 28.1 g silicon, 207 g lead, and 118.7 g tin.

(credit: modification of work by Mark Ott) Because the definitions of both the mole and the atomic mass unit are based on the same reference substance, 12C, the molar mass of any substance is numerically equivalent to its atomic or formula weight in amu. Per the amu definition, a single 12C atom weighs 12 amu (its atomic mass is 12 amu). According to the definition of the mole, 12 g of 12C contains 1 mole of 12C atoms (its molar mass is 12 g/mol). This relationship holds for all elements, since their atomic masses are measured relative to that of the amu-reference substance, 12C.

Extending this principle, the molar mass of a compound in grams is likewise numerically equivalent to its formula mass in amu. Each sample contains 6.02 × 10 23 molecules or formula units—1.00 mol of the compound or element. Clock-wise from the upper left: 130.2 g of C 8H 17OH (1-octanol, formula mass 130.2 amu), 454.4 g of HgI 2 (mercury(II) iodide, formula mass 454.4 amu), 32.0 g of CH 3OH (methanol, formula mass 32.0 amu) and 256.5 g of S 8 (sulfur, formula mass 256.5 amu). (credit: Sahar Atwa) Element Average Atomic Mass (amu) Molar Mass (g/mol) Atoms/Mole C 12.01 12.01 6.022 × 10 23 H 1.008 1.008 6.022 × 10 23 O 16.00 16.00 6.022 × 10 23 Na 22.99 22.99 6.022 × 10 23 Cl 35.45 33.45 6.022 × 10 23 Table 1. While atomic mass and molar mass are numerically equivalent, keep in mind that they are vastly different in terms of scale, as represented by the vast difference in the magnitudes of their respective units (amu versus g).

To appreciate the enormity of the mole, consider a small drop of water weighing about 0.03 g (see ). Although this represents just a tiny fraction of 1 mole of water (18 g), it contains more water molecules than can be clearly imagined.

If the molecules were distributed equally among the roughly seven billion people on earth, each person would receive more than 100 billion molecules. The mole is used in chemistry to represent 6.022 × 10 23 of something, but it can be difficult to conceptualize such a large number. Watch this and then complete the “Think” questions that follow.

Explore more about the mole by reviewing the information under “Dig Deeper.” The relationships between formula mass, the mole, and Avogadro’s number can be applied to compute various quantities that describe the composition of substances and compounds. For example, if we know the mass and chemical composition of a substance, we can determine the number of moles and calculate number of atoms or molecules in the sample. Likewise, if we know the number of moles of a substance, we can derive the number of atoms or molecules and calculate the substance’s mass.

Example 3 Deriving Moles from Grams for an Element According to nutritional guidelines from the US Department of Agriculture, the estimated average requirement for dietary potassium is 4.7 g. What is the estimated average requirement of potassium in moles? Solution The mass of K is provided, and the corresponding amount of K in moles is requested. Referring to the periodic table, the atomic mass of K is 39.10 amu, and so its molar mass is 39.10 g/mol. The given mass of K (4.7 g) is a bit more than one-tenth the molar mass (39.10 g), so a reasonable “ballpark” estimate of the number of moles would be slightly greater than 0.1 mol. The molar amount of a substance may be calculated by dividing its mass (g) by its molar mass (g/mol): The factor-label method supports this mathematical approach since the unit “g” cancels and the answer has units of “mol:”. Example 4 Deriving Grams from Moles for an Element A liter of air contains 9.2 × 10 −4 mol argon.

What is the mass of Ar in a liter of air? Solution The molar amount of Ar is provided and must be used to derive the corresponding mass in grams. Since the amount of Ar is less than 1 mole, the mass will be less than the mass of 1 mole of Ar, approximately 40 g. The molar amount in question is approximately one-one thousandth (10 −3) of a mole, and so the corresponding mass should be roughly one-one thousandth of the molar mass (0.04 g): In this case, logic dictates (and the factor-label method supports) multiplying the provided amount (mol) by the molar mass (g/mol).

