How Many Molecules Of Glucose Does It Contain? Express Your Answer Using Four Significant Figures.

3.1 Formula Mass And The Mole Concept

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 compounds 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 Figure 3 ). Figure 3. 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 Continue reading >>

Maltose - An Overview | Sciencedirect Topics

Larry R. Engelking, in Textbook of Veterinary Physiological Chemistry (Third Edition) , 2015 Disaccharides consist of two monosaccharides joined by a glycosidic bond. Structures for the most common disaccharides are shown in Fig. 18-4. Maltose (or malt sugar) is an intermediate in the intestinal digestion (i.e., hydrolysis) of glycogen and starch, and is found in germinating grains (and other plants and vegetables). It consists of two molecules of glucose in an -(1,4) glycosidic linkage. Trehalose, which contains two molecules of glucose linked together somewhat differently from maltose, is a major carbohydrate found in the hemolymph of many insects. It is also found in young mushrooms, where it accounts for about 1.5% of their weight. Cellobiose, the repeating disaccharide unit of cellulose, has -(1,4) glycosidic linkages which are broken by bacterial cellulases, but not by mammalian constitutive digestive enzymes. Lactose is found in milk, but otherwise does not occur in nature. It consists of galactose and glucose in a -(1,4) glycosidic linkage. Sucrose, or cane sugar, consists of glucose and fructose linked in an -(1,2) glycosidic bond. It is abundant in the plant world, and is familiar as table sugar. Sucrose and maltose are readily hydrolyzed by disaccharidases found in the brush border of the small intestine (see Chapter 38). Hydrolysis of sucrose to glucose and fructose is sometimes called inversion, since it is accompanied by a net change in optical rotation from dextro to levo as the equimolar mixture of glucose and fructose is formed on the mucosal surface. Therefore, the intestinal brush border enzyme that hydrolyzes sucrose (i.e., sucrase), is sometimes called invertase (see Chapter 38). A number of trisaccharides also occur free in nature, and are consume Continue reading >>

Chapter 1: Measurements In Chemistry - Chemistry

Use Your Creativity to Make a Difference! Apply for the Maurice Undergraduate Competition Foundations in General, Organic, and Biological Chemistry This content can also be downloaded as an printable PDF or an interactive PDF . For the interactive PDF, adobe reader is required for full functionality. This text is published under creative commons licensing, for referencing and adaptation, please click here. Everything around us is made up of chemicals. From the color that makes a rose so red to the gasoline that fills our cars and the silicon chips that power our computers and cell phonesChemistry is everywhere! Understanding how chemical molecules form and interact to create complex structures enables us to harness the power of chemistry and use it, just like a toolbox, to create many of the modern advances that we see today. This includes advances in medicine, communication, transportation, building infrastructure, food science and agriculture, and nearly every other technical field that you can imagine. Chemistry is one branch of science. Science is the process by which we learn about the natural universe by observing, testing, and then generating models that explain our observations. is the process by which we learn about the natural universe by observing, testing, and then generating models that explain our observations. Because the physical universe is so vast, there are many different branches of science (Figure 1.1). Thus, chemistry is the study of matter, biology is the study of living things, and geology is the study of rocks and the earth. Mathematics is the language of science, and we will use it to communicate some of the ideas of chemistry. Although we divide science into different fields, there is much overlap among them. For example, some biologists and Continue reading >>

The Mole | Chemistry For Non-majors

Is there an easier way to load this truck? When the weather is nice, many people begin to work on their yards and homes. For many projects, sand is needed as a foundation for a walk or to add to other materials. You could order up twenty million grains of sand and have people really stare at you. You could order by the pound, but that takes a lot of time weighing out. The best bet is to order by the yard, meaning a cubic yard. The loader can easily scoop up what you need and put it directly in your truck. It certainly is easy to count bananas or to count elephants (as long as you stay out of their way). However, you would be counting grains of sugar from your sugar canister for a long, long time. Atoms and molecules are extremely small far, far smaller than grains of sugar. Counting atoms or molecules is not only unwise, it is absolutely impossible. One drop of water contains about 10 22 molecules of water. If you counted 10 molecules every second for 50 years without stopping you would have counted only 1.610 10 molecules. Put another way, at that counting rate, it would take you over 30 trillion years to count the water molecules in one tiny drop. Chemists needed a name that can stand for a very large number of items. Amedeo Avogadro (1776 1856), an Italian scientist, provided just such a number. He is responsible for the counting unit of measure called the mole. A mole (mol) is the amount of a substance that contains 6.0210 23 representative particles of that substance. The mole is the SI unit for amount of a substance. Just like the dozen and the gross, it is a name that stands for a number. There are therefore6.0210 23 water molecules in a mole of water molecules. There also would be6.0210 23 bananas in a mole of bananas, if such a huge number of bananas ever exis Continue reading >>

