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chemistry
physical chemistry

Chemical Principles 7th edition Steven S. Zumdahl, Donald J. DeCoste - Solutions

For the reaction 2H2O(g) ⇌ 2H2(g) + O2(g) K = 2.4 × 10-3 at a given temperature. At equilibrium in a 2.0- L container, it is found that [H2O(g)] = 1.1 × 10-1 M and [H2(g)] = 1.9 × 10-2 M. Calculate the moles of O2(g) present under these conditions.
The reaction 2NO(g) + Br2(g) ⇌ 2NOBr(g) as Kp = 109 at 25oC. If the equilibrium partial pressure of Br2 is 0.0159 atm and the equilibrium partial pressure of NOBr is 0.0768 atm, calculate the partial pressure of NO at equilibrium.
In a study of the reaction 3Fe(s) + 4H2O(g) ⇌ Fe3O4(s) + 4H2(g) at 1200 K, it was observed that when the equilibrium partial pressure of water vapor is 15.0 torr, the total pressure at equilibrium is 36.3 torr. Calculate Kp for this reaction at 1200 K.
Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200oC in a closed container, 1.00 atm of nitrogen gas is mixed with 2.00 atm of hydrogen gas. At equilibrium, the total pressure is 2.00 atm. Calculate the partial pressure of hydrogen gas at equilibrium, and calculate the
A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.50 atm at 523 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the actual pressure in the flask was found to be 0.84 atm. Calculate Kp for the decomposition reaction PCl5(g) ⇌
A sample of S8(g) is placed in an otherwise empty, rigid container at 1325 K at an initial pressure of 1.00 atm, where it decomposes to S2(g) by the reaction S8(g) ⇌ 4S2(g) At equilibrium, the partial pressure of S8 is 0.25 atm. Calculate Kp for this reaction at 1325 K.
At a particular temperature, 12.0 moles of SO3 is placed into a 3.0- L rigid container, and the SO3 dissociates by the reaction 2SO3(g) ⇌ 2SO2(g) + O2(g) At equilibrium, 3.0 moles of SO2 is present. Calculate K for this reaction.
At a particular temperature, 8.0 moles of NO2 is placed into a 1.0- L container and the NO2 dissociates by the reaction 2NO2(g) ⇌ 2NO(g) + O2(g) At equilibrium the concentration of NO(g) is 2.0 M. Calculate K for this reaction. Equilibrium Calculations.
The equilibrium constant is 0.0900 at 25oC for the reaction H2O(g) + Cl2O(g) ⇌ 2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those which are not at equilibrium, in which direction will the system shift? a. A 1.0- L flask contains 1.0 mole of HOCl, 0.10
The equilibrium constant is 0.0900 at 25oC for the reaction H2O(g) + Cl2O(g) ⇌ 2HOCl(g) For which of the following sets of conditions is the system at equilibrium? For those which are not at equilibrium, in which direction will the system shift? a. PH2O = 1.00 atm, PCl2O = 1.00 atm, PHOCl = 1.00
At 900oC, Kp = 1.04 for the reaction CaCO3(s) ⇌ CaO(s) + CO2(g) At a low temperature dry ice (solid CO2), calcium oxide, and calcium carbonate are introduced into a 50.0- L reaction chamber. The temperature is raised to 900oC. For the following mixtures, will the initial amount of calcium oxide
At a particular temperature, K = 3.75 for the reaction SO2(g) + NO2(g) ⇌ SO3(g) + NO(g) If all four gases had initial concentrations of 0.800 M, calculate the equilibrium concentrations of the gases.
At 25oC, K = 0.090 for the reaction H2O(g) + Cl2O(g) ⇌ 2HOCl(g) Calculate the concentrations of all species at equilibrium for each of the following cases. a. 1.0 g of H2O and 2.0 g of Cl2O are mixed in a 1.0- L flask. b. 1.0 mole of pure HOCl is placed in a 2.0- L flask.
