1. What type of reactions are the following reactions?REACTIONТYРENi(s) + 2 HNO3(aq) Ni(NO3)2(aq) + H2(g)2 KCI(aq) + Pb(NO3)22 KNO3(aq) + PbCl2(s)2. Complete and balance the following equations:TYPEREACTANTSPRODUCTSNaBr(aq) +Cl2(aq)Single Replacementa.Ca(s) O2(g)b. CombustionAICI3(aq)Nap CO 3 (aq)+Double ReplacementС.3. List all of the metals that predictably form the following charges when they form an ion:+1+2+34. List all of the nonmetals that predictably form the following charges when they form an ion:-1-2-3EXPERIMENT 12 173

The given reaction is a single displacement reaction

Answered: 1. What type of reactions are the…

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter4: Stoichiometry

Section: Chapter Questions

Problem 4.87PAE

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Vitamin C, ascorbic acid (C6HgO6)(molar mass 176.1 g/mol), is a reducing agent. One way to determine the ascorbic acid content of a sample is to mix the acid with an excess of iodine, C6HgO6(aq) + I2(aq) + H2O(l) C6HgO6(aq) + 2 H3O+(aq) + 2 I(aq) and then titrate the iodine that did not react with the ascorbic acid with sodium thiosulfate. The balanced, net ionic equation for the reaction occurring in this titration is I2(aq) + 2 S2O32(aq)2 I(aq) + S4O62(aq) Suppose 50.00 mL of 0.0520 M I2 was added to the sample containing ascorbic acid. After the ascorbic acid/I2, reaction was complete, the I2 not used in this reaction required 20.30 mL of 0.196 M Na2S2O3 for titration to the equivalence point. Calculate the mass of ascorbic acid in the unknown sample.
One of the ways to remove nitrogen monoxide gas, a serious source of air pollution, from smokestack emissions is by reaction with ammonia gas, NH3. The products of the reaction, N2 and H2O, are not toxic. Write the balanced equation for this reaction. Assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
4.79 Phosphoric add (H3PO4) is important in the production of both fertilizers and detergents. It is distributed commercially as a solution with a concentration of about 14.8 M. Approximately 2.1 X l09 gallons of this concentrated phosphoric acid solution is produced annually in the United States. Assuming that all of this H3PO4 is produced by the reaction below, what mass of the mineral fluoruapatite (Ca5(PO4)3F) would be required each year? Ca5( PO4)3F+5H2SO43H3PO4+5CaSO4+HF
Balance the following equations: (a) for the reaction to produce "superphosphate" fertilizer Ca3(PO4)2(s) + H2SO4(aq) Ca(H2PO4)2(aq) + CaSO4(s) (b) for the reaction to produce diborane, B2H6 NaBH4(s) + H2SO4(aq) B2H6(g) + H2(g) + Na2SO4(aq) (c) for the reaction to produce tungsten metal from tungsten(VI) oxide WO3(s) + H2(g) W(s) + H2O() (d) for the decomposition of ammonium dichromate (NH4)2Cr2O7(s) N2(g) + H2O() + Cr2O3(s)
3.14 A number of compounds are used in cement, and reactions among them occur when water is added. In one, CaO reacts with Al2O3 and water to form Ca3Al2(OH)12. Write a bal- anced chemical equation for this process.
Aqueous hydrogen fluoride (hydrofluoric acid) is used to etch glass and to analyze minerals for their silicon content. Hydrogen fluoride will also react with sand (silicon dioxide). (a) Write an equation for the reaction of solid silicon dioxide with hydrofluoric acid to yield gaseous silicon tetrafluoride and liquid water. (b) The mineral fluorite (calcium fluoride) occurs extensively in Illinois. Solid calcium fluoride can also be prepared by the reaction of aqueous solutions of calcium chloride and sodium fluoride, yielding aqueous sodium chloride as the other product. Write complete and net ionic equations for this reaction.
Gold metal will dissolve only in aqua regia, a mixture of concentrated hydrochloric acid and concentrated nitric acid in a 3:1 volume ratio. The products of the reaction between gold and the concentrated acids are AuCl4-(aq), NO(g), and H2O. The equation for this reaction where HNO3 and HCl are strong acids is Au(s)+4Cl(aq)+4H+(aq)+NO3(aq)AuCl4(aq)+NO(g)+2H2O(a) What stoichiometric ratio of hydrochloric acid to nitric acid should be used? (b) What volumes of 12 M HCl and 16 M are HNO3 required to furnish the Cl- and NO3- ions to react with 25.0 g of gold?
3.16 Balance the following equations. (a) reaction to produce "super-phosphate" fertilizer: Ca3(PO4)2(s)+H2SO4(aq)( Ca(H2PO4)2(aq)+CaSO4(s) (b) reaction to produce diborane, B2H6: NaBH4(s) + H2SO4(aq) ( B2H6(g) + H2(g) + Na2SO4(aq) (c) reaction to produce tungsten metal from tungsten(VI) oxide: WO3(s)+ H2(g) ( W(s) + H2O(l) (d) decomposition of ammonium dichromate: (NH4)2Cr2O7(s)(N2(g)+H2O(l)+Cr2O3(s)
4.112 A metallurgical firm wishes to dispose of 1300 gallons of waste sulfuric acid whose molarity is 1.37 M. Before disposal, it will be reacted with calcium hydroxide (slaked lime), which costs $0.23 per pound. (a) Write the balanced chemical equation for this process. (b) Determine the cost that the firm will incur from this use of slaked lime.
When organic compounds containing sulfur are burned, sulfur dioxide is produced. The amount of SO2formed can be determined by the reaction with hydrogen peroxide: H2O2(aq)+SO2(g)H2SO4(aq) The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1 .302-g sample of coal is burned, and the SO2is collected in a solution of hydrogen peroxide. It took 28.44 mL of a 0.1000 M NaOH solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.
Ten mL of concentrated H3PO4 (91.7% by mass, d=1.69g/mL) was accidentally poured into a beaker containing 20.0 g of NaOH. Not all the NaOH was consumed. How many grams of NaOH were left unreacted? The equation for the reaction is H3PO4(aq)+3OH(aq)3H2O+PO43(aq)
The formation of water-Insoluble silver chloride is useful in the analysis of chloride-containing substances. Consider the following unbalanced equation: BaCl2(aq) + AgNO3(aq) AgCI(s) + Ba(NO3)2(aq) (a) Write the balanced equation. (b) What mass of AgNO3, in grams, is required for complete reaction with 0.156 g of BaCI2? What mass of AgCI is produced?

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