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general chemistry principles

Questions and Answers of General Chemistry Principles

Arrange the following compounds in the expected order of increasing solubility in water, and give the basis for your arrangement: Li2CO3, Na2CO3, MgCO3.
With a minimum of calculation, determine how much less heat is produced per mol of C8H18(l) burned in reaction (21.30) than in reaction (21.29).Reaction (21.30)Reaction (21.29) C8H18(1) + 12 O₂(g)
Suggest a reason why the hydrated beryllium ion is [Be(H2O)4]2+, whereas the hydrated magnesium ion is [Mg(H2O)6]2+.
A lithium battery used in a cardiac pacemaker has a voltage of 3.0 V and a capacity of 0.50 A h (ampere hour). Assume that 5.0 μW of power is needed to regulate the heartbeat. Appendix B. Current
The first electrolytic process to produce sodium metal used molten NaOH as the electrolyte. Write probable half-equations and an overall equation for this electrolysis.
Lithium and magnesium combine with N2 to give the nitrides Li3N and Mg3N2, respectively. Suggest a reason for this and write balanced chemical equations for the reactions.
A 1.26 L sample of KCl(aq) is electrolyzed for 3.50 min with a current of 0.910 A.(a) Calculate the pH of the solution after electrolysis.(b) Why doesn’t the result depend on the initial
Boron forms a compound with the formula B2H2(CH3)4. Suggest a probable structure.
AlF3 is almost insoluble in anhydrous HF, but it dissolves if KF is present. Passage of BF3 through the resulting solution causes AlF3 to precipitate. How can you explain these observations?
An analysis of a Solvay-process plant shows that for every 1.00 kg of NaCl consumed, 1.03 kg of NaHCO3 are obtained. The quantity of NH3 consumed in the overall process is 1.5 kg.(a) What is the
Consider the reaction Ca(OH)2(s) + Na2SO4(aq) ⇌ CaSO4(s) + 2 NaOH(aq).(a) Write a net ionic equation for this reaction.(b) Will the reaction essentially go to completion?(c) What will be [SO42-]
The standard Gibbs energies of formation, ΔfG°, for KO2(s) and K2O(s) are -240.59 kJ mol‾1 and -322.09 kJ mol‾1, respectively, at 298 K. Calculate the equilibrium constant for the reaction
The standard Gibbs energies of formation, ΔfG°, for Na2O(s) and Na2O2(s) are -379.09 kJ mol‾1 and -449.63 kJ mol‾1, respectively, at 298 K. Calculate the equilibrium constant for the reaction
The empirical formula of the mineral beryl is Be3Al2Si6O18. By using the several descriptions of silicate minerals just given as a guide, describe the structure of the silicate anion in beryl.
Without performing detailed calculations, indicate whether equilibrium is displaced either far to the left or far to the right for each of the following reactions. Use data from Appendix D as
In the manner used to construct Figure 21-5, complete the diagram outlined. Specifically, indicate the reactants (and conditions) you would use to produce the indicated substances from Ca(OH)2.Figure
Replace the calcium-containing substances shown in the diagram accompanying Exercise 13 by their magnesium-containing equivalents. Then describe the reactants (and conditions) you would use to
To prevent the air oxidation of aqueous solutions of Sn2+ to Sn4+, metallic tin is sometimes kept in contact with the Sn2+(aq). Suggest how this contact helps prevent the oxidation.
In the Dow process (Fig. 21-13), the starting material is Mg2+ in seawater and the final product is Mg metal. This process seems to violate the principle of conservation of charge. Does it?
Without performing detailed calculations, indicate why you would expect each of the following reactions to occur to a significant extent as written. Use data from Appendix D as necessary. (a)
Which has the (a) Higher melting point, MgO or BaO;(b) Greater solubility in water, MgF2 or MgCl2? Explain.
Write chemical equations to represent the following:(a) Reduction of BeF2 to Be metal with Mg as a reducing agent (b) Reaction of barium metal with Br2(l)(c) Reduction of uranium(IV) oxide to
Write chemical equations for the reactions you would expect to occur when (a) Mg(HCO3)2(s) is heated to a high temperature (b) BaCl2(l) is electrolyzed (c) Sr(s) is added to cold dilute HBr(aq)(d)
With respect to decomposition to MO(s) and SO3(g), which of the group 2 sulfates, MSO4(s), do you expect to be least stable? Explain your answer.
Assign oxidation states to all the atoms in a perborate ion based on the structure.Perborate ion: HO HO B 0-0- 0-01 B ОН ОН 2-
With respect to the decomposition to MO(s) and CO2(g), which of the group 2 carbonates, MCO3(s), do you expect to be most stable? Explain your answer.
The molecule tetraborane has the formula B4H10.(a) Show that this is an electron-deficient molecule.(b) How many bridge bonds must occur in the molecule?(c) Show that butane, C4H10, is not electron
Write Lewis structures for the following species, both of which involve coordinate covalent bonding:(a) Tetrafluoroborate ion, BF4‾, used in metal cleaning and in electroplating baths (b) Boron
Write chemical equations to represent the following:(a) The preparation of boron from BBr3(b) The formation of BF3 from B2O3(c) The combustion of boron in hot N2O(g).
Write chemical equations to represent the (a) Reaction of Al(s) with HCl(aq);(b) Reaction of Al(s) with NaOH(aq);(c) Oxidation of Al(s) to Al3+(aq) by an aqueous solution of sulfuric acid; the
Write plausible equations for the (a) Reaction of Al(s) with Br2(l);(b) Production of Cr from Cr2O3(s) by the thermite reaction, with Al as the reducing agent;(c) Separation of Fe2O3 impurity from
In some foam-type fire extinguishers, the reactants are Al2(SO4)3(aq) and NaHCO3(aq). When the extinguisher is activated, these reactants mix, producing Al(OH)3(s) and CO2(g). The Al(OH)3–CO2 foam
Some baking powders contain the solids NaHCO3 and NaAl(SO4)2. When water is added to this mixture of compounds, CO2(g) and Al(OH)3(s) are two of the products. Write plausible net ionic equations for
The maximum resistance to corrosion of aluminum is between pH 4.5 and 8.5. Explain how this observation is consistent with other facts about the behavior of aluminum presented in this text.
Describe a series of simple chemical reactions that you could use to determine whether a particular metal sample is “aluminum 2S” (99.2% Al) or “magnalium” (70% Al, 30% Mg). You are permitted
In the purification of bauxite ore, a preliminary step in the production of aluminum, [Al(OH)4]‾(aq) can be converted to Al(OH)3(s) by passing CO2(g) through the solution. Write an equation for the
In 1825, Hans Oersted produced aluminum chloride by passing chlorine over a heated mixture of carbon and aluminum oxide. In 1827, Friedrich Wöhler obtained aluminum by heating aluminum chloride with
A description for preparing potassium aluminum alum calls for dissolving aluminum foil in KOH(aq). The solution obtained is treated with H2SO4(aq), and the alum is crystallized from the resulting
Handbooks and lists of chemicals do not contain entries under the formulas Al(HCO3)3 and Al2(CO3)2. Explain why these compounds do not exist.
Compound FB(BF2)2 disproportionates at –30 °C to give BF3 and very unstable B8F12. The B8F12 molecule is unstable because it contains a strained four-membered ring of boron atoms. Write a balanced
Gallium trichloride (GaCl3) is a very active catalyst for a number of organic transformations. In the solid state, GaCl3 exists as a dimer with the formula Ga2Cl6. Draw a plausible structure for the
Comment on the accuracy of a jeweler’s advertising that “diamonds last forever.” In what sense is the statement true, and in what ways is it false?
A temporary fix for a “sticky” lock is to scrape a pencil point across the notches on the key and to work the key in and out of the lock a few times. What is the basis of this fix?
Write a chemical equation to represent (a) The reduction of silica to elemental silicon by aluminum;(b) The preparation of potassium metasilicate by the high-temperature fusion of silica and
Write a chemical equation to represent (a) The reaction of potassium cyanide solution with silver nitrate solution;(b) The combustion of Si3H8 in an excess of oxygen;(c) The reaction of dinitrogen
Describe what is meant by the terms silane and silanol. What is their role in the preparation of silicones?
Describe and explain the similarities and differences between the reaction of a silicate with an acid and that of a carbonate with an acid.
Methane and sulfur vapor react to form carbon disulfide and hydrogen sulfide. Carbon disulfide reacts with Cl2(g) to form carbon tetrachloride and S2Cl2. Further reaction of carbon disulfide and
Show that the empirical formula given for muscovite mica is consistent with the expected oxidation states of the elements present.