Chemistry Ii: Water And Organic Molecules

Table of Contents It can be quite correctly argued that life exists on Earth because of the abundant liquid water. Other planets have water, but they either have it as a gas (Venus) or ice (Mars). This relationship is shown in Figure 1. Recent studies of Mars reveal the presence sometime in the past of running fluid, possibly water. The chemical nature of water is thus one we must examine as it permeates living systems: water is a universal solvent, and can be too much of a good thing for some cells to deal with. Figure 1. Water can exist in all three states of matter on Earth, while only in one state on our two nearest neighboring planets. The above graph is from Water is polar covalently bonded within the molecule. This unequal sharing of the electrons results in a slightly positive and a slightly negative side of the molecule. Other molecules, such as Ethane, are nonpolar, having neither a positive nor a negative side, as shown in Figure 2. Figure 2. The difference between a polar (water) and nonpolar (ethane) molecule is due to the unequal sharing of electrons within the polar molecule. Nonpolar molecules have electrons equally shared within their covalent bonds. Image from Purves et al., Life: The Science of Biology, 4th Edition, by Sinauer Associates (www.sinauer.com) and WH Freeman (www.whfreeman.com), used with permission. These link up by the hydrogen bond discussed earlier. Consequently, water has a great interconnectivity of individual molecules, which is caused by the individually weak hydrogen bonds, shown in Figure 3, that can be quite strong when taken by the billions. Figure 3. Formation of a hydrogen bond between the hydrogen side of one water molecule and the oxygen side of another water molecule. Image from Purves et al., Life: The Science of Biology, Continue reading >>

Chemistry Final- Ch 1-9

Which of the following are pure substances. How many liters of oil are in a 42 gallon barrel? In which state does matter have an indefinite shape and definite volume? In which state of matter are forces between particles least dominant? Driving to the grocery store, you notice that the temperature outside is 45 degrees C. What is this temperature in F? A 12.8 mL sample of bromine has a mass of 39.9 g. What is the density of bromine? The green color of the Statue of Liberty is due to a ______________ change to the copper metal it is made of. What type of property of matter is independent of the quantity of the substance? The number 1200 written in correct scientific notation is: How many pounds are represented by 764.6 mg? [Use: 1 pound = 454 g] The number 0.0468 written in correct scientific notation is: The cost of a drug is 125 francs per gram. What is the cost in dollars per ounce? [Use: $1 = 6.25 francs and 1 ounce = 28.4 g] How many significant figures are in the number 5.06305 10^4? Provide the answer to the following problem using scientific notation and the proper number of significant digits: (6.00 10^2)(3.00 10^4) = ? Provide the answer to the following problem using the proper number of significant digits: 0.004 + 26.59 + 3.2 = ? How many significant figures are in the following measurement: 3.025 ft. What do we call a statement of observed behavior for which no exceptions have been found? How many significant figures are in the following value? 100,000 people How many significant figures are in the following measurement? 0.001 miles The number 42.246 rounded to four significant figures is: What kind of change always results in the formation of new materials? The number 88.015 rounded to 3 significant figures is: Which one of the following is an example of a Continue reading >>

Chemistry: The Central Science, Chapter 3, Section 4

Even the smallest samples that we deal with in the laboratory contain enormous numbers of atoms, ions, or molecules. For example, a teaspoon of water (about 5 mL) contains 2 1023 water molecules! It is convenient to have a special unit for describing such large numbers of objects. In everyday life we use counting units like dozen (12 objects) and gross (144 objects) to deal with large quantities. In chemistry the unit for dealing with atoms, ions, and molecules is the mole, abbreviated mol. (The term mole comes from the Latin word moles, meaning "a mass." The term molecule is the diminutive form of this word and means "a small mass.") A mole is defined as the amount of matter that contains as many objects (atoms, molecules, or whatever objects we are considering) as the number of atoms in exactly 12 g of 12C. From experiments scientists have determined the number of atoms in this quantity of 12C to be 6.0221421 1023. This number is given a special name: Avogadro's number, in honor of Amedeo Avogadro (1776-1856), an Italian scientist. For most purposes we will use 6.02 1023 for Avogadro's number throughout the text. A mole of ions, a mole of molecules, or a mole of anything else all contain Avogadro's number of these objects: Avogadro's number is so large that it is difficult to imagine. Spreading 6.02 1023 marbles over the entire surface of Earth would produce a layer about 3 mi thick! Calculate the number of C atoms in 0.350 mol of C6H12O6. SOLUTION Let's examine this question using the problem-solving steps in the Strategies in Chemistry essay on page 79 of the textbook. Analysis: We are given 0.350 mol of C6H12O6. Thus, we know both the amount of the substance and its chemical formula. The unknown is the number of C atoms in this sample. Plan: Avogadro's number prov Continue reading >>

