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chemistry and chemical reactivity

Questions and Answers of Chemistry And Chemical Reactivity

The element below aluminum in Group 3A is gallium, and there are numerous similarities in the chemistry of these two elements. For example, the hydroxides of both elements are amphoteric. A
The boron trihalides (except BF3) hydrolyze completely to boric acid and the acid HX.(a) Write a balanced equation for the reaction of BCl3 with water.(b) Calculate ΔrH° for the hydrolysis of BCl3
Draw a possible structure for the cyclic anion in the salt K3B3O6 and the anion in Ca2B2O5.
When boron hydrides burn in air, the reactions are very exothermic.(a) Write a balanced equation for the combustion of B5H9(g) in air to give B2O3(s) and H2O(g).(b) Calculate the enthalpy of
Diborane can be prepared by the reaction of NaBH4 and I2. Which substance is oxidized, and which is reduced?
(a) Write a balanced equation for the reaction of Al and H2O(ℓ) to produce H2 and Al2O3.(a) Using thermodynamic data in Appendix L, calculate ΔrH°, ΔrS°, and ΔrG° for this reaction. Do these
Write balanced equations for the reactions of aluminum with HCl(aq), Cl2, and O2.
Aluminum dissolves readily in hot aqueous NaOH to give the aluminate ion, [Al(OH)4]−, and H2. Write a balanced equation for this reaction. If you begin with 13.2 g of Al, what volume (in liters) of
Alumina, Al2O3, is amphoteric. Among examples of its amphoteric character are the reactions that occur when Al2O3 is heated strongly or “fused” with acidic oxides and basic oxides.(a) Write a
Aluminum sulfate is the most commercially important aluminum compound, after aluminum oxide and aluminum hydroxide. It is produced from the reaction of aluminum oxide and sulfuric acid. What masses
“Aerated” concrete bricks are widely used building materials. They are obtained by mixing gas forming additives with a moist mixture of lime, cement, and possibly sand. Industrially, the
Elemental silicon is oxidized by O2 to give unknown A. Compound A is dissolved in molten Na2CO3 giving B. When B was treated with aqueous hydrochloric acid, C is produced. Identify compound C.(a)
Describe the structure of pyroxenes (see page 986). What is the ratio of silicon to oxygen in this type of silicate?Data given in page 986 Six-member rings of Si atoms with O atoms in edges are a
Silicon and oxygen form a six-membered ring in the silicate anion [Si3O9]6−. What is the oxidation state of silicon in this anion? (The rare blue mineral benitoite, the California state gemstone,
Describe how ultrapure silicon can be produced from sand.
Silicate structures: Draw a structure, and give the charge for a cyclic silicate anion with the formula [Si6O18]n−.
Silicates often have chain, ribbon, cyclic, or sheet structures. One of the simpler ribbon structures is [Si2O52−]n. Draw a structure for this anionic material.
Construct Lewis structures for the several resonance forms of N2O. What is the predicted N—N bond order?(a) 1(b) 2(c) between 2 and 3(d) 3
Consult the data in Appendix L. Are any of the nitrogen oxides listed there stable with respect to decomposition to N2 and O2?Data given in Appendix L TABLE 20 Species Aluminum Al(s) AICI
Which statement about ammonia is not correct?(a) Ammonia can be made by a direct reaction of the elements.(b) Aqueous solutions of ammonia are acidic.(c) Ammonia is a gas at room temperature and
In the “contact process” for making sulfuric acid, sulfur is first burned to SO2. Environmental restrictions allow no more than 0.30% of this SO2 to be vented to the atmosphere.(a) If enough
Before hydrazine came into use to remove dissolved oxygen in the water in steam boilers, Na2SO3 was commonly used for this purpose:2 Na2SO3(aq) + O2(aq) → 2 Na2SO4(aq)What mass of Na2SO3 is
Review the structure of phosphorous acid in Table 21.6.Data given in Table 21.6(a) What is the oxidation number of the phosphorus atom in this acid?(b) Draw the structure of diphosphorous acid,
Unlike carbon, which can form extended chains of atoms, nitrogen can form chains of very limited length. Draw the Lewis electron dot structure of the azide ion, N3−. Is the ion linear or bent?
