Molar mass of sugar

Learning Objectives • To calculate the molecular mass of a covalent compound. • To calculate the formula mass of an ionic compound. • To calculate the number of atoms, molecules or formula units in a sample. Chemistry is the study of how atoms and molecules interact with each other which occurs on the atomic scale. Chemists need a way of simply determining how many molecules they have in a beaker. The mole concept, which we will introduce here, bridges that gap by relating the mass of a single atom or molecule in amu to the mass of a collection of a large number of such molecules in grams. As you learned, the mass number is the sum of the numbers of protons and neutrons present in the nucleus of an atom. The mass number is an integer that is approximately equal to the numerical value of the atomic mass. Although the mass number is unitless, it is assigned units called atomic mass units (amu). Because a molecule or a polyatomic ion is an assembly of atoms whose identities are given in its molecular or ionic formula, we can calculate the average atomic mass of any molecule or polyatomic ion from its composition by adding together the masses of the constituent atoms. The average mass of a monatomic ion is the same as the average mass of an atom of the element because the mass of electrons is so small that it is insignificant in most calculations. This is not much help in the laboratory for the typical chemist who only has a balance to weight out chemicals but needs to know ho...

In preceding sections, we focused on the composition of substances: samples of matter that contain only one type of element or compound. However, mixtures—samples of matter containing two or more substances physically combined—are more commonly encountered in nature than are pure substances. Similar to a pure substance, the relative composition of a mixture plays an important role in determining its properties. The relative amount of oxygen in a planet’s atmosphere determines its ability to sustain aerobic life. The relative amounts of iron, carbon, nickel, and other elements in steel (a mixture known as an “ Figure \(\PageIndex\): Sugar is one of many components in the complex mixture known as coffee. The amount of sugar in a given amount of coffee is an important determinant of the beverage’s sweetness. (credit: Jane Whitney) Video \(\PageIndex\): An introduction to solutions from Crash Course Chemistry. We have previously defined solutions as homogeneous mixtures, meaning that the composition of the mixture (and therefore its properties) is uniform throughout its entire volume. Solutions occur frequently in nature and have also been implemented in many forms of manmade technology. We will explore a more thorough treatment of solution properties in the chapter on solutions and colloids, but here we will introduce some of the basic properties of solutions. The relative amount of a given solution component is known as its concentration. Often, though not always, a solution...

Mass of weigh boat Mass of weigh boat + un-chewed gum Mass of un-chewed gum Mass of chewed gum Mass of sugar Percent of sugar 2.4g 8.5g 6.1g 4.7 1.4 22.95 2.4g 8.5g 6.1g 4.7 1.4 22.95 2.4g 8.5g 6.1g 4.7 1.4 22.95 Post-Lab Questions 1. What is the percent sugar? Show your calculations. (1.6/ 6.4)x100=22.95% 2. What is the molar mass of sugar C 12H 22O 11? Show your calculations. C12H22O11 = 12(mass of C) + 22(mass of H) + 11(mass of O) C12H22O11 = 12(12.01) + 22(1.008) + 11(16.00) C12H22O11 = = 342.30 3. Convert the mass of dissolved sugar to moles. Show your calculations. 4. Convert the moles of sugar to molecules of sugar. Show your calculations. 5. Convert atoms of sugar to grams of sugar. Show your calculations. 6. Imagine that you used four pieces of gum instead of two. Calculate the number of moles. Show your calculations. 7. How does the mass of the saliva alter the experimental data?

Molar Mass of an Element According tothe −24g, these masses would be way too small to measure onordinary laboratory equipment. However, if we have 6.022×10 23atoms, or 1 mole of each of these elements, we would have 26.98 g Al, 63.55 g Cu, and 12.01 g C. In other words, one mole of any element will have a mass that is numerically equal to itsatomic mass andexpressedin units of grams. This mass is called the molar mass. Figure \(\PageIndex\): One mole of aluminum, copper, and carbon.(R. Press/N. Hanacek/NIST) • 1 mol Al = 26.98 g Al = 6.022×10 23atoms Al • 1 mol Cu= 63.55g Cu= 6.022×10 23atoms Cu • 1 mol C = 12.01g C= 6.022×10 23atoms C Molar Mass of a Compound One mole of any compoundwill have a mass that is numerically equal to its molecular mass or formula mass and expressedin units of grams. This mass is also called the molar mass. In 23formula units of NaCl, or one mole of NaCl. We also calculated the molecularmass for C 12H 22O 11to be 342.3 amu. This means that the molar mass of C 12H 22O 11is342.3g and it will contain 6.022×10 23molecules of C 12H 22O 11, or one mole of C 12H 22O 11. • 1 mol NaCl= 58.44g NaCl= 6.022×10 23formula units NaCl • 1 mol C 12H 22O 11= 342.3g C 12H 22O 11= 6.022×10 23moleculesC 12H 22O 11 Figure \(\PageIndex\): One mole table salt (NaCl) and sugar (C 12H 22O 11).(Lance S. Lund) Summary of Relevant Terminology Keepingthe terminology straight (see Substance Fundamental Unit Atomic, Molecular, or Formula Mass Molar Mass aluminum (Al) atom atom...

