Q&A Hero

Q: When a particular metal is illuminated with photons, one electron is observed for each absorbed photon. What effect would decreasing the wavelength and number of photons have on the electrons leaving the surface?A) There would be more electrons leaving the surface.B) They would have higher kinetic energy.C) The electron velocity would be lower.D) The kinetic energy of the electrons would be lower.E) Two photons might be required to eject the electrons.

Q: Based on the photoelectric effect, Einstein proposed the idea that A) the energy of a single particle or photon of light is inversely proportional to its frequency. B) the wavelength of light is inversely proportional to its frequency. C) particles can show characteristics of waves under certain experimental conditions. D) the energy of an object is proportional to its mass. E) light has particle-like properties.

Q: A photon of red light has a ____ frequency and a ____ wavelength than a photon of blue light. A) lower, longer B) higher, shorter C) lower, shorter D) higher, longer E) lower, lower

Q: Rank the following regions of the electromagnetic spectrum in order of decreasing frequency. X rays, Microwaves, Infrared, Ultraviolet A) infrared, microwaves, ultraviolet, x rays B) x rays, microwaves, infrared, ultraviolet C) microwaves, infrared, ultraviolet, x rays D) microwaves, ultraviolet, infrared, x rays E) x rays, ultraviolet, infrared, microwaves

Q: Which type of electromagnetic radiation has the highest frequency? A) microwaves B) visible C) radio waves D) infrared E) ultraviolet

Q: Which type of electromagnetic radiation has the shortest wavelength? A) red light B) x rays C) microwaves D) gamma rays E) blue light

Q: Which of the following statements is incorrect? A) As the energy of a photon increases, its frequency decreases. B) As the wavelength of a photon increases, its energy decreases. C) The product of wavelength and frequency of electromagnetic radiation is a constant. D) As the wavelength of a photon increases, its frequency decreases. E) As the frequency of a photon increases, its wavelength decreases.

Q: What is the frequency of a photon having a wavelength of 954.9nm? (, )A) 3.14 x10-4 HzB) 1.44 x1027 HzC) 3.14 x1014 HzD) 2.08 x10-37 HzE) 2.08 x10-19 Hz

Q: What is the wavelength of a photon having a frequency of Hz? (, )A) 667 nmB) nmC) nmD) 0.0895nmE) nm

Q: Which of the following is/are true about electromagnetic radiation? 1) Wavelength is inversely proportional to frequency. 2) Frequency has units of s-1or Hz. 3) Waves of different wavelengths travel at different speeds in a vacuum. A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1, 2, and 3

Q: What is the wavelength of a photon having a frequency of 64.6THz? (1THz=1015Hz, c=3.00 x 108m/s, h=6.63x10-34J·s)A) 0.215nmB) 4.28 x10-23 nmC) 1.28 x10-14 nmD) 4.64nmE) 4.64 x1015 nm

Q: A 2.19-g sample of solid calcium reacted in excess fluorine gas to give a 4.27-g sample of pure solid CaF2. The heat given off in this reaction was 67.0kJ at constant pressure. Given this information, what is the enthalpy of formation of CaF2(s)?A) 67.0 kJ/molB) -67.0 kJ/molC) -1.23 x103kJ/molD) -613 kJ/molE) 1.23 x103kJ/mol

Q: A 5.09-g sample of solid silver reacted in excess chlorine gas to give a 6.76-g sample of pure solid AgCl. The heat given off in this reaction was 6.00kJ at constant pressure. Given this information, what is the enthalpy of formation of AgCl(s)?A) -127 kJ/molB) -63.6 kJ/molC) 127 kJ/molD) -6.00 kJ/molE) 6.00 kJ/mol

Q: A 9.020-g sample of an unknown metal M is burned in the presence of excess oxygen, producing the oxide M2O3(s) and liberating 191.5kJ of heat at constant pressure. What is the identity of the metal?4M(s)+3O2(g)→2M2O3(s) Substance Hf(kJ/mol) Yb2O3(s) -1814.6 Tb2O3(s) -1865.2 Sm2O3(s) -1823.0 Sc2O3(s) -1908.8 Y2O3(s) -1905.3 A) SmB) ScC) YbD) YE) Tb

