To help farmers and gardeners, commercial fertilizers have a big three-number "NPK" label on the bag that gives the amounts of three key plant nutrients:nitrogen, phosphorus and potassium. For example, a bag of "10-10-10° fertilizer has 10% by mass nitrogen, 10% by mass potassium as potash (K₂O), and10% by mass phosphorus as phosphate (P₂O).Suppose a certain fertilizer has the following composition:Ingredient* ((NH,),CO)potassium sulfate (K,SO₂)potassium chloride (KC1)0%ureainert ingredientspercent by mass40%15%What should the first (nitrogen) number on the bag label be? That is, calculate the percent by mass of nitrogen in this fertilizer. Round your answer to thenearest percent.D.P9%36%EG

Consider that the total mass of the mixture is 100g. Percent by mass of urea (fertilizer) is 40%.…

To help farmers and gardeners, commercial fertilizers have a big three-number "NPK" label on the bag that gives the amounts of three key plant nutrients: nitrogen, phosphorus and potassium. For example, a bag of "10-10-10" fertilizer has 10% by mass nitrogen, 10% by mass potassium as potash (K,O), and 10% by mass phosphorus as phosphate (P.O.) Suppose a certain fertilizer has the following composition: Ingredient ((NH,)_CO) potassium sulfate (K,SO,) potassium chloride (KC) urea inert ingredients percent by mass X 40% 9% 36% 15% What should the first (nitrogen) number on the bag label be? That is, calculate the percent by mass of nitrogen in this fertilizer. Round your answer to the nearest percent. 5

To help farmers and gardeners, commercial fertilizers have a big three-number "NPK" label on the bag that gives the amounts of three key plant nutrients: nitrogen, phosphorus and potassium. For example, a bag of "10-10-10" fertilizer has 10% by mass nitrogen, 10% by mass potassium as potash (K,O), and 10% by mass phosphorus as phosphate (P.O.) Suppose a certain fertilizer has the following composition: Ingredient ((NH,)_CO) potassium sulfate (K,SO,) potassium chloride (KC) urea inert ingredients percent by mass X 40% 9% 36% 15% What should the first (nitrogen) number on the bag label be? That is, calculate the percent by mass of nitrogen in this fertilizer. Round your answer to the nearest percent. 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4. a) A given inorganic compound contains only silicon (Si) and hydrogen (H). If the mass percentage of Si in this compound is 90.28%, what is the mass percentage of H in this compound? ( Hint: Mass% values of all the elements in a given compound should ultimately add up to what % ? Show work. Include units (the % symbol) and observe proper sig figs. b) What is the empirical formula of the compound in part a) ? Hint: You are going to have to refer to the periodic table to find molar masses of Si and H at some point during this calculation. Slide # 48 in Chapter 3 will be helpful to refer to. At each step, make sure to include at least four decimal places to avoid over- / under-estimating the empirical formula values.
5. Consider the following reaction: NazPO4(aq) + Ba(NO:)2(aq) → Baş(PO4)2(s) + NaNO3. Suppose a solution containing 3.5g Na3PO4 is mixed with a solution containing 6.40g Ba(NO3)2, how many grams of Ba3(PO4)2 can be formed? 6. Consider the reaction: 2Sb(s) + 312(s) → 2Sbl;(s). Determine the limiting reactant and the theoretical yield when 1.20g of Sb and 2.4g of Iz are mixed? What mass of the excess reactant is left when the reaction is complete?
A three-step process for producing molten iron metal from Fe203 is: 1. ЗFe203 + со — 2Fe3О4 + CO2 2. Fe304 + CO— ЗFeО + CO2 3. Feo + CO → Fe + CO2 Assuming that the reactant CO is present in excess and that the yields, respectively, for the three steps are 81.9%, 65.9% and 60.5%, what mass of iron metal would be produced from 360. kg of Fe,03?
I = 126.90g /mol C = 12.01g /mol O = 16.00g /mol
Straight-chain, saturated carboxylic acids, a class of hydrocarbons, has the general formula CnH2n+1COOH where n is an integer than ranges from 1 to 18. What would be the %C by mass if n = 14 ? Atomic weights: C=12.01, H=1.01, O=15.99.
Copper(II) sulfate forms several hydrates with the general formula CuSO4·xH2O, where x is an integer. If the hydrate is heated, the water can be driven off, leaving pure CuSO4 behind. Suppose a sample of a certain hydrate is heated until all the water is removed, and it's found that the mass of the sample decreases by 31.%. Which hydrate is it? That is, what is x?
What mass of zinc sulfide 19 5. The addition of concentrated hydrochloric acid to manganese (IV) oxide leads to the production of chlorine gas. 4 HCl(aq) + MnO2(g) MnCl2(aq) + Cl2(g) + 2H2O1) What mass of Cl can be obtained when 4.76 • 102 g of HCl react with sufficient MnO2?
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33. Sulfurous acid is unstable in aqueous solution and gradually decomposes to water and sulfur dioxide gas (which explains the choking odor associated with sulfurous acid solutions). H, SO3 (aq) – + H20(1) + SO2 (g) If 4.25 g of sulfurous acid undergoes this reaction, what mass of sulfur dioxide is released?
Abel reacts copper with silver nitrate and recovers 5.2 g Ag. However, after mass to mass stoichiometry , he discovers that the maximum yield of silver should have been 9.5 g. What is his percent yield?
Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the reaction of an acid on an alkaline earth metal peroxide, such as barium peroxide. BaO2 + HCl ---> H2O2 + BaCl2 What amount of hydrogen peroxide should result when 1.17 g of barium peroxide is treated with 28.0 mL of hydrochloric acid solution containing 0.0288 g of HCl per mL? _____ g H2O2
Researchers obtained the following data from experiments to find the molecular formula of benzocaine, a local anesthetic, which contains only carbon, hydrogen, nitrogen, and oxygen. Complete combustion of a 3.54 gg sample of benzocaine with excess O2O2 formed 8.49 gg CO2CO2 and 2.14 gg H2OH2O. Another sample of mass 2.35 gg was found to contain 0.199 gg of NN. The molar mass of benzocaine was found to be 165 Find the molar formula of benzocaine. Express your answer as a chemical formula.