GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
11th Edition
ISBN: 9780134566030
Author: Petrucci
Publisher: PEARSON
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Chapter 23, Problem 44E
Interpretation Introduction
Interpretation:
The chemical equations for the given process should be determined.
Concept introduction:
A chemical equation refers to the symbolic representation of a given
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Chapter 23 Solutions
GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
Ch. 23 - By means of orbital diagrams, write electron...Ch. 23 - Arrange the following species according to the...Ch. 23 - Describe how the transition elements compare with...Ch. 23 - With only minor irregularities, the melting points...Ch. 23 - Why do the atomic radii vary so much for two...Ch. 23 - Prob. 6ECh. 23 - Which of me first transition series elements...Ch. 23 - Why is the number of common oxidation states for...Ch. 23 - As a group, the lanthanides are more reactive...Ch. 23 - The maximum difference in standard reduction...
Ch. 23 - Complete and balance the following equations. If...Ch. 23 - By means of e chemical equation, give an example...Ch. 23 - Prob. 13ECh. 23 - Prob. 14ECh. 23 - Prob. 15ECh. 23 - Prob. 16ECh. 23 - Prob. 17ECh. 23 - According to Figure 23-8, G decreases with...Ch. 23 - Prob. 19ECh. 23 - Prob. 20ECh. 23 - Write plausible half-equations to represent each...Ch. 23 - Prob. 22ECh. 23 - Use electrode potential data from this chapter or...Ch. 23 - You are given these three reducing agents: Zn(s);...Ch. 23 - Prob. 25ECh. 23 - Prob. 26ECh. 23 - Prob. 27ECh. 23 - Use data from the text to construct a standard...Ch. 23 - When a soluble lead compound is added to a...Ch. 23 - Prob. 30ECh. 23 - Prob. 31ECh. 23 - If CO2(g) under pressure is passed into...Ch. 23 - Use equation (23.19) to determine [Cr2O72] in a...Ch. 23 - If a solution is prepared by dissolving 1.505 g...Ch. 23 - Prob. 35ECh. 23 - Prob. 36ECh. 23 - Prob. 37ECh. 23 - Prob. 38ECh. 23 - Will reaction (23.25) still be spontaneous in the...Ch. 23 - Prob. 40ECh. 23 - Prob. 41ECh. 23 - Prob. 42ECh. 23 - Prob. 43ECh. 23 - Prob. 44ECh. 23 - Prob. 45ECh. 23 - Prob. 46ECh. 23 - Prob. 47ECh. 23 - At 400C , 2Hg(I)+O2(g)2HgO(s) for the reaction...Ch. 23 - Prob. 49ECh. 23 - Prob. 50ECh. 23 - Prob. 51ECh. 23 - Prob. 52ECh. 23 - Prob. 53ECh. 23 - Prob. 54ECh. 23 - The text notes that in small quantities, zinc is...Ch. 23 - Prob. 56ECh. 23 - What formulas would you expect for the metal...Ch. 23 - For the straight-line graphs in Figure 23-8...Ch. 23 - Prob. 59ECh. 23 - Prob. 60ECh. 23 - Prob. 61ECh. 23 - Prob. 62ECh. 23 - Prob. 63ECh. 23 - Prob. 64ECh. 23 - Prob. 65ECh. 23 - Prob. 66ECh. 23 - Prob. 67ECh. 23 - Prob. 68ECh. 23 - Prob. 69ECh. 23 - Prob. 70ECh. 23 - Prob. 71ECh. 23 - For a coordination number of four, the radius of...Ch. 23 - Prob. 73ECh. 23 - Prob. 74FPCh. 23 - Several transition metal ions are found in cation...Ch. 23 - Prob. 76SAECh. 23 - Briefly describe each of the following ideas. phe...Ch. 23 - Prob. 78SAECh. 23 - Prob. 79SAECh. 23 - Prob. 80SAECh. 23 - Prob. 81SAECh. 23 - Prob. 82SAECh. 23 - Prob. 83SAECh. 23 - Prob. 84SAECh. 23 - Prob. 85SAECh. 23 - Provide the missing name or formula for the...Ch. 23 - Prob. 87SAECh. 23 - Prob. 88SAECh. 23 - Prob. 89SAECh. 23 - Prob. 90SAE
