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general chemistry principles
General Chemistry Principles And Modern Applications 11th Edition Ralph Petrucci, Jeffry Madura, F. Herring, Carey Bissonnette - Solutions
Given that ΔfH°[BaSO4(s)] = -1473 kJ/mol, what is the standard enthalpy change for the precipitation of barium sulfate?
Consider the following situations: a stick of dynamite exploding deep within a mountain cavern, the titration of an acid with base in a laboratory, and a cylinder of a steam engine with all of its valves closed. To what type of thermodynamic systems do these situations correspond?
With a minimum of calculation, estimate the final temperature reached when 100.0 mL of water at 10.00 °C is added to 200.0 mL of water at 70.00 °C. What basic principle did you use and what assumptions did you make in arriving at this estimate?
Two objects of the same mass absorb the same amount of heat when placed in a flame, but the temperature of one object increases more than the temperature of the other. Which object has the greater specific heat capacity?
How do we determine the heat capacity of the solution calorimeter (coffee-cup calorimeter)?
When water is injected into a balloon filled with ammonia gas, the balloon shrinks and feels warm. What are the sources of heat and work, and what are the signs of q and w in this process?
A gas in a 1.0 L closed cylinder has an initial pressure of 10.0 bar. It has a final pressure of 5.0 bar. The volume of the cylinder remained constant during this time. What form of energy was transferred across the boundary to cause this change? In which direction did the energy flow?
A sample can be heated very slowly or very rapidly. The darker shading in the illustration indicates a higher temperature. Which of the two sets of diagrams do you think corresponds to reversible heating and which to spontaneous, or irreversible, heating?
Suppose a system is subjected to the following changes: a 40 kJ quantity of heat is added and the system does 15 kJ of work; then the system is returned to its original state by cooling and compression. What is the value of ΔH?
The heat of reaction between carbon (graphite) and the corresponding stoichiometric amounts of hydrogen gas to form C2H2(g), C2H4(g), and C2H6(g) are 226.7, 52.3 and -84.7 kJ mol-1, respectively. Relate these values to the enthalpy diagram shown in the margin. Indicate on the diagram the standard
Is it possible to calculate a heat of reaction at 373.15 K by using standard enthalpies of formation at 298.15 K? If so, explain how you would do this, and indicate any additional data you might need.
(A) Write acceptable names for CsI, CaF2 ,FeO, CrCl3.(B) Write acceptable names for CaH2, CuCl, Ag2S, Hg2Cl2.
(A) Write formulas for the compounds (a) Boron trifluoride, (b) Potassium dichromate,(c) Sulfuric acid,(d) Calcium chloride.(B) Write formulas for the compounds (a) Aluminum nitrate, (b) Tetraphosphorus decoxide,(c) Chromium(III) hydroxide, (d) Iodic acid.
(A) Balance the equation for this reaction in acidic solution.Fe2+(aq) + MnO4-(aq) → Fe3+(aq) + Mn2+(aq)(B) Balance the equation for this reaction in acidic solution.UO2+(aq) + Cr2O72-(aq) → UO22+(aq) + Cr3+(aq)
(A) How much heat, in kilojoules (kJ), is required to raise the temperature of 237 g of water from 4.0 to 37.0 °C?(B) How much heat, in kilojoules (kJ), is required to raise the temperature of 2.50 kg Hg(l) from -20.0 to -6.0 °C? Assume a density of 13.6 g/mL and a molar heat capacity of 28.0 J
(A) Two solutions, 100.0 mL of 1.00 M AgNO31aq2 and 100.0 mL of 1.00 M NaCl1aq2, both initially at 22.4 °C, are added to a Styrofoam-cup calorimeter and allowed to react. The temperature rises to 30.2 °C. Determine qrxn per mole of AgCl1s2 in the reaction.(B) Two solutions, 100.0 mL of 1.020 M
(A) When 1.00 kg lead (specific heat capacity = 0.13 J g-1 °C-1) at 100.0 °C is added to a quantity of water at 28.5 °C, the final temperature of the lead–water mixture is 35.2 °C. What is the mass of water present?(B) A 100.0 g copper sample (specific heat capacity = 0.385 J g-1 °C-1) at
(A) Vanillin is a natural constituent of vanilla. It is also manufactured for use in artificial vanilla flavoring. The combustion of 1.013 g of vanillin, C8H8O3, in the same bomb calorimeter as in Example 7-3 causes the temperature to rise from 24.89 to 30.09 °C. What is the heat of combustion of