Copper wire is composed of many, many atoms of Cu. (credit: Emilian Robert Vicol) Solution The number of Cu atoms in the wire may be conveniently derived from its mass by a two-step computation: first calculating the molar amount of Cu, and then using Avogadro’s number ( N A) to convert this molar amount to number of Cu atoms: Considering that the provided sample mass (5.00 g) is a little less than one-tenth the mass of 1 mole of Cu (64 g), a reasonable estimate for the number of atoms in the sample would be on the order of one-tenth N A, or approximately 10 22 Cu atoms. Carrying out the two-step computation yields. Example 6 Deriving Moles from Grams for a Compound Our bodies synthesize protein from amino acids. One of these amino acids is glycine, which has the molecular formula C 2H 5O 2N. How many moles of glycine molecules are contained in 28.35 g of glycine?

Solution We can derive the number of moles of a compound from its mass following the same procedure we used for an element in: The molar mass of glycine is required for this calculation, and it is computed in the same fashion as its molecular mass. One mole of glycine, C 2H 5O 2N, contains 2 moles of carbon, 5 moles of hydrogen, 2 moles of oxygen, and 1 mole of nitrogen: The provided mass of glycine (28 g) is a bit more than one-third the molar mass (75 g/mol), so we would expect the computed result to be a bit greater than one-third of a mole (0.33 mol). Dividing the compound’s mass by its molar mass yields. Example 7 Deriving Grams from Moles for a Compound Vitamin C is a covalent compound with the molecular formula C 6H 8O 6. The recommended daily dietary allowance of vitamin C for children aged 4–8 years is 1.42 × 10 −4 mol. What is the mass of this allowance in grams?

Solution As for elements, the mass of a compound can be derived from its molar amount as shown: The molar mass for this compound is computed to be 176.124 g/mol. The given number of moles is a very small fraction of a mole (10 −4 or one-ten thousandth); therefore, we would expect the corresponding mass to be about one-ten thousandth of the molar mass (0.02 g). Performing the calculation, we get. Example 8 Deriving the Number of Atoms and Molecules from the Mass of a Compound A packet of an artificial sweetener contains 40.0 mg of saccharin (C 7H 5NO 3S), which has the structural formula: Given that saccharin has a molar mass of 183.18 g/mol, how many saccharin molecules are in a 40.0-mg (0.0400-g) sample of saccharin? How many carbon atoms are in the same sample? Solution The number of molecules in a given mass of compound is computed by first deriving the number of moles, as demonstrated in, and then multiplying by Avogadro’s number: Using the provided mass and molar mass for saccharin yields. Counting Neurotransmitter Molecules in the Brain The brain is the control center of the central nervous system.

It sends and receives signals to and from muscles and other internal organs to monitor and control their functions; it processes stimuli detected by sensory organs to guide interactions with the external world; and it houses the complex physiological processes that give rise to our intellect and emotions. The broad field of neuroscience spans all aspects of the structure and function of the central nervous system, including research on the anatomy and physiology of the brain.

Great progress has been made in brain research over the past few decades, and the BRAIN Initiative, a federal initiative announced in 2013, aims to accelerate and capitalize on these advances through the concerted efforts of various industrial, academic, and government agencies (more details available at www.whitehouse.gov/share/brain-initiative). Figure 8. (a) A typical human brain weighs about 1.5 kg and occupies a volume of roughly 1.1 L. (b) Information is transmitted in brain tissue and throughout the central nervous system by specialized cells called neurons (micrograph shows cells at 1600× magnification). Specialized cells called neurons transmit information between different parts of the central nervous system by way of electrical and chemical signals. Chemical signaling occurs at the interface between different neurons when one of the cells releases molecules (called neurotransmitters) that diffuse across the small gap between the cells (called the synapse) and bind to the surface of the other cell. These neurotransmitter molecules are stored in small intracellular structures called vesicles that fuse to the cell wall and then break open to release their contents when the neuron is appropriately stimulated. This process is called exocytosis (see ).