Q: When 49.4mL of 0.721M lead(II) nitrate reacts with 99.6mL of 0.807M sodium chloride, 0.830kJ of heat is released at constant pressure. What isHº for this reaction?Pb(NO3)2(aq)+2NaCl(aq)→PbCl2(s)+2NaNO3(aq)A) -23.3 kJB) -10.3 kJC) -4.23 kJD) -7.15 kJE) -20.6 kJ

Q: When 32.4mL of liquid benzene (C6H6, d=0.879g/mL) reacts with 81.6L of oxygen gas, measured at 1.00atm pressure and 25ºC, 1.19 x 103kJ of heat is released at constant pressure. What is Hº for the following reaction? (R=0.0821L.atm/(K.mol))2C6H6(l)+15O2(g)→12CO2(g)+6H2O(l)A) -2.35 x 101kJB) -3.22 x 102kJC) -5.36 x 103kJD) -3.27 x 103kJE) -6.53 x 103kJ

Q: How much heat is liberated at constant pressure when 58.5g of calcium oxide reacts with 83.9L of carbon dioxide gas, measured at 1.00atm pressure and 25.0ºC? (R=0.0821L.atm/(K.mol))CaO(s)+CO2(g)→CaCO3(s); Hº=-178.3kJA) -6.11 x 102kJB) -1.04 x 104kJC) -7.97 x 102kJD) -1.86 x 102kJE) -1.50 x 104kJ

Q: How much heat is released at constant pressure if 16.9mL of 0.694M silver nitrate is mixed with 79.7mL of 0.372M potassium chloride?AgNO3(aq)+KCl(aq)→AgCl(s)+KNO3(aq); Hº=-65.5kJA) -0.768 kJB) -24.4 kJC) -1.94 kJD) -45.5 kJE) -2.71 kJ

Q: The reaction of iron with hydrochloric acid is represented by the following thermochemical equation.Fe(s) + 2HCl(aq) →FeCl2(aq) + H2(g); Hº= -87.9 kJIn which of the following experiments would the temperature rise the most?A) 2.2 g of Fe added to 1.0 L of 0.03 MHClB) 1.1 g of Fe added to 1.0 L of 0.02 MHClC) 4.5 g of Fe added to 1.0 L of 0.03 MHClD) 1.1 g of Fe added to 1.0 L of 0.04 MHClE) 0.56 g of Fe added to 1.0 L of 0.02 MHCl

Q: The reaction of iron with hydrochloric acid is represented by the following thermochemical equation.Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g); Hº=-87.9kJIf, in a particular experiment, 7.36kJ of heat was released at constant pressure, what volume of H2(g), measured at STP, was produced? (R=0.0821L atm/(K mol))A) 2.92 x 102LB) 2.05 LC) 22.4 LD) 2.68 x 102LE) 1.88 L

Q: At constant pressure and 25ºC, what is Hº for the following reaction2C2H6(g)+7O2(g)→4CO2(g)+H2O(l)if the complete consumption of 11.3 g of C2H6liberates "586.3 kJ of heat energy?A) -3120 kJB) -1560 kJC) -441 kJD) -222 kJE) -786 kJ

Q: The reaction of iron with hydrochloric acid is represented by the following thermochemical equation.Fe(s)+2HCl(aq)→FeCl2(aq)+H2(g); Hº=-87.9kJHow much heat is liberated at constant pressure if 0.358g of iron reacts with 34.1mL of 0.588MHCl?A) 4.09 kJB) 31.5 kJC) 0.563 kJD) 0.881 kJE) 87.9 kJ

Q: How much heat is evolved upon the complete oxidation of 9.118g of aluminum at 25ºC and 1 atm pressure? (for Al2O3is -1676 kJ/mol.)4Al(s)+3O2(g)→2Al2O3(s)A) 1.528 x 104kJB) 566.4 kJC) 1133 kJD) 283.2 kJE) 141.6 kJ