(A) How much work, in joules, is involved when 0.225 mol N2 at a constant temperature of 23 °C is allowed to expand by 1.50 L in volume against an external pressure of 0.750 atm?(B) How much work is done, in joules, when an external pressure of 2.50 atm is applied, at a constant temperature of
(A) What mass of sucrose must be burned to produce 1.00 x 103 kJ of heat?(B) A 25.0 mL sample of 0.1045 M HCl(aq) was neutralized by NaOH(aq). Use the result of Example 7-4 to determine the heat evolved in this neutralization.Example 7-4In the neutralization of a strong acid with a strong base, the
(A) The standard heat of combustion of propene, C3H6(g), is -2058 kJ/mol. Use this value and other data from this example to determine ΔrH° for the hydrogenation of propene to propane.(B) From the data in Practice Example 7-9A and the following equation, determine the standard enthalpy of
(A) What is the enthalpy change when a cube of ice 2.00 cm on edge is brought from -10.0 °C to a final temperature of 23.2 °C? For ice, use a density of 0.917 g/cm3, a specific heat capacity of 2.01 J g-1 °C-1, and an enthalpy of fusion of 6.01 kJ/mol.(B) What is the maximum mass of ice at -15.0
(A) The standard enthalpy of formation for the amino acid leucine, C6H13O2N(s), is -637.3 kJ/mol. Write the chemical equation to which this value applies.(B) How is ΔrH° for the following reaction related to the standard enthalpy of formation of NH3(g) listed in Table 7.2? What is the value of
(A) Use data from Table 7.2 to calculate the standard enthalpy of combustion of ethanol, C2H5OH(l), at 298.15 K.(B) Calculate the standard enthalpy of combustion at 298.15 K per mole of a gaseous fuel that contains C3H8 and C4H10 in the mole fractions 0.62 and 0.38, respectively.Table 7.2 TABLE 7.2
(A) The overall reaction that occurs in photosynthesis in plants isDetermine the standard enthalpy of formation of glucose, C6H12O6(s), at 298.15 K.(B) A handbook lists the standard enthalpy of combustion of gaseous dimethyl ether, (CH3)2O(g), at 298.15 K as -31.70 kJ/g. What is the standard molar
(A) Given that ΔfH°[AgI(s)] = -61.84 kJ/mol, what is the standard enthalpy change for the precipitation of silver iodide?(B) The standard enthalpy change for the precipitation of Ag2CO3(s) is -39.9 kJ per mole of Ag2CO3(s) formed. What is ΔfH°[Ag2CO3(s)]?
(A) The enthalpy of combustion for hexadec-1-ene, C16H32, is -10,539.0 kJ mol-1, and that of hexadecane, C16H34, is -10,699.1 kJ mol-1. What is the enthalpy of hydrogenation of hexadec-1-ene to hexadecane?(B) A chemist mixes 56 g CaO, powdered lime, with 0.10 L of water at 25 °C. After the
(A) A 0.382 g sample of magnesium is allowed to react with 2.652 g of nitrogen gas. The sole product is magnesium nitride. After the reaction, the mass of unreacted nitrogen is 2.505 g. What mass of magnesium nitride is produced?(B) A 7.12 g sample of magnesium is heated with 1.80 g of bromine. All
A stainless steel ball bearing has a radius of 6.35 mm and a density of 7.75 g/cm3. Iron is the principal element in steel. Carbon is a key minor element. The ball bearing contains 0.25% carbon, by mass. Assuming that the percent isotopic abundance of 13C is 1.108%, how many 13C atoms are present
Jan Baptista van Helmont (1579–1644) weighed a young willow tree and the soil in which the tree was planted. Five years later he found that the mass of soil had decreased by only 0.057 kg, while that of the tree had increased by 75 kg. During that period he had added only water to the bucket in
When an iron object rusts, its mass increases. When a match burns, its mass decreases. Do these observations violate the law of conservation of mass? Explain.
A 0.455 g sample of magnesium is allowed to burn in 2.315 g of oxygen gas. The sole product is magnesium oxide. After the reaction, no magnesium remains and the mass of unreacted oxygen is 2.015 g. What mass of magnesium oxide is produced?
(A) What masses of magnesium and oxygen must be combined to make exactly 2.000 g of magnesium oxide?(B) What substances are present, and what are their masses, after the reaction of 10.00 g of magnesium and 10.00 g of oxygen?