One neurotransmitter that has been very extensively studied is dopamine, C 8H 11NO 2. Dopamine is involved in various neurological processes that impact a wide variety of human behaviors.

Dysfunctions in the dopamine systems of the brain underlie serious neurological diseases such as Parkinson’s and schizophrenia. (a) Chemical signals are transmitted from neurons to other cells by the release of neurotransmitter molecules into the small gaps (synapses) between the cells. (b) Dopamine, C 8H 11NO 2, is a neurotransmitter involved in a number of neurological processes. One important aspect of the complex processes related to dopamine signaling is the number of neurotransmitter molecules released during exocytosis.

Since this number is a central factor in determining neurological response (and subsequent human thought and action), it is important to know how this number changes with certain controlled stimulations, such as the administration of drugs. It is also important to understand the mechanism responsible for any changes in the number of neurotransmitter molecules released—for example, some dysfunction in exocytosis, a change in the number of vesicles in the neuron, or a change in the number of neurotransmitter molecules in each vesicle.

Significant progress has been made recently in directly measuring the number of dopamine molecules stored in individual vesicles and the amount actually released when the vesicle undergoes exocytosis. Using miniaturized probes that can selectively detect dopamine molecules in very small amounts, scientists have determined that the vesicles of a certain type of mouse brain neuron contain an average of 30,000 dopamine molecules per vesicle (about 5 × 10 −20 mol or 50 zmol). Analysis of these neurons from mice subjected to various drug therapies shows significant changes in the average number of dopamine molecules contained in individual vesicles, increasing or decreasing by up to three-fold, depending on the specific drug used. These studies also indicate that not all of the dopamine in a given vesicle is released during exocytosis, suggesting that it may be possible to regulate the fraction released using pharmaceutical therapies. Key Concepts and Summary The formula mass of a substance is the sum of the average atomic masses of each atom represented in the chemical formula and is expressed in atomic mass units.

The formula mass of a covalent compound is also called the molecular mass. A convenient amount unit for expressing very large numbers of atoms or molecules is the mole.

Experimental measurements have determined the number of entities composing 1 mole of substance to be 6.022 × 10 23, a quantity called Avogadro’s number. The mass in grams of 1 mole of substance is its molar mass. Due to the use of the same reference substance in defining the atomic mass unit and the mole, the formula mass (amu) and molar mass (g/mol) for any substance are numerically equivalent (for example, one H 2O molecule weighs approximately 18 amu and 1 mole of H 2O molecules weighs approximately 18 g). Chemistry End of Chapter Exercises. What is the total mass (amu) of carbon in each of the following molecules?

(a) CH 4 (b) CHCl 3 (c) C 12H 10O 6 (d) CH 3CH 2CH 2CH 2CH 3. What is the total mass of hydrogen in each of the molecules? (a) CH 4 (b) CHCl 3 (c) C 12H 10O 6 (d) CH 3CH 2CH 2CH 2CH 3. Calculate the molecular or formula mass of each of the following: (a) P 4 (b) H 2O (c) Ca(NO 3) 2 (d) CH 3CO 2H (acetic acid) (e) C 12H 22O 11 (sucrose, cane sugar). Determine the molecular mass of the following compounds: (a) (b) (c) (d). Determine the molecular mass of the following compounds: (a) (b) (c) (d). Which molecule has a molecular mass of 28.05 amu?

(a) (b) (c). Write a sentence that describes how to determine the number of moles of a compound in a known mass of the compound if we know its molecular formula.

Compare 1 mole of H 2, 1 mole of O 2, and 1 mole of F 2. (a) Which has the largest number of molecules? (b) Which has the greatest mass?. Which contains the greatest mass of oxygen: 0.75 mol of ethanol (C 2H 5OH), 0.60 mol of formic acid (HCO 2H), or 1.0 mol of water (H 2O)?. Which contains the greatest number of moles of oxygen atoms: 1 mol of ethanol (C 2H 5OH), 1 mol of formic acid (HCO 2H), or 1 mol of water (H 2O)?. How are the molecular mass and the molar mass of a compound similar and how are they different? Solutions Answers to Chemistry End of Chapter Exercises 1.