Which of the following is not a common oxidation number for sulfur in its compounds?(a) −2(b) +6(c) +3(d) +4
Which statement about oxygen is not true?(a) Liquid oxygen is attracted to a magnet.(b) The allotropes of oxygen are O2 and O3.(c) Oxygen is the most abundant element in the Earth’s crust.(d) All
A sulfuric acid plant produces an enormous amount of heat. To keep costs as low as possible, much of this heat is used to make steam to generate electricity. Some of the electricity is used to run
Sulfur forms anionic chains of S atoms called polysulfides. Draw a Lewis electron dot structure for the S22− ion. The S22− ion is the disulfide ion, an analogue of the peroxide ion. It occurs in
Sulfur forms a range of compounds with fluorine. Draw Lewis electron dot structures for S2F2 (connectivity is FSSF), SF2, SF4, SF6, and S2F10. What is the oxidation number of sulfur in each of these
Which halogen has the highest bond dissociation enthalpy?(a) F2 (b) Cl2 (c) Br2 (d) I2
Which of the following statements is not correct?(a) The ease of oxidation of the halide ions is F− < Cl− < Br− < I−.(b) Fluorine is the most abundant halogen in the Earth’s crust.(c) F2 is
The halogen oxides and oxoanions are good oxidizing agents. For example, the reduction of bromate ion has an E° value of 1.44 V in acid solution:Is it possible to oxidize aqueous 1.0 M Mn2+ to
Use data in Appendix L to calculate the enthalpy and free energy change for the reaction 2 NO2(g) → N2O4(g)Is this reaction exothermic or endothermic? Is the reaction product- or reactant-favored
A major use of hydrazine, N2H4, is in steam boilers in power plants.(a) The reaction of hydrazine with O2 dissolved in water gives N2 and water. Write a balanced equation for this reaction.(b) O2
Use data in Appendix L to calculate the enthalpy and free energy change for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Is this reaction exothermic or endothermic? Is the reaction product- or
The overall reaction involved in the industrial synthesis of nitric acid is NH3(g) + 2 O2(g) → HNO3(aq) + H2O(ℓ)Calculate ΔrG° for this reaction and its equilibrium constant at 25°C.
Element 109, now named meitnerium (in honor of the Austrian–Swedish physicist, Lise Meitner [1878–1968]), was produced in August 1982 by a team at Germany’s Institute for Heavy Ion Research.
The reactionoccurs at high temperatures. At 700°C, a 200.0-L tank contains 1.0 mol of CO, 0.20 mol of CO2, and 0.40 mol of C at equilibrium.(a) Calculate Kc for the reaction at 700°C.(b) Calculate
A neutral atom has two electrons with n = 1, eight electrons with n = 2, eight electrons with n = 3, and two electrons with n = 4. Assuming this element is in its ground state, supply the following
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide.(a) Laboratory measurements at 986°C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol
A mixture of CO and Cl2 is placed in a reaction flask: [CO] =0.0102 mol/L and [Cl2] = 0.00609 mol/L. When the reactionhas come to equilibrium at 600 K, [Cl2] =0.00301 mol/L.(a) Calculate the
An aqueous solution has a pH of 3.75. What is the hydronium ion concentration of the solution? Is it acidic or basic?
You place 0.0300 mol of pure SO3 in an 8.00-L flask at 1150 K. At equilibrium, 0.0058 mol of O2 has been formed. Calculate Kc for the reaction at 1150 K. (8)²0 + (8) 07 (8) EOS 7
What is the pH of a 0.0075 M solution of HCl? What is the hydroxide ion concentration of the solution?
The value of Kc for the interconversion of butane and isobutane is 2.5 at 25°C.If you place 0.017 mol of butane in a 0.50-L flask at 25°C and allow equilibrium to be established, what will be the
What is the pH of a 1.2 × 10−4 M solution of KOH? What is the hydronium ion concentration of the solution?
Cyclohexane, C6H12, a hydrocarbon, can isomerize or change into methylcyclopentane, a compound of the same formula (C5H9CH3) but with a different molecular structure.The equilibrium constant has been
What is the pH of a 0.0015 M solution of Ba(OH)2?
The equilibrium constant for the dissociation of iodine molecules to iodine atomsis 3.76 × 10−3 at 1000 K. Suppose 0.105 mol of I2 is placed in a 12.3-L flask at 1000 K. What are the
The pH of a solution of Ba(OH)2 is 10.66 at 25°C. What is the hydroxide ion concentration in the solution? If the solution volume is 125 mL, what mass of Ba(OH)2 must have been dissolved?