When 4.15 g magnesium and 82.6 g bromine react, (1) All the magnesium is used up, (2) Some bromine remains unreacted, and (3) Magnesium bromide is the only product. With this information alone, is it possible to deduce the mass of magnesium bromide produced? Explain.
When a strip of magnesium metal is burned in air (recall Figure 2-1), it produces a white powder that weighs more than the original metal. When a strip of magnesium is burned in a flashbulb, the bulb weighs the same before and after it is flashed. Explain the difference in these observations.Figure
In Example 2-1 we found that when 0.455 g of magnesium reacted with 2.315 g of oxygen, 0.755 g of magnesium oxide was obtained. Determine the mass of magnesium contained in a 0.500 g sample of magnesium oxide.Example 2-1A 0.455 g sample of magnesium is allowed to burn in 2.315 g of oxygen gas. The
(A) Use the notation AZE to represent the isotope of silver having a neutron number of 62.(B) Use the notation AZE to represent a tin ion having the same number of electrons as an atom of the isotope cadmium-112. Explain why there can be more than one answer.
In light of information presented to this point in the text, explain which of the three assumptions of Dalton’s atomic theory can still be considered correct and which cannot.Dalton’s Atomic TheoryFrom 1803 to 1808, John Dalton, an English schoolteacher, used the two fundamental laws of
A 0.406 g sample of magnesium reacts with oxygen, producing 0.674 g of magnesium oxide as the only product. What mass of oxygen was consumed in the reaction?
(A) What is the ratio of masses for 202Hg/12C, if the isotopic mass for 202Hg is 201.97062 u?(B) An isotope with atomic number 64 and mass number 158 is found to have a mass ratio relative to that of carbon-12 of 13.16034. What is the isotope, what is its atomic mass in u, and what is its mass
What is the single exception to the statement that all atoms comprise protons, neutrons, and electrons?
A 1.446 g sample of potassium reacts with 8.178 g of chlorine to produce potassium chloride as the only product. After the reaction, 6.867 g of chlorine remains unreacted. What mass of potassium chloride was formed?
With mass spectral data, the mass of an oxygen-16 atom is found to be 1.06632 times that of a nitrogen-15 atom. Given that 16O has a mass of 15.9949 u (see above), what is the mass of a nitrogen-15 atom, in u?
(A) The two naturally occurring isotopes of boron, boron-10 and boron-11, have masses of 10.0129370 u and 11.0093054 u, respectively. Which of these two occurs in greater abundance?(B) Indium has two naturally occurring isotopes and a weighted atomic mass of 114.818 u. One of the isotopes has a
The value listed for chromium in the table of atomic masses inside the front cover is 51.996 u. Should we conclude that naturally occurring chromium atoms are all of the type 5224Cr. The same table lists a value of 65.38 u for zinc. Should we conclude that zinc occurs as a mixture of isotopes?
When a solid mixture consisting of 10.500 g calcium hydroxide and 11.125 g ammonium chloride is strongly heated, gaseous products are evolved and 14.336 g of a solid residue remains. The gases are passed into 62.316 g water, and the mass of the resulting solution is 69.605 g. Within the limits of
(A) The masses and percent isotopic abundances of the three naturally occurring isotopes of silicon are 28Si, 27.9769265325 u, 92.223%; 29Si, 28.976494700 u, 4.685%; 30Si, 29.973377017 u, 3.092%. Calculate the weighted-average atomic mass of silicon.(B) Use data from Example 2-5 and the
The two naturally occurring isotopes of lithium, lithium-6 and lithium-7, have masses of 6.01512 u and 7.01600 u, respectively. Which of these two occurs in greater abundance?
Dividing the molar mass of gold by the Avogadro constant yields the mass of any individual atom of naturally occurring gold. In contrast, no naturally occurring atom of silver has the mass obtained by dividing the molar mass of silver by the Avogadro constant. How can this be?