Learning Objectives By the end of this section, you will be able to: • Describe the fundamental properties of solutions • Calculate solution concentrations using molarity • Perform dilution calculations using the dilution equation Preceding sections of this chapter focused on the composition of substances: samples of matter that contain only one type of element or compound. However, mixtures—samples of matter containing two or more substances physically combined—are more commonly encountered in nature than are pure substances. Similar to a pure substance, the relative composition of a mixture plays an important role in determining its properties. The relative amount of oxygen in a planet’s atmosphere determines its ability to sustain aerobic life. The relative amounts of iron, carbon, nickel, and other elements in steel (a mixture known as an “alloy”) determine its physical strength and resistance to corrosion. The relative amount of the active ingredient in a medicine determines its effectiveness in achieving the desired pharmacological effect. The relative amount of sugar in a beverage determines its sweetness (see Figure 3.14 Sugar is one of many components in the complex mixture known as coffee. The amount of sugar in a given amount of coffee is an important determinant of the beverage’s sweetness. (credit: Jane Whitney) Solutions Solutions have previously been defined as homogeneous mixtures, meaning that the composition of the mixture (and therefore its p...

Sugar, or more specifically, sucrose, is a molecule that is essential to photosynthesis. In fact, photosynthesis would not be possible without sugar. Sugar is necessary for the transfer of energy from the sun to the plant, and it is also necessary for the plant to create its own food. The molar mass of sugar is 12 g/mol. What is the mass of 3.5 mol glucose? C6H12O6 has a molar mass of 180.18 g/mol. To make sugar, plants use energy from sunlight to convert carbon dioxide (CO2) into a gas absorbed by the air, as well as water (H20) obtained by roots from the ground into glucose (C6H12O6). This process is referred to as photosynthesis in plants and occurs in the chloroplasts of the cells. Glucose, C6H12O6, is produced as a result of dark reactions, also known as the Calvin cycle, during photosynthesis. What Is The Molar Mass Of Sugar C6h12o6? Source: slideserve.com C6H12O6 is what defines the same as C6H12O6. The color is commonly referred to as white power. Glucose has a molecular mass of 180.156 amino acids. The carbon atoms and oxygen atoms are the building blocks of glucose, which is a white crystalline structure. Glucose is the most important type of sugar for a person’s health. To be classified, glucose is a carbohydrate that is broken down by the body into glucose molecules. glucose, which is also an energy source, provides both fuel and energy. What Is The Molar Mass For The Empirical Formula Of C6h12o6? The molar mass of C6 H12 O6 is 180.15588 g/mol. The number of at...

Start by writing the chemical equation that describes this reaction #"C"_ 6"H"_ 12"O"_ (6(aq)) -> 2"C"_ 2"H"_ 5"OH"_ ((aq)) + 2"CO"_ (2(g)) uarr# #color(white)(aaaaaaaaaaaaaaaaaaaaaaaaaaaa)/color(white)(a)# SIDE NOTE As you can see, I am assuming that by #"250 g"# of sugar you mean #"250 g"# of glucose, not sucrose, #"C"_12"H"_22"O"_11#. If you were supposed to work with sucrose instead of glucose, add this step #"C"_ 12"H"_ 22"O"_ (11(aq)) + "H"_ 2"O"_ ((l)) -> 2"C"_ 6"H"_ 12 "O"_ (6(aq))# and redo the calculations with the mass of glucose that you'll get from this reaction. #color(white)(aaaaaaaaaaaaaaaaaaaaaaaaaaaa)/color(white)(a)# Now, notice that you have a #1:2# mole ratio between glucose and ethanol, so convert the mass of glucose to moles by using the compound's molar mass #250 color(red)(cancel(color(black)("g"))) * "1 mole glucose"/(180.156color(red)(cancel(color(black)("g")))) = "1.388 moles glucose"# This means that the reaction will produce #1.388 color(red)(cancel(color(black)("moles glucose"))) * "2 moles ethanol"/(1color(red)(cancel(color(black)("mole glucose")))) = "2.776 moles ethanol"# To convert this to grams, use the molar mass of ethanol #2.776 color(red)(cancel(color(black)("moles ethanol"))) * "46.07 g"/(1color(red)(cancel(color(black)("mole ethanol")))) = "127.9 g"# Rounded to two #color(darkgreen)(ul(color(black)("theoretical yield = 130 g")))# To convert this to milliliters, use the #127.9 color(red)(cancel(color(black)("g"))) * "1 mL"/(0.79colo...

Analyzing the given data: Given Mass of sugar = 34 . 2 g Molar Mass of sugar = 342 g mol - 1 No. of moles of sugar = Given mass Molecular mass = 34 . 2 342 = 0 . 1 mole Sugar syrup contains sugar in water. So, mass of water = ( 214 . 2 - 34 . 2 ) g = 180 g Molar Mass of Water = 18 g mol - 1 No. of moles of water = Given mass Molecular mass = 180 18 = 10 mole Part (i): Molarity of solution Molarity(M): The number of moles of a solute dissolved in 1 L (1000 ml) of the solution is known as the molarity of the solution. Molarity ( M ) = Mole of solute Volume of solution ( in litre ) M = 0 . 1 180 × 1000 = 0 . 555 M Thus, the molarity of sugar is 0.555 M Part (ii): Mole fraction of sugar Total number of moles of solution = mole of solute + mole of solvent = 0 . 1 + 10 = 10 . 1 Mole fraction of sugar = Mole of sugar Total mole of solution = 0 . 1 10 . 1 = 0 . 0099 Thus, mole fraction of sugar in the syrup is 0.0099.