For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.00-L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. H2(g) + F2(g) ⇌ 2HF(g) If 0.200 mole of F2 is added to this equilibrium mixture, calculate the concentrations of
At 1100 K, Kp = 0.25 for the following reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g) Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which PSO2 = PO2 = 0.50 atm and PSO3 = 0.
At 2200oC, K = 0.050 for the reaction N2(g) + O2(g) ⇌ 2NO(g) What is the partial pressure of NO at equilibrium assuming the N2 and O2 had initial pressures of 0.80 atm and 0.20 atm, respectively?
A type of reaction we will study is that having a very small K value (K,, 1). Solving for equilibrium concentrations in an equilibrium problem usually requires many mathematical operations to be performed. However, the math involved in solving equilibrium problems for reactions having small K
At 35oC, K = 1.6 × 10-5 for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl2(g) Calculate the concentrations of all species at equilibrium for each of the following original mixtures. a. 2.0 moles of pure NOCl in a 2.0- L flask b. 2.0 moles of NO and 1.0 mole of Cl2 in a 1.0- L flask c. 1.0 mole of NOCl and
At a particular temperature, K = 2.0 × 10-6 for the reaction 2CO2(g) ⇌ 2CO(g) + O2(g) If 2.0 moles of CO2 is initially placed into a 5.0-L vessel, calculate the equilibrium concentrations of all species.
At a particular temperature, Kp = 0.25 for the reaction N2O4(g) ⇌ 2NO2(g) a. A flask containing only N2O4 at an initial pressure of 4.5 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases. b. A flask containing only NO2 at an initial pressure of 9.0 atm
For the reaction below, Kp = 1.16 at 800oC. CaCO3(s) ⇌ CaO(s) + CO2(g) If a 20.0- g sample of CaCO3 is put into a 10.0- L container and heated to 800oC, what percentage by mass of the CaCO3 will react to reach equilibrium?
At 25oC, Kp = 2.9 × 10-3 for the reaction NH4OCONH2(s) ⇌ 2NH3(g) + CO2(g) In an experiment carried out at 25oC, a certain amount of NH4OCONH2 is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.
Lexan is a plastic used to make compact discs, eyeglass lenses, and bullet-proof glass. One of the compounds used to make Lexan is phosgene (COCl2), a poisonous gas. Phosgene is produced by the reaction CO(g) + Cl2(g) ⇌ COCl2(g) for which K = 4.5 × 109 at 100.8C. a. Calculate Kp at 100.oC. b.
At a certain temperature, K = 1.1 × 103 for the reaction Fe3+(aq) + SCN2(aq) ⇌ FeSCN2+(aq) Calculate the concentrations of Fe3+, SCN2, and FeSCN21 at equilibrium if 0.020 mole of Fe(NO3)3 is added to 1.0 L of 0.10 M KSCN. (Neglect any volume change.)
Which of the following statements is(are) true? Correct the false statement(s). a. When a reactant is added to a system at equilibrium at a given temperature, the reaction will shift right to reestablish equilibrium. b. When a product is added to a system at equilibrium at a given temperature, the
How will the equilibrium position of a gas- phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift
Suppose the reaction system UO2(s) + 4HF(g) ⇌ UF4(g) + 2H2O(g) has already reached equilibrium. Predict the effect that each of the following changes will have on the equilibrium position. Tell whether the equilibrium will shift to the right, will shift to the left, or will not be affected. a.
Consider the reaction: Fe3+(aq) + SCN2(aq) ⇌ FeSCN2+(aq) How will the equilibrium position shift if a. Water is added, doubling the volume? b. AgNO3(aq) is added? (AgSCN is insoluble.) c. NaOH(aq) is added? [Fe(OH)3 is insoluble.] d. Fe(NO3)3(aq) is added?
