Domanda del libro di testo
(a) A serving of a particular ready-to-serve brown & wild rice meal contains 4.5 g fat, 42 g carbohydrate, and 4.0 g protein. Estimate the number of calories in a serving.
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Ch.5 - Thermochemistry
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 5, Problema 94
The heat of combustion of ethanol, C2H5OH(l), is -1367 kJ/mol. A bottle of stout (dark beer) contains up to 6.0% ethanol by mass. Assuming the density of the beer to be 1.0 g/mL, what is the caloric content due to the alcohol (ethanol) in a bottle of beer (500 mL)?
Guida verificata passo dopo passo1
Calculate the mass of the beer using its volume and density: \( \text{mass} = \text{volume} \times \text{density} \).
Determine the mass of ethanol in the beer using the percentage by mass: \( \text{mass of ethanol} = \text{mass of beer} \times \frac{6.0}{100} \).
Convert the mass of ethanol to moles using the molar mass of ethanol (C\(_2\)H\(_5\)OH), which is approximately 46.08 g/mol: \( \text{moles of ethanol} = \frac{\text{mass of ethanol}}{46.08} \).
Calculate the total heat of combustion for the ethanol in the beer using the heat of combustion per mole: \( \text{total heat} = \text{moles of ethanol} \times (-1367 \text{ kJ/mol}) \).
Convert the total heat from kJ to calories, knowing that 1 kJ = 239.006 calories.
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Heat of Combustion
The heat of combustion is the amount of energy released when a substance undergoes complete combustion with oxygen. For ethanol, the heat of combustion is -1367 kJ/mol, indicating that this amount of energy is released per mole of ethanol burned. This concept is crucial for calculating the energy content of ethanol in the beer.
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Percorso guidato
02:24
Combustion Apparatus
Mass Percent Concentration
Mass percent concentration is a way to express the concentration of a component in a mixture, calculated as the mass of the component divided by the total mass of the mixture, multiplied by 100. In this case, the beer contains 6.0% ethanol by mass, which means that in 100 g of beer, there are 6 g of ethanol. This concept is essential for determining the total mass of ethanol in the 500 mL of beer.
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Percorso guidato
00:38Mass Percent Calculation
Density and Volume Relationship
Density is defined as mass per unit volume, and it allows us to convert between the volume of a liquid and its mass. Given that the density of the beer is 1.0 g/mL, a 500 mL bottle of beer has a mass of 500 g. Understanding this relationship is vital for calculating the total mass of ethanol present in the beer based on its volume.
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Percorso guidato
01:09Relationship of Volume and Moles Example
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Domanda del libro di testo
The standard enthalpies of formation of gaseous propyne (C3H4), propylene (C3H6), and propane (C3H8) are +185.4, +20.4, and -103.8 kJ/mol, respectively. (c) Which is the most efficient fuel in terms of heat evolved per unit mass?
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Domanda del libro di testo
It is interesting to compare the 'fuel value' of a hydrocarbon in a hypothetical world where oxygen is not the combustion agent. The enthalpy of formation of CF4(g) is -679.9 kJ/mol. Which of the following two reactions is the more exothermic?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
CH4(g) + 4 F2(g) → CF4(g) + 4 HF(g)
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Domanda del libro di testo
The heat of combustion of fructose, C6H12O6, is -2812 kJ/mol. If a fresh golden delicious apple weighing 120 g contains 16.0 g of fructose, what caloric content does the fructose contribute to the apple?
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Domanda del libro di testo
The standard enthalpies of formation of gaseous propyne (C3H4), propylene (C3H6), and propane (C3H8) are +185.4, +20.4, and -103.8 kJ/mol, respectively. (a) Calculate the heat evolved per mole on combustion of each substance to yield CO2(g) and H2O(g). (b) Calculate the heat evolved on combustion of 1 kg of each substance.
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