Image by: Jenene from Chinatown, New York City, USA [CC BY 2.0]The process of flambéing involves pouring liqueur on food for flavor. This addition to desserts adds tons of flavor, but is there a way to explain it scientifically? Liqueur et eel(C₂H5OH), which combusts in the presence of immense heat. You maymaye noticed this in restaurants, when very large flames rise from pans on stoves. Use the legancedchemical equation for the combustion of ethanol as a reference in this asseC₂H₂OH (1)+30₂ (g) 2 CO₂ (g) + 3 H₂0 (g) potential energyEthanolOxygenCarbon dioxide.steamUse the graph above to explain if the combustion of ethanol is exothermic or endothermic.

The change of energy of reaction occurs at constant pressure is called enthalpy of reaction.

Answered: potential energy Ethanol Oxygen Carbon…

potential energy Ethanol Oxygen Carbon dioxide .steam Use the graph above to explain if the combustion of ethanol is exothermic or endothermic.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter4: Energy And Chemical Reactions

Section: Chapter Questions

Problem 89QRT

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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.
General Zod has sold Lex Luthor what Zod claims to be a new copper-colored form of kryptonite, the only substance that can harm Superman. Lex, not believing in honor among thieves, decided to carry out some tests on the supposed kryptonite. From previous tests, Lex knew that kryptonite is a metal having a specific heat capacity of 0.082 J/gC and a density of 9.2 g/cm3. Lex Luthers first experiment was an attempt to find the specific heat capacity of kryptonite. He dropped a 10 g 3 g sample of the metal into a boiling water bath at a temperature of 100.0C 0.2C. He waited until the metal had reached the bath temperature and then quickly transferred it to I 00 g 3 g of water that was contained in a calorimeter at an initial temperature of 25.0C 0.2C. The final temperature of the metal and water was 25.2C. Based on these results, is it possible to distinguish between copper and kryptonite? Explain. When Lex found that his results from the first experiment were inconclusive, he decided to determine the density of the sample. He managed to steal a better balance and determined the mass of another portion of the purported kryptonite to be 4 g 1 g. He dropped this sample into water contained in a 25-mL graduated cylinder and found that it displaced a volume of 0.42 mL 0.02 mL. Is the metal copper or kryptonite? Explain. Lex was finally forced to determine the crystal structure of the metal General Zod had given him. He found that the cubic unit cell contained four atoms and had an edge length of 600. pm. Explain how this information enabled Lex to identify the metal as copper or kryptonite. Will Lex be going after Superman with the kryptonite or seeking revenge on General Zod? What improvements could he have made in his experimental techniques to avoid performing the crystal structure determination?
Compounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called hydrogenation. C2H4(g)+H2(g)C2H6(g) Calculate the enthalpy change for this reaction, using the following combustion data: C2H4(g)+3O2(g)2CO2(g)+2H2O(l);H=1411kJC2H6(g)+72O2(g)2CO2(g)+3H2O(l);H=1560kJH2(g)+12O2(g)H2O(l);H=286kJ
Salicylic acid, C7H6O3, is one of the starting materials in the manufacture of aspirin. When 1.00 g of salicylic acid burns in a bomb calorimeter, the temperature of the bomb and water goes from 23.11C to 28.91C. The calorimeter and water absorb 21.9 kJ of heat. How much heat is given off when one mole of salicylic acid burns?
Would the amount of heat measured for the reaction in Example 5.5 be greater, lesser, or remain the same if we used a calorimeter that was a poorer insulator than a coffee cup calorimeter? Explain your answer.
1. Which of the following processes is endothermic? melting of ice at 0 °C the reaction of methane and O2 condensation of water vapor at 100 °C cooling liquid water from 25 °C to 0 °C
Which of the enthalpies of combustion in Table 5.2 the table are also standard enthalpies of formation?
9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?
Explain how the heat measured in Example 5.5 differs from the enthalpy change for the exothermic reaction described by the following equation: HCl(aq)+NaCl(aq)H2O(l)