Q: When 34.1g of lead reacts with 6.81L of oxygen gas, measured at 1.00atm and 25.0ºC, 36.1kJ of heat is released at constant pressure. What is Hº for this reaction? (R=0.0821L-atm/(K mol))2Pb(s)+O2(g)→2PbO(s)A) -4.39 x 102kJB) -5.94 x 101kJC) -3.61 x 101kJD) -2.19 x 102kJE) -1.30 x 102kJ

Q: How much heat is liberated at constant pressure if 0.834g of calcium carbonate reacts with 48.9mL of 0.668M hydrochloric acid?CaCO3(s)+2HCl(aq)→CaCl2(aq)+H2O(l)+CO2(g); Hº=-15.2kJA) -0.127 kJB) -0.375 kJC) -12.7 kJD) -0.248 kJE) -10.2 kJ

Q: Consider the following thermochemical equation:N2(g) + 2O2(g) →2NO2(g); Hº= 66.2 kJFrom this equation, we may conclude that 66.2 kJ is the quantity of heat that isA) gained from the surroundings when 1 mol of NO2 is formed at constant pressure.B) lost to the surroundings when 1 mol of NO2 is formed at constant pressure.C) gained from the surroundings when 2 mol of NO2 is formed at constant pressure.D) lost to the surroundings when 2 mol of NO2 is formed at constant pressure.E) lost to the surroundings when 1 mol of O2 is consumed at constant pressure.

Q: According to the following thermochemical equation, if 951.1g of NO2 is produced, how much heat is released at constant pressure?2NO(g)+O2(g)→2NO2(g); Hº=-114.4kJA) 114.4 kJB) 1.183 x103kJC) 2.365 x103kJD) 5.534 kJE) 1.088 x105kJ

Q: What mass of hydrogen is consumed when 587.9kJ of energy is evolved from the combustion of a mixture of H2(g) and O2(g)?H2(g)+O2(g)→H2O(l); Hº=-285.8kJA) 4.147 gB) 2.073 gC) 0.2412 gD) 6.162 gE) 2.131 g

Q: What quantity, in moles, of hydrogen is consumed when 676.8kJ of energy is evolved from the combustion of a mixture of H2(g) and O2(g)?H2(g)+O2(g)→H2O(l); Hº=-285.8kJA) 2.368 molB) 1.184 molC) 0.4223 molD) 3.368 molE) 1.368 mol

Q: What is the quantity of heat evolved at constant pressure when 60.3g H2O(l) is formed from the combustion of H2(g) and O2(g)?H2(g)+O2(g)→H2O(l); Hº=-285.8kJA) 1.17 x10-2kJB) 285.8 kJC) 1.72 x104kJD) 85.4 kJE) 9.57 x102kJ

Q: What is the change in enthalpy at 25ºC and 1 atm for the reaction of 5.00mol of elemental iron with excess oxygen gas?4Fe(s)+3O2(g)→2Fe2O3(s); Hº=-1651kJA) -1651 kJB) 2752 kJC) 2064 kJD) -2064 kJE) -412.8 kJ

Q: What is the change in enthalpy at 25ºC and 1 atm for the production of 9.00mol SnO(s)?Sn(s)+SnO2(s)→2SnO(s); Hº=16.2kJA) -72.9 kJB) -16.2 kJC) 16.2 kJD) 1.80 kJE) 72.9 kJ

Q: What is the change in enthalpy when 4.00mol of sulfur trioxide decomposes to sulfur dioxide and oxygen gas?2SO2(g)+O2(g)→2SO3(g); Hº=198kJA) 396 kJB) -198 kJC) -396 kJD) 198 kJE) 792 kJ

Q: Which of the following statements is false concerning the reaction of hydrogen gas and oxygen gas given below?H2(g) + O2(g) → H2O(l); Hº= -285.8 kJA) Per mole of O2, the change in enthalpy is -571.6 kJ.B) The value -571.6 kJ pertains to 1 mol of liquid water.C) If the equation is reversed, Hº becomes +285.8 kJ.D) If the equation is multiplied by 2, Hº becomes -571.6 kJ.E) For the reaction H2(g) + O2(g) →H2O(g), Hº is not equal to -285.8 kJ.