Chromium(VI) forms two different oxyanions, the orange dichromate ion (Cr2O7-2), and the yellow chromate ion (CrO4-2). (See the photos below.) The equilibrium reaction between the two ions is Cr2O7-2(aq) + H2O(l) ⇌ 2CrO4-2(aq) + 2H+(aq)
What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the reaction 2SO3(g) ⇌ 2SO2(g) + O2(g) in each of the following cases? a. Oxygen gas is added. b. The pressure is increased by decreasing the volume of the reaction container. c. In a rigid reaction container, the
An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) ⇌ H2(g) + CO2(g) How will this system at equilibrium shift in each of the five following cases? a. Gaseous carbon dioxide is removed. b. Water vapor is added. c. In a rigid reaction container, the pressure is
Hydrogen for use in ammonia production is produced by the reactionWhat will happen to a reaction mixture at equilibrium if a. H2O(g) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. CO(g) is removed? e. the volume
In which direction will the position of the equilibrium 2HI(g) ⇌ H2(g) + I2(g) be shifted for each of the following changes? a. H2(g) is added. b. I2(g) is removed. c. HI(g) is removed. d. In a rigid reaction container, some Ar(g) is added. e. The volume of the container is doubled. f. The
Predict the shift in the equilibrium position that will occur for each of the following reactions when the volume of the reaction container is increased. a. N2(g) + 3H2(g) ⇌ 2NH3(g) b. PCl5(g) ⇌ PCl3(g) + Cl2(g) c. H2(g) + F2(g) ⇌ 2HF(g) d. COCl2(g) ⇌ CO(g) + Cl2(g) e. CaCO3(s) ⇌ CaO(s) +
At 25° C, Kp < 1 × 10-31 for the reaction N2(g) + O2(g) ⇌ 2NO(g) a. Calculate the concentration of NO (in molecules/ cm3) that can exist in equilibrium in air at 25oC. In air PN2 = 0.8 atm and PO2 = 0.2 atm. b. Typical concentrations of NO in relatively pristine environments range from 108
Given the following equilibrium constants at 427oC, Na2O(s) ⇌ 2Na(l) + 12 O2(g) K1 = 2 × 10-25 NaO(g) ⇌ Na(l) + l2 O2(g) K2 = 2 × 10-5 Na2O2(s) ⇌ 2Na(l) + O2(g) K3 = 5 × 10-29 NaO2(s) ⇌ Na(l) + O2(g) K4 = 3 × 10-14 determine the values for the equilibrium constants for the following
Calculate a value for the equilibrium constant for the reaction O2(g) + O(g) ⇌ O3(g) given that NO2(g) ⇌ NO(g) + O(g) K = 6.8 × 10-49 O3(g) + NO(g) ⇌ NO2(g) + O2(g) K = 5.8 × 10-34
Given K = 3.50 at 458C for the reaction A(g) + B(g) ⇌ C(g) and K = 7.10 at 458C for the reaction 2A(g) + D(g) ⇌ C(g) what is the value of K at the same temperature for the reaction C(g) + D(g) ⇌ 2B(g) What is the value of Kp at 458C for the reaction? Starting with 1.50 atm partial pressures
An initial mixture of nitrogen gas and hydrogen gas is reacted in a rigid container at a certain temperature as follows: 3H2(g) + N2(g) ⇌ 2NH3(g) At equilibrium, the concentrations are [H2] = 5.0 M, [N2] = 8.0 M, and [NH3] = 4.0 M. What were the concentrations of nitrogen gas and hydrogen gas
At 25oC, Kp = 5.3 × 105 for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) When a certain partial pressure of NH3(g) is put into an otherwise empty rigid vessel at 25oC, equilibrium is reached when 50.0% of the original ammonia has decomposed. What was the original partial pressure of ammonia before any
A 2.4156-g sample of PCl5 was placed in an empty 2.000- L flask and allowed to decompose to PCl3 and Cl2 at 250.0oC: PCl5(g) ⇌ PCl3(g) + Cl2(g) At equilibrium the total pressure inside the flask was ob-served to be 358.7 torr. a. Calculate the partial pressure of each gas at equilibrium and the
At 25oC, gaseous SO2Cl2 decomposes to SO2(g) and Cl2(g) to the extent that 12.5% of the original SO2Cl2 (by moles) has decomposed to reach equilibrium. The total pressure (at equilibrium) is 0.900 atm. Calculate the value of Kp for this system
The partial pressures of an equilibrium mixture of N2O4(g) and NO2(g) are PN2O4 = 0.34 atm and PNO2 = 1.20 atm at a certain temperature. The volume of the container is doubled. Calculate the partial pressures of the two gases when a new equilibrium is established.