Show that the empirical formula given for crysotile asbestos is consistent with the expected oxidation states of the elements present.
Write plausible chemical equations for the (a) Dissolving of lead(II) oxide in nitric acid; (b) Heating of SnCO3(s);(c) Reduction of lead(II) oxide by carbon;(d) Reduction of Fe3+(aq) to Fe2+(aq)
Write plausible chemical equations for preparing each compound from the indicated starting material:(a) SnCl2 from SnO; (b) SnCl4 from Sn; (c) PbCrO4 from PbO2.What reagents (acids, bases, salts)
Lead(IV) oxide, PbO2, is a good oxidizing agent. Use appropriate data from Appendix D to determine whether PbO2(s) in a solution with [H3O+] = 1 M is a sufficiently good oxidizing agent to carry the
Aqueous tin(II) ion, Sn2+ (aq), is a good reducing agent. Use data from Appendix D to determine whether Sn2+ (aq) is a sufficiently good reducing agent to reduce (a) I2 (s) to I‾ (aq); (b) Fe3+(aq)
Would you expect the reaction of Sn(s) and Cl2(g) to yield SnCl2 or SnCl4?
Would you expect the reaction of Ge(s) and F2(g) to yield GeF2, with germanium in the +2 oxidation state, or GeF4, with germanium in the +4 oxidation state?
A chemical that should exist as a crystalline solid is seen to be a mixture of a solid and liquid in a container on a storeroom shelf. Give a plausible reason for that observation. Should the
The following series of observations is made: (1) A small piece of dry ice [CO2(s)] is added to 0.005 M Ca(OH)2(aq). (2) Initially, a white precipitate forms.(3) After a short time the precipitate
The melting point of NaCl(s) is 801 °C, much higher than that of NaOH (322 °C). More energy is consumed to melt and maintain molten NaCl than NaOH. Yet the preferred commercial process for the
Although the triiodide ion, I3‾, is known to exist in aqueous solutions, the ion is stable in only certain ionic solids. For example, CsI3 is stable with respect to decomposition to CsI and I2, but
At 298 K, the ΔfG° values for Li2O(s) and Li2O2(s) suggest that Li2O2(s) is thermodynamically more stable than Li2O(s). At 1000 K, however, the situation is reversed. The standard Gibbs energies of
The chemical equation for the hydration of an alkali metal ion is M+(g): M+(aq). The standard Gibbs energy changes and the enthalpy changes for the process are denoted by ΔhydrG° and ΔhydrH° and
When a 0.250 g sample of Ca is heated in air, 0.325 g of product is obtained. Assume that all the Ca appears in the product.(a) If the product were pure CaO, what mass should have been obtained?(b)
Comment on the feasibility of using a reaction similar to (21.4) to produce (a) Lithium metal from LiCl; (b) Cesium metal from CsCl, with Na(l) as the reducing agent in each case. Consider data
Concerning the thermite reaction, (a) Use data from Appendix D to calculate ΔrH° at 298 K for the reaction below.(b) Write an equation for the reaction when MnO2(s) is substituted for Fe2O3(s),
Use data from Appendix D (Table D-2) to calculate a value of E° for the reduction of Li+(aq) to Li(s), and compare your result with the value listed in Table 21.2.Table D-2Table 21.2 TABLE D.2
The electrolysis of 0.250 L of 0.220 M MgCl2 is conducted until 104 mL of gas (a mixture of H2 and water vapor) is collected at 23 °C and 748 mmHg. Will Mg(OH)2(s) precipitate if electrolysis is
A particular water sample contains 56.9 ppm SO42– and 176 ppm HCO3– with Ca2+ as the only cation.(a) How many parts per million of Ca2+ does the water contain?(b) How many grams of CaO are
Write an appropriate formula for each of the following:(a) Hydroxylamine; (b) Calcium hydrogen phosphate;(c) Lithium nitride.
Use Figure 22-17 to establish E° for the reduction of N2O4 to NO in an acidic solution.Figure 22-17 Acidic solution ([H+] = 1 M): +5 +3 -2 +4 +2 +1 0 - 1 0.803 V 1.065 V 0.996 V 1.591 V 1.766 V
Use Figure 22-17 to establish E° for the reduction of NO3– to NO2– in a basic solution.Figure 22-17 Acidic solution ([H+] = 1 M): +5 +3 +4 +2 +1 0 - 1 1.42 V 0.803 V 1.065 V 0.996 V 1.591 V
All the group 15 elements form trifluorides, but nitrogen is the only group 15 element that does not form a pentafluoride.(a) Suggest a reason why nitrogen does not form a pentafluoride.(b) The
For use in analytical chemistry, sodium thiosulfate solutions must be carefully prepared. In particular, the solutions must be kept from becoming acidic. In strongly acidic solutions, thiosulfate ion
What is the value of K for the dissociation of HI(g) into its elements at 298 K?