Q: Given: what is Hº for the following thermochemical equation?A) 986.9 kJB) -986.9 kJC) -139 MJD) -2320 kJE) -38.7 kJ

Q: Given the thermochemical equation2Al(s) + O2(g) → Al2O3(s); Hº= -1676 kJfind Hº for the following reaction.2Al2O3(s) →4Al(s) + 3O2(g)A) 838 kJB) 1676 kJC) -1676 kJD) 3352 kJE) -838 kJ

Q: Given:4AlCl3(s) + 3O2(g) →2Al2O3(s) + 6Cl2(g); Hº= -529.0 kJdetermine Hº for the following thermochemical equation.Cl2(g) + Al2O3(s) → AlCl3(s) + O2(g)A) +264.5 kJB) +529.0 kJC) +88.2 kJD) +176.3 kJE) -176.3 kJ

Q: In a certain experiment, 0.1000mol of hydrogen gas reacted with 0.1000mol of solid iodine at a constant 1 atm pressure, producing 0.2000mol of solid hydrogen iodide and absorbing 5.272kJ of heat in the process. Which of the following thermochemical equations correctly describes this experiment?A) H2(g) + I2(s) →2HI(s); Hº= -52.72 kJB) H2(g) + I2(s) →2HI(s); Hº= 5.272 kJC) H2(g) + I2(s) →2HI(s); Hº= -5.272 kJD) H2(g) + I2(s) →2HI(s); Hº= 10.54 kJE) H2(g) + I2(s) →2HI(s); Hº= 52.72 kJ

Q: Which of the following statements is incorrect concerning the thermochemical equation below?2SO3(g) →2SO2(g) + O2(g); Hº= 198 kJA) The enthalpy of the reactants exceeds that of the products.B) The reaction is endothermic.C) For the reaction 2SO2(g) + O2(g) → 2SO3(g), Hº= -198 kJ.D) The external pressure is 1 atm.E) For every mole of SO3(g) consumed, 99 kJ of heat at constant pressure is consumed as well.

Q: Which of the following sentences accurately describes the thermochemical equation given below?2Ag(s) + F2(g) → 2AgF(s); Hº= -409.2 kJA) If 2 mol of silver metal react with 1 mol of fluorine gas at constant volume, 2 mol of solid sodium fluoride is produced and 409.2 kJ of heat is consumed.B) If 2 atoms of silver metal react with 1 molecule of fluorine gas at constant pressure, 2 formula units of solid sodium fluoride are produced and 409.2 kJ of heat is released.C) If 2 atoms of silver metal react with 1 molecule of fluorine gas at constant pressure, 2 formula units of solid sodium fluoride are produced and 409.2 kJ of heat is consumed.D) If 2 mol of silver metal react with 1 mol of fluorine gas at constant pressure, 2 mol of solid sodium fluoride is produced and 409.2 kJ of heat is consumed.E) If 2 mol of silver metal react with 1 mol of fluorine gas at constant pressure, 2 mol of solid sodium fluoride is produced and 409.2 kJ of heat is released.

Q: Under conditions of constant pressure, for which of the following reactions is the magnitude of pressure-volume work going to be smallest?A) BaO(s) + SO3(g) →BaSO4(s)B) 2NO(g) + O2(g) →2NO2(g)C) 2H2O2(l) →2H2O(l) + O2(g)D) 2KClO3(s) →2KCl(s) + 3O2(g)E) H2(g) + Cl2(g) →2HCl(g)

Q: Under conditions of constant pressure, for which of the following reactions is the magnitudeof pressure-volume work going to be greatest?A) BaO(s) + SO3(g) →BaSO4(s)B) 2NO(g) + O2(g) →2NO2(g)C) 2H2O2(l) →2H2O(l) + O2(g)D) 2KClO3(s) →2KCl(s) + 3O2(g)E) H2(g) + Cl2(g) →2HCl(g)

Q: Which of the following statements is true concerning the decomposition of liquid water to form hydrogen gas and oxygen gas?2H2O(l) → 2H2(g) + O2(g)A) H is greater than U because the pressure is constant.B) H is less than U because of the pressure-volume work done by the gaseous products.C) H is less than U because the atmosphere does pressure-volume work on the gaseous products.D) H equals U because both are state functions.E) H is greater than U because of the pressure-volume work done by the gaseous products.