For the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) at 600. K, the equilibrium constant is 11.5. Suppose that 2.450 g of PCl5 is placed in an evacuated 500 mL bulb, which is then heated to 600. K. a. What would the pressure of PCl5 be if it did not dissociate? b. What is the partial pressure of PCl5 at
At 1258C, Kp = 0.25 for the reaction 2NaHCO3(s) ⇌ Na2CO3(s) + CO2(g) + H2O(g) A 1.00- L flask containing 10.0 g of NaHCO3 is evacuated and heated to 125oC. a. Calculate the partial pressures of CO2 and H2O after equilibrium is established. b. Calculate the masses of NaHCO3 and Na2CO3 present at
The gas arsine (AsH3) decomposes as follows: 2AsH3(g) ⇌ 2As(s) + 3H2(g) In an experiment pure AsH3(g) was placed in an empty, rigid, sealed flask at a pressure of 392.0 torr. After 48 h the pressure in the flask was observed to be constant at 488.0 torr. a. Calculate the equilibrium pressure of
For the reaction NH3(g) + H2S(g) ⇌ NH4HS(s) K = 400. at 35.0oC. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00- L vessel, what mass of NH4HS will be present at equilibrium? What is the pres-sure of H2S at equilibrium?
The hydrocarbon naphthalene was frequently used in mothballs until recently, when it was discovered that human inhalation of naphthalene vapors can lead to hemolytic anemia. Naphthalene is 93.71% carbon by mass, and a 0.256-mole sample of naphthalene has a mass of 32.8 g. What is the molecular
Consider the decomposition of the compound C5H6O3 as follows: C5H6O3(g) → C2H6(g) + 3CO(g) When a 5.63-g sample of pure C5H6O3(g) was sealed in an otherwise empty 2.50- L flask and heated to 200oC, the pressure in the flask gradually rose to 1.63 atm and remained at that value. Calculate K for
A sample of N2O4(g) is placed in an empty cylinder at 25oC. After equilibrium is reached, the total pressure is 1.5 atm, and 16% (by moles) of the original N2O4(g) has dissociated to NO2(g). a. Calculate the value of Kp for this dissociation reaction at 258C. b. If the volume of the cylinder is
Nitric oxide and bromine at initial partial pressures of 98.4 torr and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g) + Br2(g) ⇌ 2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g) ⇌ 4NO2(g) + O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0, will the mole percent of N2O5
Consider the reaction P4(g) → 2P2(g) where Kp = 1.00 × 10-1 at 1325 K. In an experiment where P4(g) was placed in a container at 1325 K, the equilibrium mixture of P4(g) and P2(g) has a total pressure of 1.00 atm. Calculate the equilibrium pressures of P4(g) and P2(g). Calculate the fraction (by
Suppose 1.50 atm of CH4(g), 2.50 atm of C2H6(g), and 15.00 atm of O2(g) are placed in a flask at a given temperature. The reactions are CH4(g) + 2O2(g) ⇌ CO2(g) + 2H2O(g) Kp = 1.0 × 104 2C2H6(g) + 7O2(g) ⇌ 4CO2(g) + 6H2O(g) Kp = 1.0 × 108 Calculate the equilibrium pressures of all gases.
Consider the reaction 3O2(g) ⇌ 2O3(g) At 1758C and a pressure of 128 torr, an equilibrium mixture of O2 and O3 has a density of 0.168 g/ L. Calculate Kp for the above reaction at 1758C.
