calculate the mass percentage composition of urea

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10 مارس 2023
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Example - 02: . Conversely, knowing the percent composition of the substances included in the mixture and the percent composition of the mixture itself, you can find the proportion in which these substances are included in the mixture. The given number of moles is a very small fraction of a mole (~104 or one-ten thousandth); therefore, we would expect the corresponding mass to be about one-ten thousandth of the molar mass (~0.02 g). Mg= 24.31 x 1 = 24.31. It is convenient to consider 1 mol of C9H8O4 and use its molar mass (180.159 g/mole, determined from the chemical formula) to calculate the percentages of each of its elements: \[\begin{align*} These cookies ensure basic functionalities and security features of the website, anonymously. Bess Ruff is a Geography PhD student at Florida State University. Here the molar mass of: N = 14 u. For a solution, mass percent equals the mass of an element in one mole of the compound divided by the molar mass of the compound, multiplied by 100%. To do this, grams; multiply the mass of the compound by a conversion factor based on the percent composition of the element in the compound. This is because naturally occurring carbon is a mixture of the isotopes 12C, 13C and 14C which have masses of 12 Da, 13.003355 Da, and 14.003242 Da respectively. 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 result is consistent with our rough estimate. Video $\PageIndex{3}$: A preview of some of the uses we will have for moles in upcoming units. Watch for rounding errors in the last significant figure to make sure all the percentages add up. 4.4: Formula Mass, Percent Composition, and the Mole is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. It means 1 gm of urea contains 1/60 mole molecules of urea. Percent composition is also useful for evaluating the relative abundance of a given element in different compounds of known formulas. The molecular formula of Urea= NH 2 CONH 2. The concentration of Fe3+ ion in a sample of H2O is 335.0 ppm. >. If we calculate the mass % of A, the mass % of B will be found by subtracting the mass % of A from 100. Mathematical manipulation of molality is the same as with molarity. This will help catch any math errors. To calculate the mass percent of an element in a compound, we divide the mass of the element in 1 mole of the compound by the compound's This online Percent Composition Calculator finds the elemental composition as well as the percentage distribution of the number of atoms and their masses for a molecule given its chemical formula. You may Accept All cookies or visit Cookie Settings to provide a controlled consent. ThoughtCo. "I rely so much on wikiHow whenever I don't understand the lesson. H2O) as well as denoted using the tiny numbers, like or , (e.g. Percent means per 100 parts, where for solutions, part refers to a measure of mass (g, mg, g, kg, etc.) In this section, we will explore how to apply these very same principles in order to derive the chemical formulas of unknown substances from experimental mass measurements. 1) Calculate the amount of water (in grams) that must be added to 5.00 g of urea (NH 2 ) 2 CO in the preparation of a 16.2 percent by mass solution. Include your email address to get a message when this question is answered. Note that these percentages sum to equal 100.00% when appropriately rounded. For example, Daltons 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. Explanation: Aluminum oxide exists as a chemical compound of aluminum and oxygen with the The results of these measurements permit the calculation of the compounds percent composition, defined as the percentage by mass of each element in the compound. [Co(NH3)6]Cl3. (m is the abbreviation for molality) 7. Bicarbonate of soda (sodium hydrogen carbonate) is used in many commercial preparations. Question: Calculate the percent composition by mass of all the elements in urea, (NH2)2CO. These