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- A 1.000-g sample of limestone gave a precipitate of Fe2O3 and Al2O3, weighing 0.0800 g. The precipitate of mixed oxides was fused with KHSO4, dissolved in sulfuric acid, and passed through a Jones reductor. The iron was titrated with 20.00 mL of 0.0100 N permanganate solution. Calculate the percentage of FeO and Al2O3 in the limestone (assume all iron present as FeO in the original sample)arrow_forwardA 5.70 g iron ore was dissolved in concentrated HCl. After the dissolution, the resulting solution was made basic by adding 6.0 M NaOH slowly until the solution is slightly turbid. Urea was then added and the solution was heated for 3 hours. The precipitate was filtered using an ashless filter paper and ignited to form Fe2O3 (159.69 g/mol). The mass of precipitate is 2.1 g. Find the % Fe3O4 (231.54 g/mol) in the iron ore sample.arrow_forwardTo determine the amount of magnetite, Fe3O4, in an impure ore, a 1.5419 g sample is dissolved in concentrated HCl, giving a mixture of Fe2+and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+and diluting with water, Fe3+is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing, and igniting the precipitate provides 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample.arrow_forward
- To determine the amount of magnetite, Fe3O4, in an impure ore, a 1.5419-g sample is dissolved in concentrated HCl, giving a mixture of Fe2+ and Fe3+. After adding HNO3 to oxidize Fe2+ to Fe3+ and diluting with water, Fe3+ is precipitated as Fe(OH)3 by adding NH3. Filtering, rinsing, and igniting the precipitate provides 0.8525 g of pure Fe2O3. Calculate the %w/w Fe3O4 in the sample. Hint: The analyte is Fe.arrow_forward3. When the first half of the solution containing NaCI and KCI, obtained from 2 g of a feldspar sample, is precipitated with H,PtCl, in an alcoholic medium, the precipitate of K,PICI, is 486 mg. When the other half of the solution is precipitated with AGNO3, 430.5 mg AgCl is formed. Calculate the percentage of Na,O and K,0 in the sample. (H :1 g/mol; Na : 23 g/mol; Cl : 35.5 g/mol; K: 39 g/mol; Pt : 195 g/mol; Ag : 108 g/mol; N : 14 g/mol; 0: 16 g/mol)arrow_forwardCerium(IV) is a strong oxidizing agent commonly used in redox titrations. Which of the following statemnt is/are NOT true for cerium(IV)? I.A Ce** standard solution is prepared using primary-standard-grade ammonium hexanitratocerate(IV), (NH4)2Ce(NO3); dissolved in hot hydrochloric acid solution. II. Ce** is yellow and Ce3* is colorless. The color change is abrupt enough that Ce** can serve as its own indicator. III. Ce**/Ce* exists in different formal potential in different acids due to the interaction of the anions part of the acid with Ce** IV. Analysis of many organic analyte such as alcohol, aldehydes can be determined using Ce**by an indirect method involving a technique of back titration of unreacted excess Ce*with standard iron Il titrant O a. 1,11,IV O b. 1, II, III O. I,II O d. II, II, IV O e. I, II, III, IVarrow_forward
- 1. A 0.9882 gram sample of iron ore is dissolved, the iron reduced to Fe2+, and the solution was titrated with 36.40 mL of 0.02065 M KMnO4 in acid solution. (a) Write the titration reaction. (b) Calculate the %FeO (M.M. = 71.85) in the sample. 2. A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the solution acidified and excess KI added. The liberated I2 requires 44.86 mL of the Na2S2O3 for titration. (a) Write the titration reaction. (b) Calculate the molarity of the titrant solution.arrow_forwardA 600.0 mg sample consisting of only CaC2O4and Mg C2O4is heated at 500oC converting the two salts to CaCO3and MgCO3. The sample weighs 465.0 mg. If the sample had been heated at 900oC where the products are CaO and MgO, what would the mixture of oxides weigh? Write in a padpaper and show the clear and complete solutionarrow_forward(i) Name the method of refining of metals such as Germanium.(ii) In the extraction of Al, impure Al2O3 is dissolved in cone. NaOH to form sodium aluminate and leaving impurities behind. What is the name of this process?(iii) What is the role of coke in the extraction of iron from its oxides?arrow_forward
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