A mixture of N2, H2 and NH3 is at equilibrium according to the equation N2(g) + 3H2(g) ‡Œ 2NH3(g) as depicted below.The volume is suddenly decreased (by increasing the external pressure), and a new equilibrium is established as depicted below. a. If the volume of the final equilibrium
A 4.72- g sample of methanol (CH3OH) was placed in an otherwise empty 1.00- L flask and heated to 250oC to vaporize the methanol. Over time the methanol vapor decomposed by the following reaction: CH3OH(g) ⇌ CO(g) + 2H2(g) After the system has reached equilibrium, a tiny hole is drilled in the
The compound SbCl5(g) decomposes at high temperatures to gaseous antimony trichloride and chlorine gas. When 89.7 g of SbCl5(g) is placed in a 15.0-L container at 1808C, the SbCl5(g) is 29.2% decomposed (by moles) after the system has reached equilibrium. a. Calculate the value of K for this
At 207oC, Kp = 0.267 for the reaction PCl5(g) ⇌ PCl3(g) + Cl2(g) a. If 0.100 mole of PCl5(g) is placed in an otherwise empty 12.0-L vessel at 207oC, calculate the partial pressures of PCl5(g), PCl3(g), and Cl2(g) at equilibrium. b. In another experiment the total pressure of an equilibrium
A 1.604-g sample of methane (CH4) gas and 6.400 g of oxygen gas are sealed in a 2.50- L vessel at 411oC and are allowed to reach equilibrium. Methane can react with oxygen to form gaseous carbon dioxide and water vapor, or methane can react with oxygen to form gaseous carbon monoxide and water
At 1000 K the N2(g) and O2(g) in air (78% N2, 21% O2, by moles) react to form a mixture of NO(g) and NO2(g). The values of the equilibrium constants are 1.5 × 10-4 and 1.0 × 10-5 for the formation of NO(g) and NO2(g), respectively. At what total pressure will the partial pressures of NO(g) and
The equilibrium constant Kp for the reaction CCl4(g) ⇌ C(s) + 2Cl2(g) at 700oC is 0.76. Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700oC.
An 8.00-g sample of SO3 was placed in an evacuated container, where it decomposed at 600.oC according to the following reaction: SO3(g) ⇌ SO2(g) ⇌ ½O2(g) At equilibrium the total pressure and the density of the gaseous mixture were 1.80 atm and 1.60 g/ L, respectively. Calculate Kp for this
A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred: 2FeSO4(s) ⇌ Fe2O3(s) + SO3(g) + SO2(g) SO3(g) ⇌ SO2(g) + ½O2(g) After equilibrium was reached, the total pressure was 0.836 atm, and the partial pressure of oxygen was 0.0275
At 450oC, Kp = 6.5 × 10-3 for the ammonia synthesis reaction. Assume that a reaction vessel with a movable piston initially contains 3.0 moles of H2(g) and 1.0 mole of N2(g). Make a plot to show how the partial pressure of NH3(g) present at equilibrium varies for the total pressures of 1.0 atm,
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container fitted with a frictionless, massless piston, where it decomposed at 25oC according to the following equation: 2NOBr(g) ⇌ 2NO(g) + Br2(g) The initial density of the system was recorded as 4.495 g/ L. After equilibrium was
A gaseous material XY(g) dissociates to some extent to produce X(g) and Y(g): XY(g) ⇌ X(g) + Y(g) A 2.00- g sample of XY (molar mass = 165 g/ mol) is placed in a container with a movable piston at 25oC. The pressure is held constant at 0.967 atm. As XY begins to dissociate, the piston moves until
Consider the reactionA(g) + B(g) ‡Œ C(g) for which K = 1.30 Ã— 102.Assume that 0.406 mole of C(g) is placed in the cylinder represented here. The temperature is 300.0 K, and the barometric pressure on the piston (which is assumed to be massless and frictionless) is constant at
Consider the accompanying diagram. Ball A is allowed to fall and strike ball B. Assume that all of ball A€™s energy is transferred to ball B at point I and that there is no loss of energy to other sources. Calculate the kinetic energy and the potential energy of ball B at point II. For a
As a system increases in volume, it absorbs 52.5 J of energy in the form of heat from the surroundings. The piston is working against a pressure of 0.500 atm. The final volume of the system is 58.0 L. What was the initial vol-ume of the system if the internal energy of the system Decreased by 102.5
What is the difference between ΔH and ΔE at constant P?