cookies track visitors across websites and collect information to provide customized ads. Al2 (SO4)3. H2O for a water molecule. The formula mass of ammonia is therefore (14.01 amu + 3.024 amu) = 17.03 amu, and its percent composition is: \[\mathrm{\%N=\dfrac{14.01\:amu\: N}{17.03\:amu\:NH_3}\times100\%=82.27\%}\], \[\mathrm{\%H=\dfrac{3.024\:amu\: N}{17.03\:amu\:NH_3}\times100\%=17.76\%}\]. First, find the molar mass of water by adding up the atomic masses of the elements. How to Calculate Mass Percent Composition Mass percent = (mass of chemical/total mass of compound) x 100 = (5 g/105 g) x 100. Mass percent tells you the percentage of each element that makes up a chemical compound. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. mass % = (mass of component/mass of total) x 100. Percent composition by element. Now, divide the mass of each element by the total mass to get the mass percentages: mass % H = (2 x 1.01) / 18.02 x 100%mass % H = 11.19%, mass % O = 16.00 / 18.02mass % O = 88.81%. What mass of Fe3+ ion is present in 3,450 mL of H2O, which has a density of 1.00 g/mL? The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. wikiHow is where trusted research and expert knowledge come together. The percent composition of a compound can be easily determined from the chemical formula of the compound. You can enter a formula manually or paste the formula copied from a web page or text document (including DOC or PDF file). Ionic compounds are composed of discrete cations and anions combined in ratios to yield electrically neutral bulk matter. A 2.30 M solution of urea (CO(NH_2)_2; FW = 60.0) in water has a density of 1.14 g/mL. Mass percent composition is also known percent by weight. What is the formula mass (amu) of calcium phosphate? (C = 12, O = 16, N = 14 and H = 1) CISCE ICSE Class 9. Hint: To solve this question we will use the formula of per cent by mass and it is calculated as the mass of the solute divided by mass of the solution (Solute + solvent) multiply by 100%. Aluminum sulfate, Al2(SO4)3, is an ionic compound that is used in the manufacture of paper and in various water purification processes. Textbook content produced by OpenStax College is licensed under a Creative Commons Attribution License 4.0 license. Vapor pressure of solvent (water) = P o = 26 mm of Hg, Mass of water (solvent) = W 1 = 100ml=100gram. The chemical formula for urea is . The two masses must be expressed in the same unit of mass, so conversions may be necessary. \%\ce O&=35.52\% \nonumber Calculate percent composition in terms of mass of a solution obtained by mixing 300 g of 25% solution of NH 4 NO 3 with 400 g of a 40% solution of solute X. Dividing the compounds mass by its molar mass yields: \[\mathrm{28.35\:\cancel{g}\:glycine\left(\dfrac{mol\: glycine}{75.07\:\cancel{g}}\right)=0.378\:mol\: glycine} \nonumber\]. Urea is the solute and water is the solvent in this question. tetraphosphorus decoxide. How do I determine the mass percentage of salt (NaCl) in a water-salt solution? We can derive the number of moles of a compound from its mass following the same procedure we used for an element in Example $\PageIndex{6}$: The molar mass of glycine is required for this calculation, and it is computed in the same fashion as its molecular mass. Temperature of water = 30C . Differentiate between molarity and molality. She has taught science courses at the high school, college, and graduate levels. Figure $\PageIndex{1}$ outlines the calculations used to derive the molecular mass of chloroform, which is 119.37 amu. This same approach may be taken considering a pair of molecules, a dozen molecules, or a mole of molecules, etc. As a reminder, the mole is an amount unit similar to familiar units like pair, dozen, gross, etc. Retrieved from https://www.thoughtco.com/mass-percent-composition-example-609567. Example $\PageIndex{11}$: Determining Percent Composition from a Molecular Formula. Support wikiHow by Step 2: Calculation of molecular mass for urea:-Molecular mass of Urea = 2 atomic mass of N + atomic mass of O + 4 atomic mass of H + atomic mass of C = 2 14 + 16 + 4 1 + 12 Molecular mass of Urea = 60 gm. The molar mass of a chemical compound is defined as the mass of a sample of that compound divided by the amount of substance in that sample, measured in moles. The key to calculating the formula mass of an ionic compound is to correctly count each atom in the formula and multiply the atomic masses of its atoms accordingly. What is the molecular mass (amu) for this compound? Element : Symbol : Atomic Mass # of Atoms : Mass Percent: Hydrogen: H: 1.00794: 4: 5.037%: . The answers add up to 100%, which was expected. Example 1: mass percent = (mass of chemical/total mass of compound) x 100 = (5 g/105 g) x 100. Using the lower indices in the formula, the mass of each element in one mole of the compound is first calculated. The cookies is used to store the user consent for the cookies in the category "Necessary". Percent composition of nitrogen in fertilizer. Example $\PageIndex{1}$: Computing Molecular Mass for a Covalent Compound. Quantitative units of concentration include molarity, molality, mass percentage, parts per thousand, parts per million, and parts per billion. To three significant digits, what is the mass percentage of iron in the compound $Fe_2O_3$? We can argue that modern chemical science began when scientists started exploring the quantitative as well as the qualitative aspects of chemistry. "% element" = "Mass of element"/"Molar mass of element"xx100% For urea, CO(NH_2)_2, the molar mass is 60.06*g*mol^-1. Additional Information: Urea has another name called carbamide. Videos in Mass Percent. Solution for Calculate the percent composition by mass of all the elements in urea, (NH2)2CO. 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. Mass percent composition describes the relative quantities of elements in a chemical compound. What is the molarity of a solution made by dissolving 332 g of C6H12O6 in 4.66 L of solution? How many $C_4H_{10}$ molecules are contained in 9.213 g of this compound? Step 1: Find the mass of the individual atoms. What are the individual ion concentrations and the total ion concentration in 0.66 M Mg(NO3)2? Figure $\PageIndex{1}$: The average mass of a chloroform molecule, CHCl3, is 119.37 amu, which is the sum of the average atomic masses of each of its constituent atoms. 22 System of Linear Equations Calculator, 33 System of Linear Equations Calculator, Simplifying Radical Expressions Calculator. Example $\PageIndex{8}$: Deriving Grams from Moles for a Compound. Mass % of B = Mass of B in a given compound / molecular mass 100. Mass percentage of . Generally, retirement benefits are based on four factors: Your age. What is the molar mass of C12H22O11? To Find: Molarity of solution =? Moles. \end{align*}\], \[\begin{align*} When a compounds formula is unknown, measuring the mass of each of its constituent elements is often the first step in the process of determining the formula experimentally. Our site uses cookies to improve your experience, to analyze traffic and to personalize ads. "This article is very helpful. The percent composition of a compound can be easily determined from the chemical formula of the compound. Example 1: mass percent = (2.01588/18.01528) x 100 = 0.11189 x 100 = 11.18%. 2. Helmenstine, Anne Marie, Ph.D. "How to Calculate Mass Percent Composition." Research source Parentheses ( ), square brackets [ ] and braces (curly brackets) { } can be used in the formulas. Percentage by mass of urea = (Mass of solute/Mass of solution) x 100 = (6/506) x 100 = 1.186%. Necessary cookies are absolutely essential for the website to function properly. % Composition of N . The cookie is set by GDPR cookie consent to record the user consent for the cookies in the category "Functional". Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. . Percentage nitrogen by mass= (Molar mass of nitrogen)/ (Molar mass of ammonium sulfate)*100. Corporate author : International Scientific Committee for the drafting of a General History of Africa Person as author : Ki-Zerbo, Joseph [editor] 132.1 = .212 = 21.2% nitrogen in ammonium sulfate. References Mass percent composition describes the relative quantities of elements in a chemical compound. Mass percent is also known as percent by weight or w/w%. The sum of all the mass percentages should add up to 100%. For example, if we know the mass and chemical composition of a substance, we can determine the number of moles and calculate number of atoms or molecules in the sample. If a solution is prepared by mixing 50 ml of vinegar into 300 ml of solution, what is the percentage by volume? \end{align*}\], \[\begin{align*} A similar unit of concentration is molality (m), which is defined as the number of moles of solute per kilogram of solvent, not per liter of solution: \[molality\: =\: \frac{moles\: solute}{kilograms\: solvent}\]. Calculate the mass of urea (NH 2 CONH 2) required in making 2.5 kg of 0.25 molal aqueous solution. Example 1: (5/105) x 100 = 0.04761 x 100 = 4.761%. Discover the activities, projects, and degrees that will fuel your love of science. To learn how to calculate mass percent when you don't know any of the masses involved, read on! Hint: The percent by mass is defined as pereent by mass of solute = mass of solute + mass of solvent mass of solute 100% Textbook . One mole of CO2 contains 1 mole of carbon atoms and 2 moles of oxygen atoms. Atomic Mass # of Atoms Mass Percent; Carbon: C: 12.0107 g/mol: 1: 19.9994%: Hydrogen: H: 4.0318 g/mol: 4: 6.7134% . Multiplying each element by its subscript gives you: Example 1: Add 2.01588 g/mol (the mass of two moles of Hydrogen atoms) with 15.9994 g/mol (the mass of a single mole of Oxygen atoms) and get 18.01528 g/mol. Performance cookies are used to understand and analyze the key performance indexes of the website which helps in delivering a better user experience for the visitors. Were committed to providing the world with free how-to resources, and even $1 helps us in our mission. 48.00 g (3 mole x 16.00 gram per mole) of O, mass % Na = 22.99 g / 84.01 g x 100 = 27.36 %, mass % H = 1.01 g / 84.01 g x 100 = 1.20 %, mass % C = 12.01 g / 84.01 g x 100 = 14.30 %, mass % O = 48.00 g / 84.01 g x 100 = 57.14 %, 32.00 g (2 mol x 16.00 gram per mole) of O, mass % C = (mass of 1 mol of carbon/mass of 1 mol of CO, mass % O = (mass of 1 mol of oxygen/mass of 1 mol of CO. You won't always be given the total mass of a mixture or solution. Divide mass of the chemical by mass of the compound and multiply by 100: 5.8/50.8 x 100 = 11.42%. Step 2: Analyze the mass of nitrogen in compound. If wikiHow has helped you, please consider a small contribution to support us in helping more readers like you. \%\ce O&=\mathrm{\dfrac{4\:mol\: O\times molar\: mass\: O}{molar\: mass\: \ce{C9H18O4}}\times 100=\dfrac{4\times 16.00\:g/mol} \nonumber{180.159\:g/mol}\times 100=\dfrac{64.00\:g/mol}{180.159\:g/mol}\times 100} \nonumber \\ For example, consider a gaseous compound composed solely of carbon and hydrogen. Calculate the molar mass of Ammonium Nitrate in grams per mole or search for a chemical formula or substance. Sign up for wikiHow's weekly email newsletter. What is the formula mass (amu) of this compound? It means 60 gm of urea contains 1 mole molecules of urea. Example 2: We want to rearrange the mass percent equation to solve for the unknown mass of the chemical: mass of the chemical = (mass percent*total mass of the compound)/100 = (15*175)/100. Advertisement cookies are used to provide visitors with relevant ads and marketing campaigns. Legal. Fertilizers supply the essential elements, nitrogen, phosphorus and potassium for plant growth. The formula for this compound indicates it contains Al3+ and SO42 ions combined in a 2:3 ratio. Potassium hydrogen carbonate ( KHCO3 ) has an average mass of 100.115 Da and is stable. Therefore, multiply the molecular mass of Hydrogen by 2, 1.00794 X 2 = 2.01588; and leave the molecular mass of Oxygen as is, 15.9994 (multiplied by one). This problem has been solved! What is the mass percent sucrose in a solution obtained by mixing 225 g of an aqueous solution that is . Our bodies synthesize protein from amino acids. Example #1: Calculate the mass percent of carbon within sodium carbonate, Na 2 CO 3. For members entering service on or after April 2, 2012, please . 