The equilibrium constant, Kc, for the reactionat 25°C is 5.9 × 10−3. Suppose 15.6 g of N2O4 is placed in a 5.000-L flask at 25°C. Calculate the following:(a) The amount of NO2 (mol) present at
Write an equilibrium constant expression for the reaction of ammonium ion, a weak acid, with water.
Several acids are listed here with their respective equilibrium constants:(a) Which is the strongest acid? Which is the weakest acid?(b) Which acid has the weakest conjugate base?(c) Which acid has
Carbonyl bromide decomposes to carbon monoxide and bromine.Kc is 0.190 at 73°C. If you place 0.0500 mol of COBr2 in a 2.00-L flask and heat it to 73°C, what are the equilibrium concentrations of
Iodine dissolves in water, but its solubility in a nonpolar solvent such as CCl4 is greater.The equilibrium constant is 85.0 for the process Nonpolar I₂ Polar H₂0 Nonpolar CCL4 Shake the test
Write an equilibrium constant expression for the reaction of fluoride ion, a weak base, with water.
Several acids are listed here with their respective equilibrium constants.(a) Which is the strongest acid? Which is the weakest acid?(b) What is the conjugate base of the acid HF?(c) Which acid has
Which of the following correctly relates the equilibrium constants for the two reactions shown?(a) K2 = 1/(K1)1⁄2(b) K2 = 1/K1(c) K2 = K12(d) K2 = −K11⁄2 A + B 2 C + ¹/2 B CA K₁ K₂
You place 0.0340 g of I2 in 100.0 mL of water. After shaking it with 10.0 mL of CCl4, how much I2 remains in the water layer?(a) K2 = 2K1(b) K2 = K12(c) K2 = 1/K1(d) K2 = 1/K12 A + B 2 C 2A + 2 B4
Which of the following ions or compounds has the strongest conjugate base? Briefly explain your choice.(a) HSO4−(b) CH3CO2H (c) HOCl
Consider the following equilibria involving SO2(g) and their corresponding equilibrium constants.Which of the following expressions relates K1 to K2?(a) K2 = K12(b) K22 = K1(c) K2 = K1(d) K2 =
The equilibrium constant K for the reactionis 6.66 × 10−12 at 1000 K. Calculate K for the reaction CO₂(g) → CO(g) + ½ 0₂(g)
Which of the following compounds or ions has the weakest conjugate base? Briefly explain your choice.(a) HCN(b) HClO(c) NH4+
Calculate K for the reactiongiven the following information: (8)7057 +(s)us (8)00 7 + (s)²ous
Which of the following compounds or ions has the weakest conjugate acid? Briefly explain your choice.(a) HCO3−(b) F−(c) NO2−
Calculate K for the reactiongiven the following information: Fe(s) + H₂O(g) → FeO(s) + H₂(g)
Which of the following compounds or ions has the strongest conjugate acid? Briefly explain your choice.(a) CN−(b) NH3(c) SO42−
Relationship of Kc and Kp:(a) Kp for the following reaction is 0.16 at 25°C. What is the value of Kc?(b) The equilibrium constant, Kc, for the following reaction is 1.05 at 350 K. What is the value
Dissolving K2CO3 in water gives a basic solution. Write a balanced equation showing how this can occur.
Dissolving ammonium bromide in water gives an acidic solution. Write a balanced equation showing how this can occur.
Epinephrine hydrochloride has a pKa value of 9.53. What is the value of Ka? Where does the acid fit in Table 16.2?Data given in Table 16.2 Increasing Acid Strength TABLE 16.2 Acid Name Perchloric
Relationship of Kc and Kp:(a) The equilibrium constant, Kc, for the following reaction at 25°C is 170. What is the value of Kp?(b) Kc for the decomposition of ammonium hydrogen sulfide is 1.8 ×
If each of the salts listed here were dissolved in water to give a 0.10 M solution, which solution would have the highest pH? Which would have the lowest pH?(a) Na2S(b) Na3PO4(c) NaH2PO4(d) NaF(e)
An organic acid has pKa = 8.95. What is its Ka value? Where does the acid fit in Table 16.2?Data given in Table 16.2 Increasing Acid Strength TABLE 16.2 Acid Name Perchloric acid Sulfuric
Which of the following common food additives would give a basic solution when dissolved in water?(a) NaNO3 (used as a meat preservative)(b) NaC6H5CO2 (sodium benzoate; used as a soft drink
Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (ΔrH° = 40.5 kJ/mol-rxn).Predict the effect of the following changes on the position of the equilibrium; that is, state which
A weak acid has a Ka of 6.5 × 10−5. What is the value of pKa for the acid?