Are the following processes exothermic or endothermic? a. the combustion of gasoline in a car engine b. water condensing on a cold pipe c. CO2(s) → CO2(g) d. F2(g) → 2F(g)
Consider the following reaction: 2H2(g) + O2(g) → 2H2O(l) ΔH = –572 kJ a. How much heat is evolved for the production of 1.00 mole H2O(l)? b. How much heat is evolved when 4.03 g hydrogen is reacted with excess oxygen? c. How much heat is evolved when 186 g oxygen is reacted with excess
The overall reaction in a commercial heat pack can be represented as 4Fe(s) + 3O2(g) → 2Fe2O3(s) ΔH = –1652 kJ a. How much heat is released when 4.00 moles of iron is reacted with excess O2? b. How much heat is released when 1.00 mole of Fe2O3 is produced? c. How much heat is released when
Consider the combustion of propane: C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l) ΔH = –2221 kJ Assume that all the heat in Example 9.1 comes from the combustion of propane. What mass of propane must be burned to furnish this amount of energy, assuming the heat transfer process is 60.% efficient?
For the following reactions at constant pressure, predict if ΔH . ΔE, ΔH , ΔE, or ΔH = ΔE. a. 2HF(g) → H2(g) + F2(g) b. N2(g) + 3H2(g) → 2NH3(g) c. 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)
Calculate the energy required to heat 1.00 kg of ethane gas (C2H6) from 25.0oC to 75.0oC first under conditions of constant volume and then at a constant pressure of 2.00 atm. Calculate Î”E, Î”H, and w for these processes also.Table
Calculate q, w, Î”E, and Î”H for the process in which 88.0 g of nitrous oxide gas (N2O) is cooled from 165oC to 55oC at a constant pressure of 5.00 atm. Table
Consider a sample containing 5.00 moles of a mona-tomic ideal gas that is taken from state A to state B by the following two pathways:For each step, assume that the external pressure is constant and equals the final pressure of the gas for that step. Calculate q, w, Î”E, and
Consider the following potential energy diagrams for two different reactions.Which plot represents an exothermic reaction? In plot a, do the reactants on average have stronger or weaker bonds than the products? In plot b, reactants must gain potential energy to convert to products. How does this
Consider a sample containing 2.00 moles of a monatomic ideal gas that undergoes the following changes:For each step, assume that the external pressure is constant and equals the final pressure of the gas for that step. Calculate q, w, Î”E, and Î”H for each step and for the
Explain how calorimetry works to calculate ΔH or ΔE for a reaction. Does the temperature of the calorimeter increase or Decrease for an endothermic reaction? How about for an exothermic reaction? Explain why ΔH is obtained directly from a coffee cup calorimeter, whereas ΔE is obtained directly
The specific heat capacity of silver is 0.24 JoC-1g-1. a. Calculate the energy required to raise the temperature of 150.0 g Ag from 273 K to 298 K. b. Calculate the energy required to raise the temperature of 1.0 mole of Ag by 1.0oC (called the molar heat capacity of silver). c. It takes 1.25 kJ of
Consider the substances in Table 9.3. Which substance requires the largest amount of energy to raise the temperature of 25.0 g of the substance from 15.0oC to 37.0oC? Calculate the energy. Which substance in Table has the largest temperature change when 550 g of the substance absorbs 10.7 kJ of
A 150.0-g sample of a metal at 75.0oC is added to 150.0 g of H2O at 15.0oC. The temperature of the water rises to 18.3oC. Calculate the specific heat capacity of the metal, assuming that all the heat lost by the metal is gained by the water.