Express The Number Of Atoms To Three Significant

CorrectEstimating the answer can help you determine whether to multiply or divide by the conversion factor. In this case, the number ofmolecules should be greater than the number of moles, so it follows that you should multiply the number of moles by Avogadro'snumber, not divide.Another strategy is to consider how the units will cancel.Hint 2. Identify how units cancelWhich operation will allow units of moles to cancel?ANSWER:CorrectThe unit "" will cancel, leaving the unit "molecules."ANSWER:Hint 4. Try it on your own without hints!The glucose molecule, , contains six carbon atoms in one molecule. The molecular weight of glucose is 180.2 . How manycarbon atoms are in 3.50 grams of glucose?Express the number of atoms to three significant figures.ANSWER:ANSWER:Answer RequestedWriting Formulas for Molecular Inorganic CompoundsLearning Goal:To review the method for writing chemical formulas in general for molecular inorganic compounds.In any chemical formula, subscripts indicate the number of each type of atom in one molecule or formula unit. For example, one molecule of containsthree carbon atoms, six hydrogen atoms, and three oxygen atoms. One molecule contains one nitrogen atom and three fluorine atoms. One formula unitof contains two sodium atoms and one sulfur atom.There are three main types of chemical formulas: organic, molecular inorganic, and ionic.1. is an organiccompound. It contains predominantly carbon and hydrogen atoms. This is the end of the preview. Sign up to access the rest of the document. Continue reading >>

Section 16.1oxidation Of Glucose And Fatty Acids To Co2

The complete aerobic oxidation of glucose is coupled to the synthesis of as many as 36 molecules of ATP: Glycolysis, the initial stage of glucose metabolism, takes place in the cytosol and does not involve molecular O. It produces a small amount of ATP and the three-carbon compound pyruvate. In aerobic cells, pyruvate formed in glycolysis is transported into the mitochondria, where it is oxidized by O to CO. Via chemiosmotic coupling, the oxidation of pyruvate in the mitochondria generates the bulk of the ATP produced during the conversion of glucose to CO. In this section, we discuss the biochemical pathways that oxidize glucose and fatty acids to CO and HO; the fate of the released electrons is described in the next section. Go to: Cytosolic Enzymes Convert Glucose to Pyruvate A set of 10 enzymes catalyze the reactions, constituting the glycolytic pathway, that degrade one molecule of glucose to two molecules of pyruvate (Figure 16-3). All the metabolic intermediates between glucose and pyruvate are watersoluble phosphorylated compounds. Four molecules of ATP are formed from ADP in glycolysis (reactions 6 and 9). However, two ATP molecules are consumed during earlier steps of this pathway: the first by the addition of a phosphate residue to glucose in the reaction catalyzed by hexokinase (reaction 1), and the second by the addition of a second phosphate to fructose 6-phosphate in the reaction catalyzed by phosphofructokinase-1 (reaction 3). Thus there is a net gain of two ATP molecules. The balanced chemical equation for the conversion of glucose to pyruvate shows that four hydrogen atoms (four protons and four electrons) are also formed: (For convenience, we show pyruvate in its un-ionized form, pyruvic acid, although at physiological pH it would be largely dissociat Continue reading >>

