08:42Thermochemical Equations and Using the energy term (heat of reaction) in mole-mass problem solvingCrash Chemistry Academy221
Multiple ChoiceNitromethane (CH3NO2), sometimes used as a fuel for drag racing, burns according to the following reaction: 4 CH3NO2 (l) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (g) + 4 NO2 (g) ∆Hº = – 2441.6 kJHow much heat is released by burning 125.0 g of nitromethane (MW:61.044 g/mol)? 124511Has a video solution.
Multiple ChoiceConsider the following reaction: 2 C6H6 (l) + 15 O2 (g) → 12 CO2 (g) + 6 H2O (g) ∆Hº = – 6278 kJWhat volume of benzene (C6H6, d = 0.880 g/mL, molar mass = 78.11 g/mol) is necessary to evolve 5.19 x 109 kJ of heat? 4512Has a video solution.
Multiple ChoiceThe creation of liquid methanol is accomplished by the hydrogenation of carbon monoxide: CO (g) + 2 H2 (g) → CH3OH (l) ∆Hº = – 128.1 kJHow much heat (in kJ) is released when 125.0 g CO reacts with 2.32 x 102 g H2?108921Has a video solution.
Multiple ChoiceConsider two identical iron nails: One nail is heated to 95℃, the other is cooled to 15℃. The two nails are placed in a coffee cup calorimeter and the system is allowed to come to thermal equilibrium. What is the final temperature of the two nails?105
Textbook QuestionIsooctane is the primary component of gasoline and burns in air to produce water rand carbon dioxide 2 C8H18(g) + 25 O2(g) → 16 CO2(g) + 18 H2O(l) ΔH°= —10,940 kJ How much energy is released if 100.0 mL of isooctane (density = 0.690 g/mL) are burned (a) 3300 kJ (b) 6620 kJ (c) 6950 kJ (d) 3.02 kJ820Has a video solution.
Textbook QuestionConsider the following reaction: 2 CH3OH1g2¡ 2 CH41g2 + O21g2 H = +252.8 kJ (d) How many kilojoules of heat are released when 38.5 g of CH41g2 reacts completely with O21g2 to form CH3OH1g2 at constant pressure?236Has a video solution.
Textbook QuestionConsider the following reaction: 2 CH3OH1g2¡ 2 CH41g2 + O21g2 H = +252.8 kJ (b) Calculate the amount of heat transferred when 24.0 g of CH3OH1g2 is decomposed by this reaction at constant pressure.4531Has a video solution.
Textbook QuestionWhen solutions containing silver ions and chloride ions are mixed, silver chloride precipitates Ag+1aq2 + Cl-1aq2 ¡ AgCl1s2 H = -65.5 kJ (a) Calculate H for the production of 0.450 mol of AgCl by this reaction. (b) Calculate H for the production of 9.00 g of AgCl. (c) Calculate H when 9.25 * 10-4 mol of AgCl dissolves in water.430Has a video solution.
Textbook QuestionAt one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO3: 2 KClO31s2¡2 KCl1s2 + 3 O21g2 H = -89.4 kJ For this reaction, calculate H for the formation of (b) 10.4 g of KCl.183Has a video solution.
Textbook QuestionAt one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO3: 2 KClO31s2¡2 KCl1s2 + 3 O21g2 H = -89.4 kJ For this reaction, calculate H for the formation of (a) 1.36 mol of O2202Has a video solution.
Textbook QuestionConsider the decomposition of liquid benzene, C6H61l2, to gaseous acetylene, C2H21g2: C6H61l2 ¡ 3 C2H21g2 H = +630 kJ (b) What is H for the formation of 1 mol of acetylene?178Has a video solution.
Textbook QuestionWhat mass of natural gas (CH4) must burn to emit 267 kJ of heat? CH4( g) + 2 O2( g)¡CO2( g) + 2 H2O( g) ΔH °rxn = -802.3 kJ24692Has a video solution.
Textbook QuestionNitromethane (CH3NO2) burns in air to produce significant amounts of heat. 2 CH3NO2(l ) + 32 O2( g)¡2 CO2( g) + 3 H2O(l ) + N2( g) ΔH °rxn = -1418 kJ How much heat is produced by the complete reaction of 5.56 kg of nitromethane?1677Has a video solution.
Textbook QuestionTitanium reacts with iodine to form titanium(III) iodide, emitting heat. 2 Ti(s) + 3 I2( g)¡2 TiI3(s) ΔH °rxn = -839 kJ Determine the mass of titanium that react if 1.55 * 103 kJ of heat is emitted by the reaction.991Has a video solution.
Textbook QuestionThe propane fuel (C3H8) used in gas barbeques burns according to the thermochemical equation: C3H8( g) + 5 O2( g)¡3 CO2( g) + 4 H2O( g) ΔH °rxn = -2044 kJ If a pork roast must absorb 1.6 * 103 kJ to fully cook, and if only 10% of the heat produced by the barbeque is actually absorbed by the roast, what mass of CO2 is emitted into the atmosphere during the grilling of the pork roast?2928Has a video solution.
Textbook QuestionCharcoal is primarily carbon. Determine the mass of CO2 produced by burning enough carbon (in the form of charcoal) to produce 5.00 * 102 kJ of heat. C(s) + O2( g)¡CO2( g) ΔH °rxn = -393.5 kJ2169Has a video solution.
Textbook QuestionThe familiar "ether" used as an anesthetic agent is diethly ether, C4H10O. Its heat of vaporization is +26.5 kJ/mol at Calorimetry and Heat Capacity (Section 9.7) 9.76 What is the difference between heat capacity and specific heat? 9.77 Does a measurement carried out in a bomb calorimeter give its boiling point. How much energy in kilojoules is required to convert 100 mL of diethyl ether at its boiling point from liquid to vapor if its density is 0.7138 g/mL?205Has a video solution.
Textbook QuestionHow much energy in kilojoules is required to convert 100 mL of water at its boiling point from liquid to vapor, and how does this compare with the result calculated in Problem 9.68 for diethyl ehter? [ΔHvap(H2O) = + 40.7 kJ/mol]355Has a video solution.
Textbook QuestionAluminum metal reacts wiht chlorine with a spectacular display of sparks: 2 Al(s) + 3 Cl2(g) → 2 AlCl3(s) ΔH° = -1408.4 kJ How much heat in kilojoules is released on reaction of 5.00 g of Al?353Has a video solution.
Textbook QuestionHow much heat in kilojoules is evolved or absorbed in the reaction of 1.00 g of Na with H2O? Is the reaction exother- mic or endothermic? 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g) ΔH° = -368.4 kJ494Has a video solution.
Textbook QuestionHow much heat in kilojoules is evolved or absorbed in each of the following reactions?(b) Reaciton of 4.88 g of barium hydroxid eoctahydrate with ammonium chloride: Ba(OH)2·8 H2O (s) + 2 NH4Cl (s) → BaCl2(aq) + 2 NH3(aq) + 10 H2O(l) ΔH° = +80.3 kJ206Has a video solution.
Textbook QuestionHow much heat in kilojoules is evolved or absorbed in each of the following reactions? (a) Burning of 15.5 g of propane: C3H8 (g) + 5 O2(g) → 3 CO2(g) + 4 H2O (l) ΔH°=-2220 kJ454Has a video solution.
Textbook QuestionThe combustion of one mole of liquid octane, CH3(CH2)6CH3, produces 5470 kJ of heat. Calculate how much heat is produced if 1.000 gallon of octane is combusted. See Exercise 3.68 for necessary information about octane.1745Has a video solution.
Textbook QuestionNitromethane (CH3NO2), sometimes used as a fuel in drag racers, burns according to the following equation. How much heat is released by burning 100.0 g of nitromethane? 4 CH3NO2(l) + 7 O2(g) → 4 CO2(g) + 6 H2O(g) + 4 NO2(g) ΔH° = -2441.6 kJ542Has a video solution.
Textbook QuestionHow much heat in kilojoules is evolved or absorbed in the reaction of 2.50 g Fe2O3 with enough carbon monoxide to produce iron metal? Is the process exothermic or endothermic? Fe2O3(s) + 3 CO2(g) → 2 Fe(s) + 3 CO2(g) ΔH° = -24.8 kJ441Has a video solution.
Textbook QuestionHow much heat in kilojoules is evolved or absorbed in the reaction of 233.0 g of calcium oxide with enough carbon to produce calcium carbide? Is the process exothermic or endothermic? CaO(s) + 3 C(s) → CaC2(s) + CO(g) ΔH° = 464.6 kJ728Has a video solution.
Textbook QuestionMethanol 1CH3OH2 is used as a fuel in race cars. (d) Calculate the mass of CO2 produced per kJ of heat emitted.219Has a video solution.
Textbook QuestionMethanol 1CH3OH2 is used as a fuel in race cars. (c) Calculate the heat produced by combustion per liter of methanol. Methanol has a density of 0.791 g>mL.486Has a video solution.
Textbook QuestionAssume that 100.0 mL of 0.200 M CsOH and 50.0 mL of 0.400 M HCl are mixed in a calorimeter. The solutions start out at 22.50 °C, and the final temperature after reaction is 24.28 °C. The densities of the solutions are all 1.00 g/mL, and the specific heat of the mixture is 4.2 J/(g•°C). What is the enthalpy change for the neutralization reaction of 1.00 mol of CsOH in kJ?246Has a video solution.
Textbook QuestionDetermine the mass of CO2 produced by burning enough of each fuel to produce 1.00 * 102 kJ of heat. a. CH4( g) + 2 O2( g)¡CO2( g) + 2 H2O( g) ΔH °rxn = -802.3 kJ2279Has a video solution.
Textbook QuestionLiquid butane (C4H10) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as -0.5 °C. (c) How much heat must be added to vaporize 250 g of butane if its heat of vaporization is 21.3 kJ/mol? What volume does this much butane occupy at 755 torr and 35 °C?544Has a video solution.
Textbook QuestionAt the end of 2012, global population was about 7.0 billion people. What mass of glucose in kg would be needed to provide 1500 Cal/person/day of nourishment to the global population for one year? Assume that glucose is metabolized entirely to CO21g2 and H2O1l2 according to the following thermochemical equation: C6H12O61s2 + 6 O21g2¡6 CO21g2 + 6 H2O1l2 H = -2803 kJ434Has a video solution.
Textbook QuestionThe automobile fuel called E85 consists of 85% ethanol and 15% gasoline. E85 can be used in the so-called flex-fuel vehicles (FFVs), which can use gasoline, ethanol, or a mix as fuels. Assume that gasoline consists of a mixture of octanes (different isomers of C8H18), that the average heat of combustion of C8H181l2 is 5400 kJ>mol, and that gasoline has an average density of 0.70 g>mL. The density of ethanol is 0.79 g>mL. (a) By using the information given as well as data in Appendix C, compare the energy produced by combustion of 1.0 L of gasoline and of 1.0 L of ethanol.1222Has a video solution.
Textbook QuestionA mixture of 2.0 mol of H2( g) and 1.0 mol of O2( g) is placed in a sealed evacuated container made of a perfect insulating material at 25 °C. The mixture is ignited with a spark and reacts to form liquid water. Determine the temperature of the water.638Has a video solution.
Textbook QuestionWhen 10.00 g of phosphorus is burned in O2( g) to form P4O10(s), enough heat is generated to raise the temperature of 2950 g of water from 18.0 °C to 38.0 °C. Calculate the enthalpy of formation of P4O10(s) under these conditions.13551Has a video solution.
Textbook QuestionA gaseous fuel mixture contains 25.3% methane (CH4), 38.2% ethane (C2H6), and the rest propane (C3H8) by volume. When the fuel mixture contained in a 1.55 L tank, stored at 755 mmHg and 298 K, undergoes complete combustion, how much heat is emitted? (Assume that the water produced by the combustion is in the gaseous state.)1733Has a video solution.
Textbook QuestionCytochrome, a complicated molecule that we will represent as CyFe2+, reacts with the air we breathe to supply energy required to synthesize adenosine triphosphate (ATP). The body uses ATP as an energy source to drive other reactions (Section 19.7). At pH 7.0 the following reduction potentials pertain to this oxidation of CyFe2+: O21g2 + 4 H+1aq2 + 4 e- ¡ 2 H2O1l2 Ered ° = +0.8 (b) If the synthesis of 1.00 mol of ATP from adenosine diphosphate (ADP) requires a ∆G of 37.7 kJ, how many moles of ATP are synthesized per mole of O2?252Has a video solution.
Textbook QuestionIt is estimated that the net amount of carbon dioxide fixed by photosynthesis on the landmass of Earth is 5.5 * 1016 g>yr of CO2. Assume that all this carbon is converted into glucose. (a) Calculate the energy stored by photosynthesis on land per year, in kJ.663Has a video solution.
Textbook QuestionAt 791 K and relatively low pressures, the gas-phase decomposition of acetaldehyde 1CH3CHO2 is second order in acetaldehyde. CH3CHO1g2S CH41g2 + CO1g2 The total pressure of a particular reaction mixture was found to vary as follows: (c) If the volume of the reaction mixture is 1.00 L, what is the total amount of heat liberated (in joules) after a reaction time of 605 s?132Has a video solution.Textbook QuestionConsider the reaction that occurs on mixing 50.0 mL of 0.560 M NaHCO3 and 50.0 mL of 0.400 M NaOH at 25 °C. (c) How much heat (in joules) is liberated by the reaction? (Standard heats of formation are given in Appendix B.)136Has a video solution.Textbook QuestionReaction of gaseous fluorine with compound X yields a sin- gle product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (d) How much heat in kilojoules is released or absorbed in the reaction of 25.0 g of X with a stoichiometric amount of F2, assuming 87.5% yield for the reaction?181Has a video solution.Showing 41 of 41 practiceMore practice (0)
Textbook QuestionConsider the reaction that occurs on mixing 50.0 mL of 0.560 M NaHCO3 and 50.0 mL of 0.400 M NaOH at 25 °C. (c) How much heat (in joules) is liberated by the reaction? (Standard heats of formation are given in Appendix B.)136Has a video solution.
Textbook QuestionReaction of gaseous fluorine with compound X yields a sin- gle product Y, whose mass percent composition is 61.7% F and 38.3% Cl. (d) How much heat in kilojoules is released or absorbed in the reaction of 25.0 g of X with a stoichiometric amount of F2, assuming 87.5% yield for the reaction?181Has a video solution.