A biology experiment requires the preparation of a water bath at 37.0oC (body temperature). The temperature of the cold tap water is 22.0oC, and the temperature of the hot tap water is 55.0oC. If a student starts with 90.0 g of cold water, what mass of hot water must be added to reach 37.0oC?
A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 JoC-1g-1) and a 10.00-g sample of iron pellets (specific heat capacity = 0.45 JoC-1g-1) are heated to 100.0oC. The mixture of hot iron and aluminum is then dropped into 97.3 g of water at 22.0oC. Calculate the final temperature of
A sample of nickel is heated to 99.8oC and placed in a coffee cup calorimeter containing 150.0 g water at 23.5oC. After the metal cools, the final temperature of metal and water mixture is 25.0oC. If the specific heat capacity of nickel is 0.444 J/oC g, what mass of nickel was originally heated?
Hydrogen gives off 120 J/ g of energy when burned in oxygen, and methane gives off 50 J/ g under the same circumstances. If a mixture of 5.0 g hydrogen and 10. g methane is burned, and the heat released is transferred to 50.0 g water at 25.0oC, what final temperature will be reached by the water?
In a coffee cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed. The following reaction occurs: Ag+(aq) + Cl2(aq) → AgCl(s)
Consider an airplane trip from Chicago, Illinois, to denver, Colorado. List some path-Dependent functions and some state functions for the plane trip.
Consider the reaction 2HCl(aq) + Ba(OH)2(aq) → BaCl2(aq) + 2H2O(l) ΔH = –118 kJ
The heat capacity of a bomb calorimeter was determined by burning 6.79 g of methane (energy of combustion = –802 kJ/ mol CH4) in the bomb. The temperature changed by 10.8oC. a. What is the heat capacity of the bomb? b. A 12.6-g sample of acetylene (C2H2) produced a temperature increase of 16.9oC
The combustion of 0.1584 g benzoic acid increases the temperature of a bomb calorimeter by 2.54oC. Calculate the heat capacity of this calorimeter. (The energy re-leased by combustion of benzoic acid is 26.42 kJ/ g.) A 0.2130- g sample of vanillin (C8H8O3) is then burned in the same calorimeter,
Combustion of table sugar produces CO2(g) and H2O(l). When 1.46 g of table sugar is combusted in a constant-volume (bomb) calorimeter, 24.00 kJ of heat is liberated. a. Assuming that table sugar is pure sucrose [C12H22O11(s)], write the balanced equation for the combustion reaction. b. Calculate
Calculate w and ΔE when 1 mole of a liquid is vaporized at its boiling point (80oC) and 1.00 atm pressure. ΔHvap for the liquid is 30.7 kJ mol21 at 80.oC.
Given the following data:Calculate Î”H for the reaction On the basis of enthalpy change, is this a useful reaction for the synthesis of ammonia?
Consider 2.00 moles of an ideal gas that is taken from state A (PA = 2.00 atm, VA = 10.0 L) to state B (PB = 1.00 atm, VB = 30.0 L) by two different pathways.These pathways are summarized in the following graph of P versus V: Calculate the work (in units of J) associated with the two pathways. Is
Calculate ΔH for the reaction N2H4(l) + O2(g) → N2(g) + 2H2O(l) given the following data: 2NH3(g) + 3N2O(g) → 4N2(g) + 3H2O(l) ΔH = –1010.kJ N2O(g) + 3H2(g) → N2H4(l) + H2O(l) ΔH = –317 kJ 2NH3(g) + ½O2(g) → N2H4(l) + H2O(l) ΔH = 2143 kJ H2(g) + ½O2(g) → H2O(l) ΔH = –286 kJ
Given the following data: C2H2(g) + 5/2 O2(g) → 2CO2(g) + H2O(l) ΔH = –1300. kJ C(s) + O2(g) → CO2(g) ΔH = –394 kJ H2(g) + ½ O2(g) → H2O(l) ΔH = -286 kJ calculate ΔH for the reaction 2C(s) + H2(g) → C2H2(g)

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