Calculating Formula Masses

Since a molecule - scratch that, there we go again, calling everything molecules! Since a formula is made of atoms, we can calculate a formula mass by simply adding up all the atoms that are in it. This is an application of the law of conservation of mass. Count up the number of atoms of each type in the formula, and add up the total mass. We've broken this out in the form of a table in these examples, and you'll probably want to use a somewhat similar method. Which of the following is a correct calculation of the formula mass? What is the formula mass of CaCO3 to 1 decimal place? When a formula contains polyatomic ions, the number of atoms inside the brackets are multiplied by any subscript immediately behind the brackets, as shown in this example. Which of the following is a correct calculation of the formula mass? What is the formula mass of Ba(HSO3)2 to 1 decimal place? Sometimes when ionic crystals form, water becomes a part of the crystal structure. This is known as water of hydration, and the crystals are called "hydrates", or "hydrated salts". Formulas for hydrates always include a dot separator, followed by the number of water molecules attached, such as formulas like CuSO4.5H2O. There are several ways you can do such formulas. One method is to treat the water of hydration as having its own mass, and add it to the other masses as shown in this example. Which of the following is a correct calculation of the formula mass? The above were all examples of ionic formulas, but exactly the same principle applies to true molecular formulas, such as that of glucose. To two decimal places, what is the formula mass of CH3CH2OH (ethanol)? In each of the above examples the atomic masses were rounded off at the second decimal point. Some of the atomic masses of the elements Continue reading >>

2.4: Significant Figures In Calculations

Use significant figures correctly in arithmetical operations. Before dealing with the specifics of the rules for determining the significant figures in a calculated result, we need to be able to round numbers correctly. Torounda number, first decide how many significant figures the number should have. Once you know that, round to that many digits, starting from the left. If the number immediately to the right of the last significant digit is less than 5, it is dropped and the value of the last significant digit remains the same. If the number immediately to the right of the last significant digit is greater than or equal to 5, the last significant digit is increased by 1. Consider the measurement $207.518 \: \text{m}$. Right now, the measurement contains six significant figures. How would we successively round it to fewer and fewer significant figures? Follow the process as outlined in Table $\PageIndex{1}$. Notice that the more rounding that is done, the less reliable the figure is. An approximate value may be sufficient for some purposes, but scientific work requires a much higher level of detail. It is important to be aware of significant figures when you are mathematically manipulating numbers. For example, dividing 125 by 307 on a calculator gives 0.4071661238 to an infinite number of digits. But do the digits in this answer have any practical meaning, especially when you are starting with numbers that have only three significant figures each? When performing mathematical operations, there are two rules for limiting the number of significant figures in an answerone rule is for addition and subtraction, and one rule is for multiplication and division. In operations involving significant figures, the answer is reported in such a way that it reflects the reliabil Continue reading >>

The Mole

The mole is the unit of amount in chemistry. It provides abridge between the atom and the macroscopic amounts of material that wework with in the laboratory. It allows the chemist to weigh out amountsof two substances, say iron and sulfur, such that equal numbers of atomsof iron and sulfur are obtained. A mole of a substance is definedas: The mass of substance containing the same numberof fundamental units as there are atoms in exactly 12.000 g of 12C. Fundamental units may be atoms, molecules, or formula units, dependingon the substance concerned. At present, our best estimate of the numberof atoms in 12.000 g of 12C is 6.022 x 1023, a hugenumber of atoms. This is obviously a very important quantity.For historical reasons, it is called Avogadro's Number, and is given thesymbol NA. Unfortunately, the clumsy definition of the mole obscures its utility.It is nearly analogous to defining a dozen as the mass of a substance thatcontains the same number of fundamental units as are contained in 733 gof Grade A large eggs. This definition completely obscures the utilityof the dozen: that it is 12 things! Similarly, a mole is NAthings. The mole is the same kind of unit as the dozen -- a certain numberof things. But it differs from the dozen in a couple of ways.First, the number of things in a mole is so huge that we cannot identifywith it in the way that we can identify with 12 things. Second, 12is an important number in the English system of weights and measures, sothe definition of a dozen as 12 things makes sense. However, the choiceof the unusual number, 6.022 x 1023, as the number of thingsin a mole seems odd. Why is this number chosen? Would it not makemore sense to define a mole as 1.0 x 1023 things, a nice (albeitlarge) integer that everyone can easily remember? To unde Continue reading >>