Consider the isomerization of butane with an equilibrium constant of K = 2.5. (See Study Question 13.) The system is originally at equilibrium with [butane] = 1.0 M and [isobutane] = 2.5 M.(a) If
The decomposition of NH4HSis an endothermic process. Using Le Chatelier’s principle, explain how increasing the temperature would affect the equilibrium. If more NH4HS is added to a flask in which
Suppose 0.086 mol of Br2 is placed in a 1.26-L flask and heated to 1756 K, a temperature at which the halogen dissociates to atoms.If Br2 is 3.7% dissociated at this temperature, calculate Kc.
The equilibrium constant for the reactionis 1.7 × 10−3 at 2300 K.(a) What is K for the reaction when written as follows?(b) What is K for the following reaction? N₂(g) + 0₂(g) →2 NO(g)
Which is the stronger of the following two acids?(a) Benzoic acid, C6H5CO2H, pKa = 4.20(b) 2-chlorobenzoic acid, ClC6H4CO2H, pKa = 2.90
At 1800 K, oxygen dissociates very slightly into its atoms.If you place 0.050 mol of O2 in a 10.-L vessel and heat it to 1800 K, how many O atoms are present in the flask? O₂(g) 2 0(g) ⇒ Kp = 1.2
Calculate the pH of a 0.0010 M aqueous solution of HF.
Kp for the formation of phosgene, COCl2, is 6.5 × 1011 at 25°C.What is the value of Kp for the dissociation of phosgene? (8) DOD → (8)ID + (8)OD
Which is the stronger of the following two acids?(a) Acetic acid, CH3CO2H, Ka = 1.8 × 10−5(b) Chloroacetic acid, ClCH2CO2H, pKa = 2.85
The equilibrium constant, Kc, for the following reaction is 1.05 at 350 K.If an equilibrium mixture of the three gases at 350 K contains 0.0206 M CH2Cl2(g) and 0.0163 M CH4, what is the equilibrium
Chloroacetic acid (ClCH2CO2H) has Ka = 1.41 ×10−3. What is the value of Kb for the chloroacetateion (ClCH2CO2−)?
Carbon tetrachloride can be produced by the following reaction:Suppose 0.12 mol of CS2 and 0.36 mol of Cl2 are placed in a 10.0-L flask. After equilibrium has been achieved, the mixture contains
A weak base has Kb = 1.5 × 10−9. What is the value of Ka for the conjugate acid?
Acetic acid and sodium hydrogen carbonate, NaHCO3, are mixed in water. Write a balanced equation for the acid–base reaction that could, in principle, occur. Using Table 16.2, decide whether the
Equal numbers of moles of H2 gas and I2 vapor are mixed in a flask and heated to 700°C. The initial concentration of each gas is 0.0088 mol/L, and 78.6% of the I2 is consumed when equilibrium is
The trimethylammonium ion, (CH3)3NH+, is the conjugate acid of the weak base trimethylamine, (CH3)3N. A chemical handbook gives 9.80 as the pKa value for (CH3)3NH+. What is the value of Kb for
The chromium(III) ion in water, [Cr(H2O)6]3+, is a weak acid with pKa = 3.95. What is the value of Kb for its conjugate base, [Cr(H2O)5OH]2+?
The equilibrium constant for the butane ⇄ isobutane isomerization reaction is 2.5 at 25°C. If 1.75 mol of butane and 1.25 mol of isobutane are mixed, is the system at equilibrium? If not, when it
Ammonium chloride and sodium dihydrogen phosphate, NaH2PO4, are mixed in water. Write a balanced equation for the acid–base reaction that could, in principle, occur. Using Table 16.2, decide
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 × 10−3.(a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain
Which of the following correctly relates the two equilibrium constants for the two reactions shown?(a) K2 = −K12(b) K2 = 1/(K1)1⁄2(c) K2 = 1/K12(d) K2 = 2K1 NOCI(g) →NO(g) 2 NO(g) + Cl₂(g)
For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) NH4+(aq) + Br−(aq): (b) HPO4²-(aq) +
Consider the following equilibrium:(a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each

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