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Fundamentals of General, Organic, and Biological Chemistry (Mastering Chemistry) | 8th Edition | ISBN: 9780134015187 | Authors: John McMurry, David Ballantine, Carl Hoeger, Virginia Peterson ISBN: 9780134015187 2044

Solution for problem 7.3 Chapter 7.3

Fundamentals of General, Organic, and Biological Chemistry (Mastering Chemistry) | 8th Edition

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Fundamentals of General, Organic, and Biological Chemistry (Mastering Chemistry) | 8th Edition | ISBN: 9780134015187 | Authors: John McMurry, David Ballantine, Carl Hoeger, Virginia Peterson

Fundamentals of General, Organic, and Biological Chemistry (Mastering Chemistry) | 8th Edition

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Problem 7.3

In photosynthesis, green plants convert carbon dioxide and water into glucose \(\left(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\right)\) according to the following equation:

                                  \(6 \mathrm{CO}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(a q)+6 \mathrm{O}_{2}(g)\)

(a) Estimate \(\Delta H\) for the reaction using bond dissociation energies from Table 7.1. Give your answer in kJ/mol. (\(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\). has \(\mathrm{C}-\mathrm{C}\) bonds, seven \(\mathrm{C}-\mathrm{H}\) bonds, seven \(\mathrm{C}-\mathrm{O}\) bonds, and five \(\mathrm{O}-\mathrm{H}\) bonds).

(b) Is the reaction endothermic or exothermic?

Text Transcription:

C_8/H_12/O_6

6 CO_2 (g)+6 H_2 O (l) longrightarrow C_6 H_12 O_6 (a q)+6 O_2 (g)

C_6H_12O_6

C-C

C-H

C-O

O-H

Step-by-Step Solution:
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Friday, September 16, 2016 Week 3 Notes CHE 152 - Ions and the periodic table for main group elements: • - metals lose electrons (until they have the same number of electrons as the nearest noble gas) and become cations - nonmetals tend to gain electrons (until they have the same number of electrons as the nearest noble gas) and become anions • an atomic mass unit (amu) is exactly 1/12 the mass of a carbon-12 isotope • isotopic mass: the mass of a given isotope - the mass number =/= the mass on the periodic table (atomic mass) this is because the atomic mass is the weighted average of the isotopes of a • given element. found by taking the sum of isotopic masses multiplies by their abundance fraction • molar mass: the atomic mass expressed in grams - Avogadro’s number and the mole • Avogadro’s number is 6.022 x 10 23 • the mole is a unit for expressing the number of expressing the number of atoms, ions, molecules, etc. in a “common-size” unit • a mole is the amount of anything that contains Avogadro’s number of units - mole = (number of things) / (6.022 x 10 )23 • the relationship between mass and moles - mole = (mass of the substance) / (molar mass) • compounds have different properties than reactants - there are 119 million known compounds • there are microscale and macroscale equations 1 Frid

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Chapter 7.3, Problem 7.3 is Solved
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Textbook: Fundamentals of General, Organic, and Biological Chemistry (Mastering Chemistry)
Edition: 8
Author: John McMurry, David Ballantine, Carl Hoeger, Virginia Peterson
ISBN: 9780134015187

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