Within the limits of experimental error, show that the law of conservation of mass was obeyed in the following experiment: 10.00 g calcium carbonate (found in limestone) was dissolved in 100.0 mL hydrochloric acid (d = 1.148 g/mL). The products were 120.40 g solution (a mixture of hydrochloric acid
Bromine has two naturally occurring isotopes, bromine-79 and bromine-81, with masses of 78.918338 u and 80.916291 u, respectively. Bromine has an atomic mass interval of [79.901, 79.907]. Estimate the percent isotopic abundances of 79Br by using (a) The lower bound and (b) The upper bound of the
(A) Write a symbol for the ion most likely formed by an atom of each of the following: Li, S, Ra, F, I, and Al.(B) Classify each of the following elements as a main-group or transition element. Also, specify whether they are metals, metalloids, or nonmetals: Na, Re, S, I, Kr, Mg, U, Si, B, Al, As,
In Example 2-1, we established that the mass ratio of magnesium to magnesium oxide is 0.455 g magnesium/ 0.755 g magnesium oxide.(a) What is the ratio of oxygen to magnesium oxide, by mass?(b) What is the mass ratio of oxygen to magnesium in magnesium oxide?(c) What is the percent by mass of
(A) What is the mass of 2.35 x 1024 atoms of Cu?(B) How many lead-206 atoms are present in a 22.6 g sample of lead metal? See Figure 2-16.Figure 2-16 (a) 6.02214 x 1023 F atoms = 18.9984 g (b) 6.02214 x 1023 Cl atoms = 35.45 g (c) 6.02214 x 1023 Mg atoms = 24.305 g (d) 6.02214 x 1023 Pb atoms =
Samples of pure carbon weighing 3.62, 5.91, and 7.07 g were burned in an excess of air. The masses of carbon dioxide obtained (the sole product in each case) were 13.26, 21.66, and 25.91 g, respectively.(a) Do these data establish that carbon dioxide has a fixed composition?(b) What is the
The following data were obtained for compounds of nitrogen and hydrogen:(a) Show that these data are consistent with the law of multiple proportions.(b) If the formula of compound B is N2H2 what are the formulas of compounds A and C? Compound A B C с Mass of Nitrogen, g 0.500 1.000 0.750 Mass
The following data were obtained for compounds of iodine and fluorine:(a) Show that these data are consistent with the law of multiple proportions.(b) If the formula for compound A is IF, what are the formulas for compounds B, C, and D? Compound A B C D Mass of lodine,
There are two oxides of copper. One oxide has 20% oxygen, by mass. The second oxide has a smaller percent of oxygen than the first. What is the probable percent of oxygen in the second oxide?
The two oxides of carbon described were CO and CO2. Another oxide of carbon has 1.106 g of oxygen in a 2.350 g sample. In what ratio are carbon and oxygen atoms combined in molecules of this third oxide? Explain.
In an experiment similar to that described in Exercise 19, drop 1 carried a charge of 6.41 x 10-19 C; drop 2 had 1/2 the charge of drop 1; drop 3 had twice the charge of drop 1; drop 4 had a charge of 1.44 x 10-18 C; and drop 5 had 1/3 the charge of drop 4. Are these data consistent with the value
Complete the following table. What minimum amount of information is required to completely characterize an atom or ion? Name Sodium Silicon Symbol Na 40K - 20Ne²+ Number Protons Number Electrons 11 37 11 33 Number Neutrons 12 14 42 126 Mass Number 23 | 8 | | | | 85 80
Arrange the following species in order of increasing(a) Number of electrons; (b) Number of neutrons;(c) Mass. Sn Ar Te Cu 12Cd Co K 40 122 120,
For the atom 108Pd with mass 107.90389 u, determine(a) The numbers of protons, neutrons, and electrons in the atom;(b) The ratio of the mass of this atom to that of an atom of 126C.
The following data on isotopic masses are from a chemical handbook. What is the ratio of each of these masses to that of 126C?(a) 3517Cl, 34.96885 u; (b) 2612Mg, 25.98259 u; (c) 22286Rn, 222.0175 u.
For the mineral torbernite, Cu(UO2)2(PO4)2 . 8 H2O, determine(a) The total number of atoms in one formula unit;(b) The ratio, by number, of H atoms to O atoms;(c) The ratio, by mass, of Cu to P;(d) The element present in the greatest mass percent;(e) The mass required to contain 1.00 g P.
Determine the mass percent H2O in the hydrate Cr(NO3)3 . 9 H2O.
A 1.562 g sample of the alcohol CH3CHOHCH2CH3 is burned in an excess of oxygen. What masses of CO2 and H2O should be obtained?
Name these compounds: (a) Ba(NO3)2;(b) HNO2 ;(c) CrO2; (d) KIO3;(e) LiCN; (f) KIO; (g) Fe(OH)2;(h) Ca(H2PO4)2; (i) H3PO4; (j) NaHSO4; (k) Na2Cr2O7;(l) NH4C2H3O2; (m) MgC2O4; (n) Na2C2O4.
Assign suitable names to the compounds (a) CS2(b) SiF4(c) ClF5(d) N2O5(e) SF6(f) I2Cl6.
