Answered: Part A Calculate the mass percent… | bartleby

Chemistry: An Atoms First Approach

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter5: Stoichiometry

Section: Chapter Questions

Problem 168CP

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Question

Please answer question 13 Part B, C, and D

Part A
Iron is mined from the earth as iron ore. Common
ores include Fe2 O3 (hematite), Fe3 O4
(magnetite), and FECO3 (siderite).
Calculate the mass percent composition of iron for Fe2 O3 (hematite).
Express the mass percent to two decimal places.
Part B
Calculate the mass percent composition of iron for Fe3 O4 (magnetite).
Express the mass percent to two decimal places.
?
%

Iron is mined from the earth as iron ore. Common
Part C
ores include Fe2 O3 (hematite), Fe3 O4
(magnetite), and FECO3 (siderite).
Calculate the mass percent composition of iron for FeCO3 (siderite).
Express the mass percent to two decimal places.
?
%
Part D
Which ore has the highest iron content?
hematite
magnetite
siderite

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A substance X2Z has the composition (by mass) of 40.0% X and 60.0% Z. What is the composition (by mass) of the compound XZ2?
You have a pure sample of apholate, C12H24N9P3, a highly effective commercial insecticide. Calculate the molar mass of apholate. Calculate the mass of N in 100. g apholate. A sample containing 250.0 mg apholate is sprayed on an agricultural field. Calculate the mass of phosphorus in this sample of apholate; express your result in grams. Calculate the number of phosphorus atoms in this sample of apholate.
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The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry textbook estimates that if 1.00 × 108 tons Mg were taken out of the sea each year, it would take one million years for the Mg concentration to drop to 0.12%. Do sufficient calculations to either verify or refute this statement. Assume that Earth is a sphere with a diameter of 8000 mi, 67% of which is covered by oceans to a depth of 1 mi, and that no Mg is washed back into the oceans at any time.
Solid copper(II) chloride forms a hydrate of formula CuCl2 ⋅ xH2O. A student heated a sample of hydrated copper(II) chloride, in order to determine the value of x. The following results were obtained: mass of crucible = 16.221 g mass of crucible and hydrated copper(II) chloride = 18.360 g mass of crucible and anhydrous copper(II) chloride = 17.917 g At. Mass: Cu 63.55 Cl 35.45 H 1.008 O 16.00 1. Calculate percentage of anhydrous copper(II) chloride (answer must have 4 sig. fig)
Most fertilizers consist of nitrogen-containing compounds such as NH3, CO(NH2)2, NH4NO3, and (NH4)2SO4. Plants use the nitrogen content in these compounds for protein synthesis. (Express your answer using four significant figures.) Calculate the mass percent composition of nitrogen in NH3. Calculate the mass percent composition of nitrogen in CO(NH2)2. Calculate the mass percent composition of nitrogen in NH4NO3. Calculate the mass percent composition of nitrogen in (NH4)2SO4. Which fertilizer has the highest nitrogen content?
You can also calculate percent composition from a formula. This is similar to percent abundance in that what percentage of a compound is each element. If you look at the compound and tell how many of each element there is, you calculate the percent composition. Ex. Calculate the total mass of a compound just like before - CO2 C = 1 X 12 = 12g O = 2 X 16 = 32g 12+32 = 44g Then take the mass of each and divide by the total. 12/44 X100 = 27% carbon 32/44 X 100 = 73% oxygen CO2 is 27% carbon and 73% oxygen. What percentage of Na3PO4 is sodium (Na)?
Solid copper(II) chloride forms a hydrate of formula CuCl2 ⋅ xH2O. A student heated a sample of hydrated copper(II) chloride, in order to determine the value of x. The following results were obtained: mass of crucible = 16.221 g mass of crucible and hydrated copper(II) chloride = 18.360 g mass of crucible and anhydrous copper(II) chloride = 17.917 g At. Mass: Cu 63.55 Cl 35.45 H 1.008 O 16.00 1. Calculate percentage of H2O (answer must have 4 sig. fig)
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The mineral iron pyrite (FeS2), typically, has a mass percentage of what is known as fool’s gold of 90-95%. The actual percentage in a sample can be determined using gravimetric analysis. To find the % mass of FeS2 the sulphur in FeS2 is firstly converted to sulphate (SO42-). These sulphate ions (SO42-) is mixed with an excess of barium chloride (BaCl2) to form barium sulphate (BaSO4), according to the following reaction: Ba2+(aq) + SO42- (aq) à BaSO4 (s) When the reaction has gone to completion, the BaSO4 precipitate is collected in a filter paper and carefully washed. The filter paper and its contents are then transferred to a crucible. The crucible and its contents are heated until constant mass is achieved. The data for the analysis of a mineral sample is shown in the table below: Initial Mass of mineral sample 17.5 g Mass of crucible and filter paper 144.60 g Mass of crucible, filter paper and dry BaSO4 196.89 g Molar mass…

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