Q: The phrase "the heat absorbed or released by a system undergoing a physical or chemical change at constant pressure" isA) the change in enthalpy of the system.B) the change in internal energy of the system.C) the definition of a state function.D) the temperature change of the system.E) a statement of Hess's law.

Q: Which of the following statements about enthalpy is false? A) Enthalpy is a state function. B) At constant pressure, the enthalpy change is equal to the heat absorbed or released. C) Enthalpy is an extensive property. D) The change in enthalpy of a process cannot be negative. E) The SI unit of enthalpy is J.

Q: Which of the following statements is incorrect? A) Internal energy is a state function. B) The value of qis positive when heat flows into a system from the surroundings. C) The value of qis positive in an endothermic process. D) Heat flows from a system into the surroundings in an endothermic process. E) Enthalpy is a state function.

Q: H2 and F2 react according to the following equation, forming HF.H2(g) + F2(g) → 2HF(g); Hº= -271 kJIf H2(g) and F2(g) were mixed in a thermally insulated vessel, the reaction that occurred would beA) endothermic, and the temperature of the reaction system would fall.B) We could not tell unless the original and final temperatures were given.C) exothermic, and the temperature of the reaction system would fall.D) exothermic, and the temperature of the reaction system would rise.E) endothermic, and the temperature of the reaction system would rise.

Q: Which of the following statements is not true for an exothermic reaction? A) The products have a higher heat content than the reactants. B) The temperature of the reaction system increases. C) The temperature of the surroundings increases. D) Heat passes from the reaction system to the surroundings. E) The enthalpy change for the reaction is negative.

Q: At constant pressure, the sign of qfor the process H2O(l) →H2O(s) is expected to beA) positive, and the process is exothermic.B) negative, and the process is endothermic.C) impossible to predict.D) negative, and the process is exothermic.E) positive, and the process is endothermic.

Q: At constant pressure, the sign of q for the process CO2(s) → CO2(g) is expected to beA) positive, and the process is exothermic.B) negative, and the process is exothermic.C) impossible to predict.D) positive, and the process is endothermic.E) negative, and the process is endothermic.

Q: What is the change in internal energy of the system (U) if 10 kJ of heat energy is absorbed by the system and 70 kJ of work is done by the system for a certain process?A) -60 kJB) 80 kJC) 10 kJD) 60 kJE) -80 kJ

Q: If q=28 kJ and w= 85 kJ for a certain process, that process A) requires a catalyst. B) is endothermic. C) occurs slowly. D) is exothermic. E) cannot occur.

Q: If q=-91 kJ for a certain process, that processA) requires a catalyst.B) is exothermic.C) occurs rapidly.D) is endothermic.E) cannot occur.

Q: Which of the following statements about heat is false? A) If heat flows into a system, the extra energy of the system appears in the form of internal energy. B) A hot object possesses more heat than a cold object. C) If the system and surroundings are in thermal equilibrium, there is no heat flow between them. D) A process in which heat flows out of a system is said to be exothermic. E) Heat is a form of energy flow.

Q: Which of the following does not result in a change in the internal energy of the system? A) work is done on the system B) work is done on the surroundings C) heat flows into the system D) heat flows to the surroundings E) none of the above

Q: Which of the following is an endothermic process? A) work is done by the system on the surroundings B) heat energy flows from the system to the surroundings C) work is done on the system by the surroundings D) heat energy is evolved by the system E) none of the above

Q: Calculate U of a gas for a process in which the gas absorbs 9J of heat and does 25J of work by expanding.A) 16 JB) 34 JC) -34 JD) 0, because U is a state functionE) -16 J

Q: What is the kinetic energy of a 2000-lb car traveling at 48miles per hour? (1lb=0.4536kg, 1mi=1.609 km)A) 2.1 x 10-7JB) 1.0 x 106JC) 3.5 x 1019JD) 2.1 x 105JE) 3.1 x 10-8J

Q: The internal energy of a substance is defined as A) the potential energy of all particles which make up the substance. B) the kinetic energy of all particles which make up the substance. C) the sum of the potential and kinetic energy of all particles which make up the substance. D) the thermal energy of all particles which make up the substance. E) the chemical energy of all particles which make up the substance.