Write formulas for the compounds: (a) Aluminum sulfate;(b) Ammonium dichromate; (c) Silicon tetrafluoride;(d) Iron(III) oxide;(e) Tricarbon disulfide;(f) Cobalt(II) nitrate; (g) Strontium nitrite; (h) Hydrobromic acid;(i) Iodic acid; (j) Phosphorus dichloride trifluoride.
Write formulas for the compounds: (a) Magnesium perchlorate; (b) Lead(II) acetate; (c) Tin(IV) oxide;(d) Hydroiodic acid;(e) Chlorous acid; (f) Sodium hydrogen sulfite; (g) Calcium dihydrogen phosphate;(h) Aluminum phosphate; (i) Dinitrogen tetroxide;(j) Disulfur dichloride.
Write a formula for (a) The chloride of titanium having Ti in the O.S. +4; (b) The sulfate of iron having Fe in the O.S. +3; (c) An oxide of chlorine with Cl in the O.S. +7; (d) An oxoanion of sulfur in which the apparent O.S. of S is +7 and the ionic charge is -2.
Write a formula for (a) An oxide of nitrogen with N in the O.S. +5; (b) An oxoacid of nitrogen with N in the O.S. +3; (c) An oxide of carbon in which the apparent O.S. of C is +4/3; (d) A sulfur-containing oxoanion in which the apparent O.S. of S is +2.5 and the ionic charge is -2.
Name the acids: (a) HClO2(b) H2SO3(c) H2Se;(d) HNO2.
Supply the formula for the acids: (a) Hydrofluoric acid; (b) Nitric acid; (c) Phosphorous acid; (d) Sulfuric acid.
Name the following compounds and specify which ones are best described as ionic: (a) OF2; (b) XeF2;(c) CuSO3; (d) (NH4)2HPO4.
Name the following compounds and specify which ones are best described as ionic: (a) KNO2; (b) BrF3;(c) S2Cl2; (d) Mg(ClO)2; (e) Cl2O.
Without performing detailed calculations, indicate which of the following hydrates has the greatest % H2O by mass: CuSO4 · 5 H2O, Cr2(SO4)3 · 18 H2O, MgCl2 · 6 H2O, and LiC2H3O2 · 2 H2O.
Without performing detailed calculations, determine the hydrate of Na2SO3 that contains almost exactly 50% H2O, by mass.
(A) For the reaction 4 NH3 + 3 O3 → 2 N2 + 6 H2O, how many grams of NH3 are consumed per gram of O2?(B) In the combustion of octane, C8H18 how many grams of O2 are consumed per gram of octane?
In the United States, the concentration of glucose, C6H12O6, in the blood is reported in units of milligrams per deciliter (mg/dL). In Canada, the United Kingdom, and elsewhere, the blood glucose concentration is reported in millimoles per liter (mmol/L), where 1 mmol = 1 x 10 3 mol. If a person
A 25.00 mL sample of HCl(aq) was added to a 0.1000 g sample of CaCO3 All the CaCO3 reacted, leaving some excess HCl(aq).CaCO3(s) + 2 HCl(aq)→CaCl2(aq) + H2O(l) + CO2(g)The excess HCl(aq) required 43.82 mL of 0.01185 M Ba(OH)2 to complete the following reaction. What was the molarity of the
The following set of reactions is to be used as the basis of a method for producing nitric acid, HNO3. Calculate the minimum masses of N2, H2, and O2 required per kilogram of HNO3.N2(g) 3 H2(g) → 2 NH3(g) 4 NH3(g) 5 O2(g) → 4 NO(g) 6 H2O(g) 2 NO(g) O2(g) → 2 NO2(g) 3 NO2(g) H2O(l) → 2
A 2.05 g sample of an iron–aluminum alloy (ferroaluminum) is dissolved in excess HCl(aq) to produce 0.105 g H2(g). What is the percent composition, by mass, of the ferroaluminum?Fe(s) + 2 HCl(aq) → FeCl2(aq) + H2(g) 2 Al(s) + 6 HCl(aq) → 2 AlCl3(aq) + 3 H2(g).
Aluminum sulfate, Al2(SO4)3, is a strong electrolyte. What are the aluminum and sulfate ion concentrations in 0.0165 M Al2(SO4)3?