Do you expect the ions ICl2+ and ICl2– to have the same shape? Explain.
(A) What is the value of K for the dissociation of HF(g) into its elements at 298 K? Use data from Table 22.6.(B) Use data from Table 22.6 to determine K and the percent dissociation of HCl(g) into
Fluorine is able to stabilize elements in very high oxidation states. For each of the elements Na, Mg, Al, Si, P, S, and Cl, give the formula of the highest oxidationstate of fluoride that is known
(A) Use information from Figure 22-17 to decide whether the nitrite anion, NO2–, disproportionates spontaneously in basic solution to NO3– and NO. Assume standard-state conditions.(B) Does HNO2
Which of the following dilute aqueous solutions can be used to obtain oxygen and hydrogen gases simultaneously through electrolysis using platinum electrodes: H2SO4(aq), CuSO4(aq), NaOH(aq),
The oxides of the phosphorus(III), antimony(III), and bismuth(III) are P4O6, Sb4O6, and Bi2O3. Only one of these oxides is amphoteric. Which one? Which of these oxides is most acidic? Which is most
Would you expect the shape of the ozonide ion to be the same as that of ozone? Explain.
The oxides of the selenium(IV) and tellurium(IV) are SeO2 and TeO2. One of these oxides is amphoteric and one is acidic. Which is which?
Electrostatic potential maps for OF2 and OCl2 are shown in the margin. Explain the differences.
A 55 L cylinder contains Ar at 145 atm and 26 °C. What minimum volume of air at STP must have been liquefied and distilled to produce this Ar? Air contains 0.934% Ar, by volume.
In the solid phase, PCl5 forms PCl4+ and PCl6+ However, PBr5 forms PBr4+Br– Suggest a reason for this difference in structure.
Write condensed structural formulas for phosphoric acid and phosphorous acid. Condensed structural formulas are discussed on page 70. Structural formula: HO || H-C-C-0-H H
Some sources of natural gas contain 8% He by volume. How many liters of such a natural gas must be processed at STP to produce 5.00 g of He?
Use VSEPR theory to predict the probable geometric structures of (a) XeO3;(b) XeO4;(c) XeF5+.
Use VSEPR theory to predict the probable geometric structures of the molecules (a) O2XeF2;(b) O3XeF2;(c) OXeF4.
Write a chemical equation for the hydrolysis of XeF4 that yields XeO3, Xe, O2, and HF as products.
Write a chemical equation for the hydrolysis in alkaline solution of XeF6 that yields XeO64–, Xe, O2, F‾, and H2O as products.
Provide an explanation for the observation that helium, neon, and argon do not react directly with fluorine.
Provide an explanation for the inability of O2 to react directly with xenon.
Freshly prepared solutions containing iodide ion are colorless, but over time they usually turn yellow. Describe a plausible chemical reaction (or reactions) to account for this observation.
The following properties of astatine have been measured or estimated: (a) Covalent radius; (b) Ionic radius (At–);(c) First ionization energy; (d) Electron affinity; (e) Electronegativity; (f)
Fluorine can be prepared by the reaction of hexafluoro-manganate(IV) ion, MnF62–, with antimony pentafluoride to produce manganese(IV) fluoride and SbF6–, followed by the disproportionation of
Make a general prediction about which of the halogen elements, F2, Cl2, Br2, or I2, displaces other halogens from a solution of halide ions. Which of the halogens is able to displace O2(g) from
The abundance of F‾ in seawater is 1 g F‾ per ton of seawater. Suppose that a commercially feasible method could be found to extract fluorine from seawater.(a) What mass of F2 could be obtained
Fluorine is produced chiefly from fluorite, CaF2. Fluorine can also be obtained as a by-product of the production of phosphate fertilizers, derived from phosphate rock [3 Ca3(PO4)2 · CaF2]. What is
Show by calculation whether the disproportionation of chlorine gas to chlorate and chloride ions will occur under standard-state conditions in an acidic solution.

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