Ch. 5: Chemical Reactions

What is the correct procedure to calculate the mass of a substance, given the number of moles? The number of entities in a mole (to 4 sig figs) is equal to ___x1023 and is called ______ number. What is the molar mass of the compound KrF2? What is the molar mass of the compound SF6? What is the molar mass of the compound CCl4? What is the molar mass of the compound CH2O? Which pieces of information are necessary to calculate the molar mass of a compound? The boiling of water is an example of a ____ change. When converting from grams to number of molecules, the magnitude of the answer ______ (increases/decreases). What is the correct mathematical operation to convert the number of atoms in a sample to the number of moles? Which of the following describe a physical change? the melting of a chocolate bar, the cooking of an egg, dissolving sugar in a cup of hot tea, the burning of a candle The _____ is the SI unit for amount of substance. Specifically, it is defined as the amount of a substance that contains the same number of entities as the number of ______ in exactly 12g of carbon-12. True or false: A chemical change may involve physical changes. The new substances that are formed in a chemical reaction are called _______. The molecular mass of a compound is the ___ of the atomic masses of the elements in one ___ of the compound. How many C, H, and O atoms are found in the products of the following reaction? CH3CH2OH + 3 O2 --> 2 CO2 + 3 H2O In balancing the following chemical equation, what coefficient should be placed in front of H2O? The conversion of potassium chlorate to potassium chloride is an example of a _____ change. Which term describes the sum of the atomic masses of all the elements in a compound? True or False: Reduction is the gain of electrons. True or Fa Continue reading >>

Tutor For Fall Study

Have you heard of splenda? Splenda is the trademarked name for sucralose (C12H19O8Cl3), an artificial chlorinated sweetener used in diet coke and other soft drinks. Suppose you were worried about the amount of chlorine in your can of diet coke, which contains 2.1 grams (g) of splenda. Can you tell me how many grams of chlorine are in your can? Your result should have 2 significant figures. (Here are a couple hints for you: the molecular weight of splenda is 397.63 g splenda / mol splenda and the molecular weight of chlorine (Cl) is 35.453 g Cl / mol Cl.) 2.1 g splenda * ( 1 mol splenda / 397.63 g splenda) * (3 mol Cl / 1 mol splenda) * (35.453 g Cl / 1 mol Cl) = 0.56 g Cl Given Value Unit Conversion Composition Stoichiometry Molecular Weight As part of an experiment, suppose I gave you a 10.0 mL solution with 0.511 glucose molarity. Suppose, also, that you left the solution on a window sill over the week-end, and the liquid solution dried up, leaving only glucose. Can you tell me how many grams (g) of glucose (C6H12O6) would be left? Your result should have 3 significant figures. (Here is a hint for you: the molecular weight of C6H12O6 is 180 g glucose / mol glucose.) 10.0 mL solution * (1 L solution / 1000 mL solution) * (0.511 mol C6H12O6 / 1 L solution) * (180 g C6H12O6 / 1 mol C6H12O6) = 0.920 g C6H12O6 Given Value Unit Conversion Solution Concentration Molecular Weight Impersonal: Suppose the WHO recommended limit for arsenic in drinking water is equal to 0.000014 grams of arsenite (AsO2-) / L solution. To determine the concentration of arsenite in a solution sample that is safe, one needs to check it against the WHO recommendation. How many grams of arsenite (AsO2-) / L solution are in a sample with 0.58 moles of arsenite (AsO2-) in 100 kiloliters (100 kL) of sol Continue reading >>

A Sample Of Glucose, C6h12o6 Contains 2.03*10^21 Atoms Of Carbon. (a)how

a sample of glucose, c6h12o6 contains 2.03*10^21 atoms of carbon. (a)how many atoms of hydrogen does it contain? (b)how many molecules of glucose does it contain? (c)how many moles of glucose does it contain? (d)what is the mass of this sample in grams? its kinda long, but i would appreciate it if someone would guide me through it Molecular weight of glucose is 180.16 g/mo and its formula is C6H1206. a.) 2.03 x10^21 atoms of carbon*(1 mol/6.02 x 10^23 atoms)*(12 moles of H/6 moles of C)*(6.02x10^23 atoms/mole of H)=atoms of H ****Notice that Avogadro's number cancels out b.) 2.03 x10^21 atoms of carbon*(1 mol/6.02 x 10^23 atoms)*(1 mole of glucose/12 moles of C)*(6.02 x 10^23 atoms/1mole of glucose)= molecules of glucose ****Notice that Avogadro's number cancels out c.)2.03 x10^21 atoms of carbon*(1 mol/6.02 x 10^23 atoms)*(1 mole of glucose/12 moles of C)= moles of glucose d.2.03 x10^21 atoms of carbon*(1 mol/6.02 x 10^23 atoms)*(1 mole of glucose/12 moles of C)*(180.16 g/mole)= glucose in grams Continue reading >>