Both glucose and fructose arc simple sugars with the same molecular formula of C6H12O6. Sucrose (C121122O11), or table sugar, consists of a glucose molecule bonded to a fructose molecule (a water molecule is eliminated in the formation of sucrose), (a) Calculate the energy released when a 2.0-g glucose tablet is burned in air. (b) To what height can a 65-kg person climb after ingesting such a tablet, assuming only 30% of the energy released is available for work. (See the hint for Problem 10.127.) Repeat the calculations for a 2.0-g sucrose tablet.
(a)
Interpretation:
The energy changes in 2.0 g of Glucose and Sucrose tablet has to be calculated and the height the person can climb after ingesting the tablet has to be calculated.
Concept Introduction:
Heat is flow of thermal energy involving two bodies at various temperatures. The flow of thermal energy involving two bodies at various temperatures is called as heat. The flow of heat implies that energy is either released or absorbed on describing about energy changes that takes place during a process.
Exothermic process is the chemical process in which heat is released to the surroundings.
Endothermic process is the chemical process in which heat is absorbed from the surroundings.
The change in enthalpy that is associated with the formation of one mole of a substance from its related elements being in standard state is called standard enthalpy of formation (
The standard enthalpy of reaction is the enthalpy of reaction that takes place under standard conditions.
To calculate: The energy changes for 2 grams of Glucose and Sucrose
Answer to Problem 10.137QP
The heat change for Glucose is
The heat change for Sucrose is
Explanation of Solution
Weight of Glucose =
Molar mass of Glucose =
Heat of combustion of Glucose =
Moles of Glucose =
=
Moles of Sucrose =
Moles of Glucose =
Moles of Sucrose =
To calculate the energy changes for 2 grams of Glucose and Sucrose
Energy change in Glucose =
=
Energy change in Sucrose =
=
Energy change in Glucose =
Energy change in Sucrose =
The energy changes for 2 grams of Glucose and Sucrose were calculated using the values the moles and heat of combustions of Glucose and Sucrose. The energy changes for 2 grams of Glucose and Sucrose were found to be
(b)
Concept Introduction:
The energy possessed by an object due to its relative point to some other object, stress surrounded by itself, its electric charge or any other external factor is called as potential energy.
Potential energy can be calculated using the formula,
Answer to Problem 10.137QP
Height climbed by the person on ingesting Glucose is 15 m.
Height climbed by the person on ingesting Sucrose is 16 m.
Explanation of Solution
To calculate the heat in Joules
Heat of Sucrose = 9.9×103 J
Heat of Glucose = 9.3×103 J
To calculate the height climbed
Height climbed by the person on ingesting Glucose =15 m.
Height climbed by the person on ingesting Sucrose =16 m.
Heights climbed by the person on ingesting Glucose and Sucrose were calculated using the values of mass, acceleration due to gravity and heat. The heights climbed by the person on ingesting Glucose and Sucrose were found to be 15 m and16 m.
Want to see more full solutions like this?
Chapter 10 Solutions
Loose Leaf For Chemistry: Atoms First With Connect 2y Access Card
- How fast (in meters per second) must an iron ball with a mass of 56.6 g be traveling in order to have a kinetic energy of 15.75 J?arrow_forwardNiagara Falls has a height of 167 ft (American Falls). What is the potential energy in joules of 1.00 lb of water at the top of the falls if we take water at the bottom to have a potential energy of zero? What would be the speed of this water at the bottom of the falls if we neglect friction during the descent of the water?arrow_forwardFind the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the number of carbon atoms in the molecule, and determine an equation that gives H for the combustion of a given hydrocarbon. Then use the equation to predict the enthalpy of combustion for n-C12H26 and compare it to experimental values.arrow_forward
- How many milliliters of water at 23 C with a density of 1.00 g/mL must be mixed with 180 mL (about 6 oz) of coffee at 95 C so that the resulting combination will have a temperature of 60 C? Assume that coffee and water have the same density and the same specific heat.arrow_forwardHydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an antiseptic. H2O2 can be prepared in a process whose overall change is H2(g)+O2(g)H2O2(l) Calculate the enthalpy change using the following data: H2O2(l)H2O(l)+12O2(g);H=98.0kJ2H2(g)+O2(g)2H2O(l);H=571.6kJarrow_forwardCompounds 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=286kJarrow_forward
- 9.41 Under what conditions does the enthalpy change equal the heat of a process?arrow_forwardA sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.00 mol of ethanol at constant volume and 25.00C? The reaction is C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) Is q equal to U or H?arrow_forwardIf takes 1.25 kJ of energy to heat a certain sample of pure silver from 12.0 °C to 15.2 °C. Calculate the mass of the sample of silver.arrow_forward
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Physical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning