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chemistry a molecular approach

Chemistry A Molecular Approach 5th Edition Nivaldo Tro - Solutions

Write an equilibrium expression for each chemical equation involving one or more solid or liquid reactants or products. a. CO3²- (aq) + H₂O(1) b. 2 KCIO3(s) = 2 KCl(s) + 3 O₂(g) c. HF(aq) + H₂O(1) H3O+ (aq) + F(aq) d. NH3(aq) + H₂O(1) ⇒ NH‡ (aq) + OH (aq) HCO3(aq) + OH (aq)
Find and fix the mistake in the equilibrium expression. PC15 (8) PC13(1) + Cl₂(g) Ke [PC13][C1₂] [PC]s]
Consider the reaction:An equilibrium mixture of this reaction at a certain temperature has [CO] = 0.105 M, [H2] = 0.114 M, and [CH3OH] = 0.185 M.What is the value of the equilibrium constant (Kc) at this temperature? CO(g) + 2 H₂(g) CH3OH(g)
Consider the reaction:An equilibrium mixture of this reaction at a certain temperature has [NH3] = 0.278 M and [H2S] = 0.355 M. What is the value of the equilibrium constant (Kc) at this temperature? NH4HS(S) - NH3(g) + H₂S(g)
Consider the reaction:In a reaction mixture at equilibrium, the partial pressure of NO is 108 torr and that of Br2 is 126 torr. What is the partial pressure of NOBr in this mixture? 2 NO(g) + Br₂(g) = 2 NOBr(g) Kp = 28.4 at 298 K
Consider the reaction:In a reaction at equilibrium, the partial pressure of SO2 is 137 torr and that of Cl2 is 285 torr. What is the partial pressure of SO2Cl2 in this mixture? SO₂C12 (8) SO2(g) + Cl₂(g) Kp = 2.91 × 10³ at 298 K
For the reaction A(g) ⇌ 2 B(g), a reaction vessel initially contains only A at a pressure of PA = 1.32 atm. At equilibrium, PA = 0.25 atm. Calculate the value of Kp.
Consider the reaction:A solution is made containing an initial [Fe3 + ] of 1.0 * 10-3 M and an initial [SCN–] of 8.0 * 10-4 M. At equilibrium, [FeSCN2 + ] = 1.7 * 10-4 M. Calculate the value of the equilibrium constant (Kc). Fe³+ (aq) + SCN (aq) FeSCN²+ (aq)
For the reaction 2 A(g) ⇌ B(g) + 2 C(g), a reaction vessel initially contains only A at a pressure of PA = 255 mmHg. At equilibrium, PA = 55 mmHg. Calculate the value of Kp.
Consider the reaction:A reaction mixture is made containing an initial [SO2Cl2] of 0.020 M. At equilibrium, [Cl2] = 1.2 * 10-2 M. Calculate the value of the equilibrium constant (Kc). SO₂Cl2(8) SO₂(g) + Cl₂(g)
Consider the reaction:A reaction mixture in a 3.67-L flask at a certain temperature initially contains 0.763 g H2 and 96.9 g I2. At equilibrium, the flask contains 90.4 g HI. Calculate the equilibrium constant (Kc) for the reaction at this temperature. H₂(8) + 12(g) 2 HI(g)
Consider the reaction:A reaction mixture in a 5.19-L flask at a certain temperature contains 26.9 g CO and 2.34 g H2. At equilibrium, the flask contains 8.65 g CH3OH. Calculate the equilibrium constant (Kc) for the reaction at this temperature. CO(g) + 2 H₂(g) = CH₂OH(g)
Consider the reaction:At a certain temperature, Kc = 8.5 * 10-3. A reaction mixture at this temperature containing solid NH4HS has [NH3] = 0.166 M and [H2S] = 0.166 M. Will more of the solid form or will some of the existing solid decompose as equilibrium is reached? NH4HS(s) NH3(g) + H₂S(g)
Consider the reaction:A reaction mixture contains 0.112 atm of H2, 0.055 atm of S2, and 0.445 atm of H2S. Is the reaction mixture at equilibrium? If not, in what direction will the reaction proceed? 2 H₂S(g) = 2 H₂(g) + S₂(g) Kp = 2.4 x 104 at 1073 K
Silver sulfate dissolves in water according to the reaction:A 1.5-L solution contains 6.55 g of dissolved silver sulfate. If additional solid silver sulfate is added to the solution, will it dissolve? Ag2SO4(s) 2 Ag+ (aq) + SO42- (aq) K 1.1 x 10-5 at 298 K =
Nitrogen dioxide dimerizes according to the reaction:A 2.25-L container contains 0.055 mol of NO2 and 0.082 mol of N2O4 at 298 K. Is the reaction at equilibrium? If not, in what direction will the reaction proceed? 2 NO2(g) N₂O4(8) Kp = 6.7 at 298 K
Consider the reaction and the associated equilibrium constant:Find the equilibrium concentrations of A and B for each value of a and b. Assume that the initial concentration of A in each case is 1.0 M and that no B is present at the beginning of the reaction.a. a = 1; b = 1 b. a = 2; b = 2 c. a =
Consider the reaction and the associated equilibrium constant:Find the equilibrium concentrations of A, B, and C for each value of a, b, and c. Assume that the initial concentrations of A and B are each 1.0 M and that no product is present at the beginning of the reaction.a. a = 1; b = 1; c = 2 b.
For the reaction shown here, Kc = 0.513 at 500 K.N2O4( g) ⇌ 2 NO2(g)If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?
Consider the reaction: If a mixture of solid nickel(II) oxide and 0.20 M carbon monoxide comes to equilibrium at 1500 K, what is the equilibrium concentration of CO2? NiO(s) + CO(g) Ni(s) + CO₂(g) K 4.0 x 10³ at 1500 K =
For the reaction shown here, Kc = 255 at 1000 K.CO(g) + Cl2(g) ⇌ COCl2(g)If a reaction mixture initially contains a CO concentration of 0.1500 M and a Cl2 concentration of 0.175 M at 1000 K, what are the equilibrium concentrations of CO, Cl2, and COCl2 at 1000 K?
Consider the reaction:If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O+ at 25 °C? HC₂H3O₂ (aq) + H₂O(1) H3O+(aq) + C₂H3O₂ (aq) K 1.8 x 10-5 at 25 °C =
Consider the reaction:If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C? SO₂Cl₂(g) = SO₂(g) + Cl₂(g) K 2.99 x 10-7 at 227 °C =
Consider the reaction:A reaction mixture initially contains a Br2 partial pressure of 755 torr and a Cl2 partial pressure of 735 torr at 150 K. Calculate the equilibrium partial pressure of BrCl. Br₂(g) + Cl₂(g) 2 BrCI(g) Kp = 1.11 × 10-¹ at 150 K
Consider the reaction:A reaction mixture initially contains a CO partial pressure of 1344 torr and a H2O partial pressure of 1766 torr at 2000 K. Calculate the equilibrium partial pressures of each of the products. CO(g) + H₂O(g) CO₂(g) + H₂(g) Kp = 0.0611 at 2000 K
Consider the reaction:Find the equilibrium partial pressures of A and B for each value of Kp. Assume that the initial partial pressure of B in each case is 1.0 atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions.a. Kp = 1.0b. Kp = 1.0 * 10-4c. Kp
Consider this reaction at equilibrium:Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance.a. COCl2 is added to the reaction mixture.b. Cl2 is added to the reaction mixture.c. COCl2 is removed from the reaction mixture. CO(g) + Cl₂(g) = COCI₂(g)
Consider this reaction at equilibrium:Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance.a. NO is added to the reaction mixture.b. BrNO is added to the reaction mixture.c. Br2 is removed from the reaction mixture. 2 BrNO (g) 2 NO(g) 2 NO(g) +
Consider this reaction at equilibrium:Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance.a. O2 is removed from the reaction mixture.b. KCl is added to the reaction mixture.c. KClO3 is added to the reaction mixture.d. O2 is added to the reaction
Consider this reaction at equilibrium:Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance.a. C is added to the reaction mixture.b. H2O is condensed and removed from the reaction mixture.c. CO is added to the reaction mixture.d. H2 is removed from
Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. a. 1₂(g) 21(g) (volume is increased) b. 2 H₂S(g) = 2 H₂(g) + S₂(g) (volume is decreased) c. I₂(g) +
Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. CO₂(g) + H₂(g) (volume is decreased) PCI,(g) (volume is increased) a. CO(g) + H₂O(g) - - b. PC13(g) +
This reaction is exothermic.Predict the effect (shift right, shift left, or no effect) of increasing and decreasing the reaction temperature. How does the value of the equilibrium constant depend on temperature? C6H1206(S) + 6 0₂(g) +6 0₂(g) → 6 CO₂(g) 6 CO₂(g) + 6H₂O(g)
Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction:Which disturbance will favor CH4 at equilibrium?a. Adding more C to the reaction mixture b. Adding more H2 to the reaction mixture c. Raising the temperature of the reaction mixture d.
Carbon monoxide replaces oxygen in oxygenated hemoglobin according to the reaction:a. Use the reactions and associated equilibrium constants at body temperature given here to find the equilibrium constant for the reaction just shown.b. Suppose that an air mixture becomes polluted with carbon
Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction:If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional or less hydrogen gas, or have no effect on the quantity of hydrogen gas.a. Adding more C
Nitrogen monoxide is a pollutant in the lower atmosphere that irritates the eyes and lungs and leads to the formation of acid rain. Nitrogen monoxide forms naturally in atmosphere according to the endothermic reaction:Use the ideal gas law to calculate the concentrations of nitrogen and oxygen
The reaction CO2(g) + C(s) ⇌ 2 CO(g) has Kp = 5.78 at 1200 K.a. Calculate the total pressure at equilibrium when 4.45 g of CO2 is introduced into a 10.0-L container and heated to 1200 K in the presence of 2.00 g of graphite.b. Repeat the calculation of part a in the presence of 0.50 g of graphite.
Which compound do you expect to be most soluble in octane (C8H18)?a) CH3OH b) CBr4 c) H2O d) NH3
Vitamins are often categorized as either fat-soluble or water-soluble. Water-soluble vitamins, on one hand, dissolve in body fluids and are easily eliminated in the urine, so there is little danger of overconsumption. Fat-soluble vitamins, on the other hand, can accumulate in the body’s fatty
Explain why drinking seawater results in dehydration.
An aqueous solution is saturated in both potassium chlorate and carbon dioxide gas at room temperature. What happens when the solution is warmed to 85 °C?a) Potassium chlorate precipitates out of solution.b) Carbon dioxide bubbles out of solution.c) Potassium chlorate precipitates out of solution
What pressure of carbon dioxide is required to keep the carbon dioxide concentration in a bottle of club soda at 0.12 M at 25 °C? SORT You are given the desired solubility of carbon dioxide and asked to find the pressure required to achieve this solubility. STRATEGIZE Use Henry's law to find the
What is a solution? What are the solute and solvent?
If the solvent–solute interactions in a mixture are comparable in strength to the solvent–solvent interactions and the solute–solute interactions, what can you conclude about solution formation in this mixture?(a) A homogeneous solution forms.(b) A homogeneous solution does not form.(c) The
A 500.0-mL sample of pure water is allowed to come to equilibrium with pure oxygen gas at a pressure of 755 mmHg.What mass of oxygen gas dissolves in the water? (The Henry’s law constant for oxygen gas is 1.3 * 10-3 M/atm.)a) 15.7 g b) 6.5 * 10-3 gc) 0.041 g d) 0.021 g
What volume (in mL) of a soft drink that is 10.5% sucrose (C12H22O11) by mass contains 78.5 g of sucrose?(The density of the solution is 1.04 g/mL.) SORT You are given a mass of sucrose and the concentration and density of a sucrose solution, and you are asked to find the volume of
What does it mean to say that a substance is soluble in another substance? Which units are used in reporting solubility?
A potassium bromide solution is 7.55 % potassium bromide by mass, and its density is 1.03 g/mL. What mass of potassium bromide is contained in 35.8 mL of the solution?a) 2.78 g b) 2.70 gc) 4.88 g d) 2.62 g
Why do two ideal gases thoroughly mix when combined? What drives the mixing?
The enthalpy of solution for cesium fluoride is -36.8 kJ/mol. What can you conclude about the relative magnitudes of ΔHsolute and ΔHhydration? (a) AHsolute>|AHhydration (b) AHsolute
A solution is prepared by dissolving 17.2 g of ethylene glycol (C2H6O2) in 0.500 kg of water. The final volume of the solution is 515 mL. Calculate the concentration of the solution in each unit.(a) Molarity (b) Molality (c) Percent by mass (d) Mole fraction (e) Mole percent
What is the molarity of a 6.56% by mass glucose (C6H12O6) solution? (The density of the solution is 1.03 g/mL.) SORT You are given the con- centration of a glucose solution in percent by mass and the density of the solution. Find the concentra- tion of the solution in molarity. STRATEGIZE Begin
A solution contains 22.4 g glucose (C6H12O6) dissolved in 0.500 L of water. What is the molality of the solution?(Assume a density of 1.00 g/mL for water.)a) 0.238 m b) 44.8 mc) 0.249 m d) 4.03 m
What is entropy? Why is entropy important in discussing the formation of solutions?
A solution is saturated in both nitrogen gas and potassium bromide at 75 °C. When the solution is cooled to room temperature, what is most likely to happen?(a) Some nitrogen gas bubbles out of solution.(b) Some potassium bromide precipitates out of solution.(c) Some nitrogen gas bubbles out of
Calculate the vapor pressure at 25 °C of a solution containing 99.5 g sucrose (C12H22O11) and 300.0 mL water.The vapor pressure of pure water at 25 °C is 23.8 torr. Assume the density of water is 1.00 g/mL. SORT You are given the mass of sucrose and volume of water in a solution. You are
A sodium nitrate solution is 12.5% NaNO3 by mass and has a density of 1.02 g/mL. Calculate the molarity of the solution.a) 1.44 M b) 12.8 Mc) 6.67 M d) 1.50 M
What kinds of intermolecular forces are involved in solution formation?
Examine the Henry’s law constants in Table 14.4. Why is the constant for ammonia larger than the others?(a) Because ammonia is polar and the other substances in the table are nonpolar.(b) Because ammonia has the highest molar mass of the substances listed in the table.(c) Because ammonia is
A solution contains 3.95 g of carbon disulfide (CS2) and 2.43 g of acetone (CH3COCH3). At 35 °C the vapor pressures of pure carbon disulfide and pure acetone are 515 torr and 332 torr, respectively. Assuming ideal behavior, calculate the vapor pressures of each component and the total vapor $Use the mole fraction of each component along with Raoult's law to calculate the par- tial pressure of each$
Determine the vapor pressure at 25 °C of an aqueous ethylene glycol (C2H6O2) solution that is 14.8 % C2H6O2 by mass. The vapor pressure of pure water at 25 °C is 23.8 torr.a) 3.52 torr b) 22.7 torrc) 1.14 torr d) 20.3 torr
Explain how the relative strengths of solute–solute interactions, solvent–solvent interactions, and solvent–solute interactions affect solution formation.
A solution contains a mixture of substance A and substance B, both of which are volatile. The mole fraction of substance A is 0.35. At 32 °C the vapor pressure of pure A is 87 mmHg, and the vapor pressure of pure B is 122 mmHg. What is the total vapor pressure of the solution at this
What does the statement like dissolves like mean with respect to solution formation?
Calculate the freezing point of a 1.7 m aqueous ethylene glycol solution. SORT You are given the molality of a solution and asked to find its freezing point. STRATEGIZE To solve this problem, use the freezing point depression equation. GIVEN: 1.7 m solution FIND: freezing point (from
What is the vapor pressure of a solution in which the mole fraction of the solute is 0.200 and the vapor pressure of the pure solvent is 100.0 torr? (Assume a single nonvolatile, nonelectrolyte solute).(a) 20.0 torr(b) 80.0 torr(c) 100.0 torr(d) 120.0 torr
A solution contains equal amounts (in moles) of liquid components A and B. The vapor pressure of pure A is 100 mmHg and that of pure B is 200 mmHg. The experimentally measured vapor pressure of the solution is 120 mmHg.What are the relative strengths of the solute–solute, solute–solvent, and
What mass of glucose (C6H12O6) should be dissolved in 10.0 kg of water to obtain a solution with a freezing point of -4.2 °C?a) 0.023 kg b) 4.1 kgc) 0.41 kg d) 14.1 kg
What mass of ethylene glycol (C2H6O2), in grams, must be added to 1.0 kg of water to produce a solution that boils at 105.0 °C? SORT You are given the desired boiling point of an ethylene glycol solution con- taining 1.0 kg of water and asked to find the mass of ethylene glycol you need to add
What are the three steps involved in evaluating the enthalpy changes associated with solution formation?
Solution A is a 1.0 m solution with a nonionic solute and water as the solvent. Solution B is a 1.0 m solution with the same nonionic solute and ethanol as the solvent. Which solution has the greater increase in its boiling point (relative to the pure solvent)?(a) Solution A (b) Solution B
Which of these aqueous solutions has the highest boiling point?a) 1.25 M C6H12O6b) 1.25 M KNO3c) 1.25 M Ca(NO3)2d) None of the above (they all have the same boiling point)
The osmotic pressure of a solution containing 5.87 mg of an unknown protein per 10.0 mL of solution is 2.45 torr at 25 °C. Find the molar mass of the unknown protein. SORT You are told that a solution of an unknown protein contains 5.87 mg of the protein per 10.0 mL of solution. You are also given
What is the heat of hydration (ΔHhydration)? How does the enthalpy of solution depend on the relative magnitudes of ΔHsolute and ΔHhydration?
Which aqueous solution has the highest boiling point?(a) 0.50 M C12H22O11(b) 0.50 M NaCl(c) 0.50 M MgCl2
The osmotic pressure of a solution containing 22.7 mg of an unknown protein in 50.0 mL of solution is 2.88 mmHg at 25 °C.Determine the molar mass of the protein.a) 246 g/mol b) 3.85 g/molc) 2.93 * 103 g/mol d) 147 g/mol
The freezing point of an aqueous 0.050 m CaCl2 solution is -0.27 °C. What is the van’t Hoff factor (i) for CaCl2 at this concentration? How does it compare to the expected value of i? SORT You are given the molality of a solution and its freezing point. You are asked to find the value of i, the
Explain dynamic equilibrium with respect to solution formation.What is a saturated solution? An unsaturated solution?A supersaturated solution?
The enthalpy of solution for NaOH is -44.46 kJ/mol. What can you conclude about the relative magnitudes of the absolute values of ΔHsolute and ΔHhydration, where ΔHsolute is the heat associated with separating the solute particles and ΔHhydration is the heat associated with dissolving the
A solution contains 0.102 mol Ca(NO3)2 and 0.927 mol H2O. Calculate the vapor pressure of the solution at 55 °C.The vapor pressure of pure water at 55 °C is 118.1 torr. (Assume that the solute completely dissociates.) SORT You are given the number of moles of each com- ponent of a solution and
How does the solubility of a solid in a liquid depend on temperature?How is this temperature dependence exploited to purify solids through recrystallization?
A 2.4 m aqueous solution of an ionic compound with the formula MX2 has a boiling point of 103.4 °C. Calculate the van’t Hoff factor (i) for MX2 at this concentration.a) 2.8 b) 83c) 0.73 d) 1.0
How does the solubility of a gas in a liquid depend on temperature?How does this temperature dependence affect the amount of oxygen available for fish and other aquatic animals?
A solution is an equimolar mixture of two volatile components A and B. Pure A has a vapor pressure of 50 torr, and pure B has a vapor pressure of 100 torr. The vapor pressure of the mixture is 85 torr. What can you conclude about the relative strengths of the intermolecular forces between particles
An aqueous solution at 25 °C is in equilibrium with a gaseous mixture containing an equal number of moles of oxygen, nitrogen, and helium. Rank the relative concentrations of each gas in the aqueous solution from highest to lowest. a) [0₂] > [N₂] > [He] c) [N₂] > [He] > [0₂] b) [He] >
How does the solubility of a gas in a liquid depend on pressure?How does this pressure dependence account for the bubbling that occurs upon opening a can of soda?
What is Henry’s law? For what kinds of calculations is Henry’s law useful?
What are the common units for expressing solution concentration?
How are parts by mass and parts by volume used in calculations?
What is the effect of a nonvolatile solute on the vapor pressure of a liquid? Why is the vapor pressure of a solution different from the vapor pressure of the pure liquid solvent?
What is Raoult’s law? For what kind of calculations is Raoult’s law useful?
Explain the difference between an ideal and a nonideal solution.
What is the effect on vapor pressure of a solution with particularly strong solute–solvent interactions? With particularly weak solute–solvent interactions?
Explain why the lower vapor pressure for a solution containing a nonvolatile solute results in a higher boiling point and lower melting point compared to the pure solvent.
What are colligative properties?
What is osmosis? What is osmotic pressure?
Explain the meaning of the van’t Hoff factor and its role in determining the colligative properties of solutions containing ionic solutes.
Describe a colloidal dispersion. What is the difference between a colloidal dispersion and a true solution?
What is the Tyndall effect, and how can it be used to help identify colloidal dispersions?

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