Concept explainers
(a)
Interpretation:
The percent composition of iron in
(a)
Explanation of Solution
The percent composition of any substance is calculated by dividing the mass of substance in a sample by total mass of the sample. This ratio is multiplied by
To determine the percent composition let the
The mass of Fe from periodic table is
The mass of O from periodic table is
Therefore, the total mass for
Now, the percent composition of Fe is,
(b)
Interpretation:
The percent iron in
(b)
Explanation of Solution
To determine the percent composition let the sample size be
The mass of Fe from periodic table is
The mass of O from periodic table is
Therefore, the total mass for
Now, the percent composition of Fe is,
(c)
Interpretation:
The percent iron in
(c)
Explanation of Solution
To determine the percent composition, let the sample size be
The mass of Fe from periodic table is
The mass of O from periodic table is
Therefore, the total mass for
Now, the percent composition of Fe is,
(d)
Interpretation:
The percent iron in
(d)
Explanation of Solution
To determine the percent composition, let the sample size be
The mass of Fe from periodic table is
The mass of C from periodic table is
The mass of O from periodic table is
Therefore, the total mass for
Now, the percent composition of Fe is,
Out of all the iron minerals, wustite
Want to see more full solutions like this?
Chapter 4 Solutions
INTRO TO CHEMISTRY EBK ACCESS CARD >I<
- Chlorine exists mainly as two isotopes, 37Cl and 33Cl. Which is more abundant? How do you know?arrow_forwardThe sugar sucrose, which is present in many fruits and vegetables, reacts in the presence of certain yeast enzymes to produce ethanol and carbon dioxide gas. Balance the following equation for this reaction of sucrose. C12H22O11(aq) + H2O(l) C2H5OH(aq) + CO2(g)arrow_forwardBoron forms an extensive series of compounds with hydrogen, all with the general formula BxHy. To analyze one of these compounds, you burn it in air and isolate the boron in the form of B2O3 and the hydrogen in the form of water. You find that 0.1482 g BxHy gives 0.4221 g B2O3 when burned in excess O2. Determine the empirical I formula of BxHy.arrow_forward
- Chalky, white crystals in mineral collections are often labeled borax, which has the molecular formula Na2B4O7 10H2O, when actually they are partially dehydrated samples with the molecular formula Na2B4O7 5H2O, which is more stable under the storage conditions. Real crystals of borax are colorless and transparent. (a) Calculate the percent mass that the mineral has lost when it partially dehydrates. (b) Is the percent boron by mass the same in both compounds?arrow_forwardPhosphorus occurs naturally in the form of fluorapatite, CaF2 3Ca3(PO4)2. The dot indicates 1 part CaF2 to 3 parts Ca3(PO4)2. This mineral is reacted with an aqueous solution of H2SO4 in the preparation of a fertilizer. The products are phosphoric acid, hydrogen fluoride, and gypsum, CaSO4 2H2O. Write the balanced equation describing this process.arrow_forward4.28 One of the steps in the manufacture of nitric acid is the oxidation of ammonia shown in this equation: 4NH3(g)+5O2(g)4NO(g)+6H2O(g) If 43.0 kg of NH3 reacts with 35.4 kg of O2, what mass of NO forms?arrow_forward
- The reaction between potassium chlorate and red phosphorus takes place when you strike a match on a matchbox. If you were to react 52.9 g of potassium chlorate (KCIO3) with excess red phosphorus, what mass of tetraphosphorus decaoxide (P4O10) could be produced? KClO3(s)+P4(s)P4O10(s)+KCl(s)(unbalanced)arrow_forward4.106 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what mass of CO2 is evolved during the process.arrow_forwardIn a reaction, 1.2 g element A reacts with exactly 3.2 g oxygen to form an oxide, AOx; 2.4 g element A reacts with exactly 3.2 g oxygen to form a second oxide, AOy. (a) Determine the ratio x:y. (b) If x = 2, determine what the identity of element A might be.arrow_forward
- Balance the following chemical equations. a. H2S + O2 SO2 + H2O b. Ni + HCl NiCl2 + H2 c. IBr + NH3 NH4Br + NI3 d. C2H6 + O2 CO2 + H2Oarrow_forward4.48 Elemental phosphorous is used in the semiconductor industry. It can be obtained from an ore called fluoroapatite via reaction with SiO2 and C: 4Ca5( PO4)3F+18SiO2+30C3P4+30CO+18CaSiO3+2CaF2 Suppose a particular semiconductor production plant requires 1500 kg of P4. If the recovery of P4 from this reaction is 73% efficient, what mass of fluoroapatite is needed?arrow_forwardThe deep blue compound Cu(NH3)4S04 is made by the reaction of copper(II) sulfate and ammonia CuSO4(aq) + 4 NH3(aq) Cu(NH3)4SO4(aq) (a) If you use 10.0 g of CuSO4 and excess NH3, what is the theoretical yield of Cu(NH3)4SO4? (b) If you isolate 12.6 g of Cu(NH3)4SO4, what is the percent yield of Cu(NH3)4SO4?arrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning