Calculate the standard enthalpy difference between 2-ethyl-1-butene and 1-hexene to determinewhich molecule is more stable. The heats of formation are -55.8 kJ/mol for 2-ethyl-1-butene and-40.5 kJ/mol for 1-hexene.O a. 2-ethyl-1-butene is more stable by 15.3 kJ/molO b. The two stabilities can't be compared because the molecules are not isomers.O c. 1-Hexene is more stable by 15.3 kJ/mol

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Answered: Calculate the standard enthalpy…

EBK A SMALL SCALE APPROACH TO ORGANIC L

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ISBN:9781305446021

Author:Lampman

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Chapter26: Biodiesel

Section: Chapter Questions

Problem 2Q

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Camping stoves are fueled by propane (C3H8), butane [C4H10(g), fH = 127.1 kJ/mol]. gasoline. or ethanol (C2H5OH). Calculate the enthalpy of combustion per gram of each of these fuels. [Assume that gasoline is represented by isooctane, C8H18(), with fH = 259.3 kJ/mol.) Do you notice any great differences among these fuels? How are these differences related to their composition?
The enthalpy change when 1 mol methane (CH4) is burned is 890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
Quinone is an important type of molecule that is involved in photosynthesis. The transport of electrons mediated by quinone in certain enzymes allows plants to take water, carbon dioxide, and the energy of sunlight to create glucose. A 0.1964-g sample of quinone (C6H4O2) is burned in a bomb calorimeter with a heat capacity of 1.56 kJ/C. The temperature of the calorimeter increases by 3.2C. Calculate the energy of combustion of quinone per gram and per mole.
Isomers are molecules with the same elemental composition but a different atomic arrangement. Three isomers with the formula C4H8 are shown in the models below. The enthalpy of combustion (cH) of each isomer, determined using a calorimeter, is as follows: (a) Draw an energy level diagram relating the energy content of the three isomers to the energy content of the combustion products, CO2(g) and H2O(). (b) Use the cH data in part (a), along with the enthalpies of formation of CO2(g) and H2O() from Appendix L, to calculate the enthalpy of formation for each of the isomers. (c) Draw an energy level diagram that relates the enthalpies of formation of the three isomers to the energy of the elements in their standard states. (d) What is the enthalpy change for the conversion of cis-2-butene to trans-2-butene?
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). The temperature increases by 10.9 C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g. (a) Calculate the enthalpy change for the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.
A compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When 1.000 g of this compound burns in excess oxygen, the enthalpy change is 49.53 kJ. (a) What is the empirical formula of this compound? (b) What is the molecular formula of this compound? (c) What is the standard enthalpy of formation of this compound? (d) Two compounds that have this molecular formula appear in Appendix G. Which one was used in this exercise?
Chloroform, CHCl3, is formed from methane and chlorine in the following reaction. CH4(g) + 3 Cl2(g) 3 HCl(g) + CHCl3(g) Calculate rH, the enthalpy change for this reaction, using the enthalpies of formation of CO2(g), H2O(), CHCI3(g) (fH = 103.1 kJ/mol), and the enthalpy changes for the following reactions: CH4(g) + 2 O2(g) 2 H2O() + CO2(g) rH = 890.4 kJ/mol-rxn 2 HCl(g) H2(g) + Cl2(g) rH = +184.6 kJ/mol-rans
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)
Methane, CH4, can be converted to methanol, which, like ethanol, can be used as a fuel. The energy level diagram shown here presents relationships between energies of the fuels and their oxidation products. Use the information in the diagram to answer the following questions. (The energy terms are per mol-rxn.) (a) Which fuel, methanol or methane, yields the most energy per mole when burned? (b) Which fuel yields the most energy per gram when burned? (c) What is the enthalpy change for the conversion of methane to methanol by reaction with O2(g)? (d) Each arrow on the diagram represents a chemical reaction. Write the equation for the reaction that converts methane to methanol.
The enthalpy changes for the following reactions can be measured: CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) rH = 802.4 kJ/mol-rxn CH3OH(g) + 32 O2(g) CO2(g) + 2 H2O(g) rH = 676 kJ/mol-rxn (a) Use these values and Hesss law to determine the enthalpy change for the reaction CH4(g) + O2(g) CH3OH(g) (b) Draw an energy level diagram that shows the relationship between the energy quantities involved in this problem.
Isooctane (2,2,4-trimethylpentane), one of the many hydro carbons that make up gasoline, burns in air to give water and carbon dioxide. 2C8H18(l)+25O2(g)16CO2(g)+18H2O(l)rH=10,922kJ/mol Calculate the enthalpy change if you burn 1.00 L isooctane (density = 0.69 g/mL).
Fructose is a sugar commonly found in fruit. A sample of fructose, C6H12O6, weighing 4.50 g is burned in a bomb calorimeter that contains 1.00 L of water (d=1.00g/mL). The heat capacity of the calorimeter is 16.97 kJ/PC. The temperature of the calorimeter and water rise from 23.49C to 27.72C. (a) What is q for the calorimeter? (b) What is q for water in the calorimeter? (c) What is q when 4.50 g of fructose are burned in the calorimeter? (d) What is q for the combustion of one mole of fructose?

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