11.3.1 Concentration in Commercial Applications Thinkstock. How many moles of NH4Br are present in 88.9 mL of a 0.228 M solution? Componen ts Mixing ratio by mass (%) SiO 2 46.96 CaO 39.77 PH 9.8 Fe 2O 3 2.79 Al 2O 3 3.95 TiO 2 0.22 K 2O 0.04 MgO 1.39 Na . Another way to specify an amount is percentage composition by mass (or mass percentage, % m/m). Parts per thousand is defined as follows: \[ppth\: =\: \frac{mass\: of\: solute}{mass\: of\: sample}\times 1000\]. The average molecular mass of a chloroform molecule is therefore equal to the sum of the average atomic masses of these atoms. The elemental makeup of a compound defines its chemical identity, and chemical formulas are the most succinct way of representing this elemental makeup. How would I calculate the mass percent of a MgBr2 solution that contains 5.80g of MgBr2 in 45.0g of solution? Video $\PageIndex{4}$: A video overview of how to calculate percent composition of a compound based on its chemical formula. Compound. If the formula used . This is a worked example problem showing how to calculate mass percent composition. Then, divide the mass of the chemical by the total mass of compound. For these sorts of applications, the percent composition of a compound is easily derived from its formula mass and the atomic masses of its constituent elements. Plug the values to calculate the mass percentage of N: Its formula is NaHCO3. Again, make sure your mass percents add up to 100%. This cookie is set by GDPR Cookie Consent plugin. After this, it calculates the total number of elements (N-atoms). Using formula for mass percentage as under: (Weight/Volume)% = (Weight of Solute/Volume of Solution)*100 (Weight/Volume)% = (3.6/140)*100 (Weight/Volume)% = 2.57%. Now, the molar mass of the molecule can be calculated according to the number of atoms present in the molecule. 11.11 g of urea (NH 2 CONH 2) was dissolved in 100 g of water. The number of molecules in a given mass of compound is computed by first deriving the number of moles, as demonstrated in Example $\PageIndex{8}$, and then multiplying by Avogadros number: Using the provided mass and molar mass for saccharin yields: \[\mathrm{0.0400\:\cancel{g}\:\ce{C7H5NO3S}\left(\dfrac{\cancel{mol}\:\ce{C7H5NO3S}}{183.18\:\cancel{g}\:\ce{C7H5NO3S}}\right)\left(\dfrac{6.022\times10^{23}\:\ce{C7H5NO3S}\:molecules}{1\:\cancel{mol}\:\ce{C7H5NO3S}}\right)}\\ To calculate the percentage composition of an element in a compound, we use the equation: In 1 mole of urea, 2 moles of nitrogen atoms are there. In this case, several readers have written to tell us that this article was helpful to them, earning it our reader-approved status. ", Unlock expert answers by supporting wikiHow, https://chem.libretexts.org/Bookshelves/Analytical_Chemistry/Supplemental_Modules_(Analytical_Chemistry)/Quantifying_Nature/Density_and_Percent_Compositions, https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map%3A_Introductory_Chemistry_(Tro)/06%3A_Chemical_Composition/6.06%3A_Mass_Percent_Composition_of_Compounds, https://www.omnicalculator.com/chemistry/mass-percent, https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map%3A_Introductory_Chemistry_(Tro)/06%3A_Chemical_Composition/6.07%3A_Mass_Percent_Composition_from_a_Chemical_Formula, http://sciencenotes.org/wp-content/uploads/2015/01/Periodic-Table-Color.png, https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map%3A_Introductory_Chemistry_(Tro)/13%3A_Solutions/13.05%3A_Specifying_Solution_Concentration-_Mass_Percent, (Calculate Mass Percent). As long as we know the chemical formula of the substance in question, we can easily derive percent composition from the formula mass or molar mass. Molar mass of (NH2)2CO is 60.0553 g/mol. This cookie is set by GDPR Cookie Consent plugin. Performing the calculation, we get: This is consistent with the anticipated result. Example 2: Add all of the calculated molar masses together: Carbon + Hydrogen + Oxygen = 72.0642 + 12.09528 + 95.9964 = 180.156 g/mol. What is the percentage of N in urea? The percentage yield formula is calculated to be the experimental yield divided by theoretical yield multiplied by 100. . Example $\PageIndex{1}$: What is the mass percentage of Fe in a piece of metal with 87.9 g of Fe in a 113 g sample? This approach is perfectly acceptable when computing the formula mass of an ionic compound. Rearranging to solve for the mass of solute, \[mass\: solute =\: \frac{(15.0\, ppm)(240.0\: g\: solution)}{1,000,000}=0.0036g=3.6\, mg\]. Molarity is moles per liter, whereas molality is moles per kilogram of solvent. In the previous section, we discussed the relationship between the bulk mass of a substance and the number of atoms or molecules it contains (moles). Now that the equation is filled in, simply solve to calculate the mass percent. In unit 2, we used Avogadros number to convert between mass of an element, moles of an element,and number of atoms 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 substances mass.s, Example $\PageIndex{7}$: Deriving Moles from Grams for a Compound. Analytical cookies are used to understand how visitors interact with the website. View solution. The mass of the chemical youre interested in is the mass given in the problem. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. Example 2: mass percent = (molar mass of the element/total molecular mass of compound) x 100 = (72.0642/180.156) x 100 = 0.4000 x 100 = 40.00%. For members entering service before April 2, 2012, please enter the average of your highest thirty-six consecutive months of annual regular compensation (base salary). To calculate mass percent, start by identifying the mass of the chemical-in-question. One of these amino acids is glycine, which has the molecular formula C2H5O2N. Helmenstine, Anne Marie, Ph.D. (2020, August 28). But what if the chemical formula of a substance is unknown? a) The chemical formula of ammonium phosphate is N H 4 3 P O 4 and Potassium nitrate is K N O 3 and ammonium sulfate is N H 4 2 S O 4 . The recommended daily dietary allowance of vitamin C for children aged 48 years is 1.42 104 mol. Calculate the percentage by mass of nitrogen in the bag of fertilizer. 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. Substituting, \[\frac{0.6g\, Pb}{277g\, solution}\times 1000=2.17\, ppth\]. In this example, you are given the total mass and the percentage you want, but are asked to find the amount of solute to add to the solution. Now, we can useAvogadros number and formula mass (also called molecular weight)to convent between mass of a sample, moles, and number of molecules. This information can be crucial for understanding the properties and behavior of the compound, as well as for identifying it. Out of these, the cookies that are categorized as necessary are stored on your browser as they are essential for the working of basic functionalities of the website. What volume of 3.99 M H2SO4 is needed to obtain 4.61 mol of H2SO4? Mass Percent Calculator. Calculate the molarity and molality of the solution. Calculate the percent mass of urea in this solution. For a solution, mass percent equals the mass of an element in one mole of the compound divided by the molar mass of the compound, multiplied by 100%. Progress. Hard. Copyright 2017-2023ezcalc.me. For instance, if you added 50 grams of NaCl to 1000 grams of water, that mass percent would be 50/1050 x 100 = 4.76%. Comparing the percent composition achieved practically to the theoretical value obtained from the formula of the compound makes it possible to determine the purity of a chemical. Solving for Mass Percent When Given Masses, {"smallUrl":"https:\/\/www.wikihow.com\/images\/thumb\/a\/a2\/Calculate-Mass-Percent-Step-1.jpg\/v4-460px-Calculate-Mass-Percent-Step-1.jpg","bigUrl":"\/images\/thumb\/a\/a2\/Calculate-Mass-Percent-Step-1.jpg\/aid2931007-v4-728px-Calculate-Mass-Percent-Step-1.jpg","smallWidth":460,"smallHeight":345,"bigWidth":728,"bigHeight":546,"licensing":"

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