171020 chapter 5.pdf - Sucrose(C12H22O11 is oxidized in the...

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Sucrose (C 12 H 22 O 11 ) is oxidized in the body by O 2 via a complex set of reactions that ultimately produce CO 2 ( g ), H 2 O( g ) and 5.64x10 3 kJ/mol of heat. __C 12 H 22 O 11 ( s ) + __O 2 (g) ! __CO 2 ( g ) + __H 2 O(g) A. Heat is released; - Δ H B. Heat is released; + Δ H C. Heat is absorbed; - Δ H D. Heat is absorbed; + Δ H
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How much heat is released per gram of sucrose oxidized? (MM sucrose = 342.30 g/mol) 2 C 12 H 22 O 11 ( s ) + 35 O 2 (g) ! 24 CO 2 ( g ) + 22 H 2 O(g) + heat Δ H rxn = -5.64x10 3 kJ per mol sucrose A. -16.5 kJ B. +16.5 kJ C. -19.3x10 6 kJ D. +19.3x10 6 kJ
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Chapter 5: Thermochemistry Learning Objectives: 5G. Relate the amount of heat associated with a change in temperature using a specific heat or a specific heat capacity 5H. Use a thermochemical cycle, Hess' Law, to calculate H rxn 5I. Use enthalpies of formation ( H f ) from to calculate H rxn 5J. Determine H rxn using the appropriate method (Hess’s Law, H f , or calorimetry); choose the appropriate method to determine H rxn based on the information given
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In the laboratory a student heats 20.0g of pure copper from room temperature (22.1 °C) to 100.0 °C. How much heat is required to increase the temperature? c Cu = 0.385 J/g " ° C A. -600 J B. +600 J C. -600 kJ D. +600 kJ
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5.4c.-LO.5G. Calorimetry Enthalpy can be determined in different ways: 1. Experimentally using a calorimeter 2. Calculated using Hess’s law 3. Calculated with heats of formation, H f ° Constant-pressure calorimetry Constant-volume calorimetry (not covered!)
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5.4c.-LO.6G. Calculating amount of heat (q) PROBLEM: A 15.0 g piece of unknown metal was heated to 100.0 °C was
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