(a) 12.01 amu; (b) 12.01 amu; (c) 144.12 amu; (d) 60.05 amu 3. (a) 123.896 amu; (b) 18.015 amu; (c) 164.086 amu; (d) 60.052 amu; (e) 342.297 amu 5.

(a) 56.107 amu; (b) 54.091 amu; (c) 199.9976 amu; (d) 97.9950 amu 7. Use the molecular formula to find the molar mass; to obtain the number of moles, divide the mass of compound by the molar mass of the compound expressed in grams. Its formula has twice as many oxygen atoms as the other two compounds (one each). Therefore, 0.60 mol of formic acid would be equivalent to 1.20 mol of a compound containing a single oxygen atom. The two masses have the same numerical value, but the units are different: The molecular mass is the mass of 1 molecule while the molar mass is the mass of 6.022 × 10 23 molecules. (a) 256.528 g/mol; (b) 72.150 g mol −1; (c) 378.103 g mol −1; (d) 58.080 g mol −1; (e) 180.158 g mol −1 15.

(a) 197.382 g mol −1; (b) 257.163 g mol −1; (c) 194.193 g mol −1; (d) 60.056 g mol −1; (e) 306.464 g mol −1 17. (a) 0.819 g; (b) 307 g; (c) 0.23 g; (d) 1.235 × 10 6 g (1235 kg); (e) 765 g 19. (a) 99.41; (b) 2.27 g; (c) 3.5 g; (d) 222 kg; (e) 160.1 g 21. (a) 9.60 g; (b) 19.2 g; (c) 28.8 g 23. Zirconium: 2.038 × 10 23 atoms; 30.87 g; silicon: 2.038 × 10 23 atoms; 9.504 g; oxygen: 8.151 × 10 23 atoms; 21.66 g 25.

AlPO 4: 1.000 mol Al 2Cl 6: 1.994 mol Al 2S 3: 3.00 mol 27. 3.113 × 10 25 C atoms 29. 0.865 servings, or about 1 serving.

20.0 g H 2O represents the least number of molecules since it has the least number of moles.

Study Guide Chapter 3 What is average mass? What is average atomic mass? What is the atomic mass? What is the mole? If you have a mole of cheese, how many pieces of cheese do you have? What is the Avogdro’s number? What is this number used for?

How do we use the mole in chemical reactions? Students must be able to calculate the mass of given numbers of atoms of an element. For example, calculate the mass of 10 atoms of carbon.

See example 3.2. Students must be able to calculate the moles of atoms. See example 3.3.

Students must be able to calculate number of atoms. See example 3.3. Students must be able to calculate number of moles and mass. What is molar mass?

Students must be able to calculate the molar masses for a given compound. For example, calculate the molar mass of C 6H 12O 6.

See examples 3.6 and 3.7 and 3.8. Discuss, in as many details as you can, the conceptual problem solving approach. What is percent composition? What is the percent mass composition of C 6H 12O 6. See example 3.9. What is the formula of a compound? How can we determine the formula of a compound?

How do we determine the empirical formula of a compound? What type of data do we need to have to determine the empirical formula for a compound? What type of data do we need to have to determine the molecular formula of a compound? How do we determine the molecular formula from the empirical formula? A compound that contains only C, H and O is 48.64% C and 8.16% H. What is the empirical formula for this compound?

See examples 3. What is a chemical reaction? What is a chemical equation? Describe a chemical equation in detail. Students must learn how to do read a chemical equation. Why are we required to balance chemical equations?

How do we balance chemical equations? See examples 3.13 – 3.14. What is stoichiometric calculations? When do we perform such calculations?

See examples 3.15 – 3.16. What is a limiting reagent? How do we calculate the limiting reagent?

What type of data do we need to calculate the limiting reagent? What is theoretical yield? What is actual (experimental) yield?

What is percent yield? What does percent yield mean?