Q: The air whipped up by a tornado possesses what type(s) of energy? A) potential energy only B) internal energy only C) kinetic energy only D) kinetic energy, potential energy, and internal energy E) kinetic energy and potential energy only

Q: The energy associated with the motion of a speeding bullet is called _____. A) heat B) internal energy C) temperature D) kinetic energy E) potential energy

Q: The energy associated with the separation of two electrical charges is called _____. A) heat B) internal energy C) temperature D) kinetic energy E) potential energy

Q: Which of the following is not a fuel-oxidizer mixture used in rockets?A) kerosene-oxygenB) hydrogen-oxygenC) octane-oxygenD) aluminum-ammonium perchlorateE) hydrazine-dinitrogen tetroxide

Q: Which of the following is/are correct about fossil fuels? 1) Anthracite coal is pure, amorphous carbon. 2) Purified natural gas is a mixture of primarily methane and small amounts of ethane, propane, and butane. 3) Gasoline obtained from petroleum primarily contains the hydrocarbon octane (C8H18). A) 1 only B) 2 only C) 3 only D) 1, 2 and 3 E) none

Q: Calculate the change in enthalpy when 52.0 g of solid chromium at 25ºC and 1 atm pressure is oxidized. (Hºf for Cr2O3(s) is -1135 kJ/mol.)4Cr(s) + 3O2(g) → 2Cr2O3(s)A) -1135 kJB) -284 kJC) -568 kJD) +1135 kJE) +568 kJ

Q: From the following information, determine the enthalpy of formation of C2H4(g).C2H4(g) → C(s) + H2(g); Hº= -26.2 kJA) -26.2 kJ/molB) 26.2 kJ/molC) 104.8 kJ/molD) -52.4 kJ/molE) 52.4 kJ/mol

Q: What is the standard enthalpy of formation of MgCO3(s)?MgO(s)+CO2(g)→MgCO3(s); Hº=-100.7kJ SubstanceHºf(kJ/mol)MgO(s)-601.6CO2(g)-393.5A) 107.4 kJB) -308.8 kJC) -894.4 kJD) -1095.8 kJE) 894.4 kJ

Q: The standard enthalpies of formation of various iodine species are as follows: SubstanceHºf(kJ/mol)I(g)+107I2(g)+21HI(g)+26What additional information is needed to calculate the standard enthalpy change of the following reaction?H2(g) + I2(g) → 2HI(g)A) none, because the answer is 2 times 26 kJ/molB) the enthalpy of formation of I-(g) and H+(g)C) the enthalpy of formation of solid iodineD) none, because the enthalpy of formation of I2(g) and HI(g) are given and the enthalpy of elemental hydrogen is zeroE) the enthalpy of formation of gaseous hydrogen

Q: What is the standard enthalpy of formation of liquid diethylamine, (CH3CH2)2NH?N2O5(g) + 8CH4(g) → 2(CH3CH2)2NH(l) + 5H2O(l); Hº= -1103 kJ SubstanceHºf(kJ/mol)N2O5(g)+11.3CH4(g)-74.9H2O(l)-285.8A) -131 kJ/molB) -421 kJ/molC) +131 kJ/molD) -1452 kJ/molE) +421 kJ/mol

Q: What is the standard enthalpy change for the following reaction?N2H4(l) + 2NO2(g) → 2N2O(g) + 2H2O(l) SubstanceHºf(kJ/mol)N2H4(l)+50.6NO2(g)+33.1N2O(g)+82.1H2O(l)-285.8A) -290.6 kJB) -524.2 kJC) -119.7 kJD) +290.6 kJE) +119.7 kJ

