Course Activity: Charges on Transition Metal lons5 of 6Part FThe compound iron chloride can exist with either iron(II) ions or iron(IIl) ions. Conduct Internet research tolearn about the differences between iron(II) chloride and iron(III) chloride. Give the chemical formula foreach compound. Describe their appearance and uses. Based on your findings, are these two forms of thesame compound, or are they two completely different compounds?X,Font SizesAE星E 三ヨSuperscriptparametersiron(II) chlorideiron(III) chloridechemical formulaappearanceusesCharacters used: 88 / 15000Rart C Part EIn each test, iron(II) sulfate and iron(III) nitrate were combined with the same substance or substances.However, the sulfate and nitrate parts of the compounds didn't participate in any of the chemicalreactions; only the iron ions reacted. Comparing the results for each pair of tests, what can you concludeabout the iron(II) and iron(IIl) ions?BU x'X,Font SizesA目三三三Characters used: 0/ 15000Part FThe compound iron chloride can exist with either iron(II) ions or iron(III) ions. Conduct Internet research tolearn about the difforencon iron/l) chloride and iron/II\ chloride. Give the chemical formula for

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Part F The compound iron chloride can exist with either iron(II) ions or iron(IIl) ions. Conduct Internet research to learn about the differences between iron(lI) chloride and iron(III) chloride. Give the chemical formula for each compound. Describe their appearance and uses. Based on your findings, are these two forms of the same compound, or are they two completely different compounds? BIU X, Font Sizes A - 三 E三ヨ Superscript parameters iron(II) chloride iron(III) chloride chemical formula appearance uses Characters used: 88 / 15000

Part F The compound iron chloride can exist with either iron(II) ions or iron(IIl) ions. Conduct Internet research to learn about the differences between iron(lI) chloride and iron(III) chloride. Give the chemical formula for each compound. Describe their appearance and uses. Based on your findings, are these two forms of the same compound, or are they two completely different compounds? BIU X, Font Sizes A - 三 E三ヨ Superscript parameters iron(II) chloride iron(III) chloride chemical formula appearance uses Characters used: 88 / 15000

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter2: Chemical Compounds

Section: Chapter Questions

Problem 143QRT: The present average concentration (mass percent) of magnesium ions in seawater is 0.13%. A chemistry...

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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.
An adult human body contains 6.0 L blood, which contains about 15.5 g hemoglobin per 100.0 mL blood. The molar mass of hemoglobin is approximately 64,500 g/mol and there is 4 mol iron per 1 mol hemoglobin. A news item claims that there is sufficient iron in the hemoglobin of the body that this iron, if it were in the form of metallic iron, could make a 3-in. iron nail that weighs approximately 3.7 g. Show sufficient calculations to either support or refute the claim.
Two general chemistry students working together in the lab weigh out 0.832 g of CaCl2 2 H2O into a crucible. After heating the sample for a short time and allowing the crucible to cool, the students determine that the sample has a mass of 0.739 g. They then do a quick calculation. On the basis of this calculation, what should they do next? (a) Congratulate themselves on a job well done. (b) Assume the bottle of CaCl2 2 H2O was mislabeled; it actually contained something different. (c) Heat the crucible again, and then reweigh it.
3.116 The simplest approximate chemical formula for the human body could be written as C728H4850O1970N104Ca24P16K4S4Na3Cl2Mg. Based on this formula, describe how you would rank by mass the ten most abundant elements in the human body.
The age of the universe is unknown, but some conclude from measuring Hubbles constant that the age is about 18 billion years old, which is about four times the age of Earth. If so, calculate the age of the universe in seconds. If you had a sample of carbon with the same number of carbon atoms as there have been seconds since the universe began, determine whether you could measure this sample on a laboratory balance that can detect masses as small as 0.1 mg.
4-102 Aspartame, an artificial sweetener used as a sugar substitute in some foods and beverages, has the molecular formula C14H18N2O5. (a) How many mg of aspartame are present in 3.72 × 1026 molecules of aspartame? (b) Imagine you obtain 25.0 mL of aspartame, which is known to have a density of 1.35 g/mL. How many molecules of aspartame are present in this volume? (c) How many hydrogen atoms are present in 1.00 mg of aspartame? (d) Complete the skeletal structure of aspartame, where all the bonded atoms are shown but double bonds, triple bonds, and/or lone pairs are missing. (e) Identify the various types of geometries present in each central atom of aspartame using VSEPR theory. (f) Determine the various relative bond angles associated with each central atom of aspartame using VSEPR theory. (g) What is the most polar bond in aspartame? (h) Would you predict aspartame to be polar or nonpolar? (i) Is aspartame expected to possess resonance? Explain why or why not. (j) Consider the combustion of aspartame, which results in formation of NO2(g) as well as other expected products. Write a balanced chemical equation for this reaction. (k) Calculate the weight of C02(g) that can be prepared from 1.62 g of aspartame mixed with 2.11 g of oxygen gas.
When the supply of oxygen is limited, iron metal reacts with oxygen to produce a mixture of FeO and Fe2O3. In a certain experiment, 20.00 g iron metal was reacted with 11.20 g oxygen gas. After the experiment, the iron was totally consumed, and 3.24 g oxygen gas remained. Calculate the amounts of FeO and Fe2O3 formed in this experiment.
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?
3.83 For the reaction of nitrogen, N2, and hydrogen, H2, to form ammonia, NH3, a student is attempting to draw a particulate diagram, as shown below. Did the student draw a correct representation of the reaction? If not, what was the error the student made?