(A) Seawater is approximately 0.438 M NaCl and 0.0512 M MgCl2. What is the molarity of Cl-—that is, the total [Cl-]—in seawater?(B) A water treatment plant adds fluoride ion to the water to the extent of 1.5 mg F-/L.(a) What is the molarity of fluoride ion in this water?(b) If the fluoride ion
(1) Which solution is the best electrical conductor?(a) 0.50 M CH3COCH3;(b) 0.50 M CH3CH2OH;(c) 1.00 M CH2(OH)CH(OH)CH2OH;(d) 0.050 M CH3COOH;(e) 0.025 M RbNO3.(2) Which solution has the highest total molarity of ions?(a) 0.008 M Ba(OH)2;(b) 0.010 M KI; (c) 0.011 M CH3COOH;(d) 0.030 M
Sodium dithionite, Na2S2O4, is an important reducing agent. One interesting use is the reduction of chromate ion to insoluble chromium(III) hydroxide by dithionite ion, S2O42- in basic solution. Sulfite ion is another product. The chromate ion may be present in wastewater from a chromium-plating
Using information from this chapter, indicate whether each of the following substances in aqueous solution is a nonelectrolyte, weak electrolyte, or strong electrolyte.(a) HC6H5O; (b) Li2SO4;(c) MgI2;(d) (CH3CH2)2O;(e) Sr(OH)2.
Predict whether a reaction will occur in each of the following cases. If so, write a net ionic equation for the reaction.(a) NaOH(aq) + MgCl2(aq) → ?(b) BaS(aq) + CuSO4(aq) → ?(c) (NH4)2SO4(aq) + ZnCl2(aq) → ?
Apply the solubility guidelines in Table 5.1 to predict whether each of the following solids is water soluble or insoluble. For which are the solubility guidelines inconclusive? (a) Al2(SO4)3; (b) Cr(OH)3; (c) K3PO4; (d) Li2CO3;(e) ZnS; (f ) Mg(MnO4)2; (g) AgClO4; (h) CaSO4; (i) PbO.Table
(A) Indicate whether a precipitate forms by completing each equation as a net ionic equation. If no reaction occurs, so state.(a) AlCl3(aq) + KOH(aq) → ?(b) K2SO4(aq) + FeBr3(aq) → ?(c) CaI2(aq) + Pb(NO3)2(aq) → ?(B) Indicate through a net ionic equation whether a precipitate forms when the
Select the (a) Best and (b) Poorest electrical conductors from the following solutions, and explain the reason for your choices: 0.10 M NH3; 0.10 M NaCl; 0.10 M CH3COOH (acetic acid); 0.10 M CH3CH2OH (ethanol).
Write a net ionic equation to represent the reaction of (a) Aqueous strontium hydroxide with nitric acid;(b) Solid aluminum hydroxide with hydrochloric acid.
(A) Write a net ionic equation to represent the reaction of aqueous ammonia with propionic acid, CH3CH2COOH. Assume that the neutralization reaction goes to completion. What is the formula of the salt that results from this neutralization?(B) Calcium carbonate is a major constituent of the hard
What response would you expect in the apparatus of Figure 5-4 if the solution tested were 1.0 M HCl? What response would you expect if the solution were both 1.0 M HCl and 1.0 M CH3COOH?Figure 5-4 (a) 2+ (b) 2+ + (c)
You are given the four solids, K2CO3, CaO, ZnSO4, and BaCO3, and three solvents, H2O(l), HCl(aq), and H2SO4(aq). You are asked to prepare four solutions, each containing one of the four cations, that is, one with K+(aq), one with Ca2+(aq), and so on. Using water as your first choice, what solvent
Indicate whether each of the following is an oxidation–reduction reaction.(a) MnO2(s) + 4 H+(aq) + 2 Cl-(aq) → Mn2+(aq) + 2 H2O(l) + Cl2(g)(b) H2PO4-(aq) + OH-(aq) → HPO42-(aq) + H2O(l)
(A) Identify whether each of the following is an oxidation–reduction reaction.(a) (NH4)2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2 NH4NO3(aq)(b) 2 Pb(NO3)2(s) → 2 PbO(s) + 4 NO2(g) + O2(g)(B) Identify the species that is oxidized and the species that is reduced in the reaction below.5 VO2+(aq) +
Disregarding the fact that the expressions below are not balanced, is it likely that either represents a reaction that could possibly occur? Explain.(a) MnO4-(aq) + Cr2O72-(aq) + H+(aq) → MnO2(s) + Cr3+(aq) + H2O(l)(b) Cl2(g) + OH-(aq) → Cl-(aq) + ClO3-(aq) + H2O(l)
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