Q: What is the standard enthalpy change for the following reaction?3CH4(g) + 4O3(g) → 3CO2(g) + 6H2O(g) SubstanceHºf(kJ/mol)CH4(g)-74.87O3(g)+142.7CO2(g)-393.5H2O(g)-241.8A) -2285.1 kJB) -2977.5 kJC) +2977.5 kJD) +2285.1 kJE) -3426.5 kJ

Q: What is the standard enthalpy change for the combustion of liquid cyclopentane, C5H10?2C5H10(l) + 15O2(g) → 10CO2(g) + 10H2O(l) SubstanceHºf(kJ/mol)C5H10(l)-105.6CO2(g)-393.5H2O(l)-285.8A) +573.7 kJB) -573.7 kJC) +784.9 kJD) -784.9 kJE) -6581.8 kJ

Q: At 25ºC, the standard enthalpy of combustion of gaseous propane (C3H8) is -2219.0 kJ per mole of propane, and the standard enthalpy of combustion of gaseous propylene (C3H6) is -2058.3 kJ per mole of propylene. What is the standard enthalpy change for the following reaction at 25ºC? SubstanceHºf(kJ/mol)CO2(g)-393.5H2O(l)-285.8A) +104.7 kJB) -20.4 kJC) -125.1 kJD) +160.7 kJE) -160.7 kJ

Q: What is the standard enthalpy of formation of liquid n-butanol, CH3CH2CH2CH2OH?CH3CH2CH2CH2OH(l) + 6O2(g) →4CO2(g) + 5H2O(l); Hº= -2675 kJ SubstanceHºf(kJ/mol)CO2(g)-393.5H2O(l)-285.8A) -328 kJB) +3355 kJC) -1996 kJD) +328 kJE) -3355 kJ

Q: What is the standard enthalpy change for the combustion of gaseous propylene, C3H6?C3H6(g) + O2(g) →3CO2(g) + 3H2O(l)SubtanceHºf(kJ/mol)C3H6(g)+20.4CO2(g)-393.5H2O(l)-285.8A) +2017.5 kJB) -2058.3 kJC) -658.9 kJD) -2017.5 kJE) +2058.3 kJ

Q: What is Hº for the following reaction?2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) SubstanceHºf(kJ/mol)C2H2(g)+226.7CO2(g)-393.5H2O(l)-393.5A) +1692.2 kJB) -452.6 kJC) -1692.2 kJD) +2599.0 kJE) -2599.0 kJ

Q: What is the standard enthalpy of formation of liquid butyraldehyde, CH3CH2CH2CHO(l)?CH3CH2CH2CHO(l) + O2(g) →4H2O(l) + 4CO2(g); Hº= -2471.8 kJ SubstanceHºf(kJ/mol)CO2(g)-393.5H2O(l)-285.8A) -245.4 kJ/molB) +245.4 kJ/molC) -1792.5 kJ/molD) -3151.1 kJ/molE) +3151.1 kJ/mol

Q: At 25ºC, when 1.00 g of sulfur is burned at constant pressure in excess oxygen to give SO2(g), 9.28 kJ of heat is liberated. What is the enthalpy of formation of SO2(g)?A) 9.28 kJ/molB) -594 kJ/molC) 298 kJ/molD) -9.28 kJ/molE) -298 kJ/mol

Q: From the following information, determine Hºf of malonic acid, CH2(COOH)2(s).CH2(COOH)2(s) + 2O2(g) →3CO2(g) + 2H2O(l); Hº= -861.0 kJ SubstanceHºf(kJ/mol)CO2(g)-393.5H2O(l)-285.8A) 2613 kJB) 891.1 kJC) -1540.3 kJD) -2613.1 kJE) -891.1 kJ

Q: What is Hº of the following reaction?CO2(g) + 2CH4(g) →C3H8(g) + O2(g) SubstanceHºf(kJ/mol)CO2(g)-393.5CH4(g)-74.9C3H8(g)-104.7A) -348.4 kJB) -573.1 kJC) 438.6 kJD) 348.4 kJE) -648.0 kJ