Lecture 4 - Monday: Finishing through 9.6, Starting Chapter...

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1 Monday: Finishing through 9.6, Starting Chapter 6. PS1 due today at 2:00PM NOTE: PS2 Prob 2 : NO (g) + NO 2 (g) + O 2 (g) N 2 O 5 (g) Δ H o = -112.5 kJ Practice Problems: Ch 9- 19, 33, 35, 37, 43, 51, 57, 63, 83
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2 Open Container P const, Δ V 0 Δ E = q V q P E i E f E i E f E= q P + w = q P -P Δ V Closed Container Δ V= 0, w = 0 q p = E+ Δ V Δ
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3 Standard States and Standard Enthalpy Changes Standard State: P = 1 bar (10 5 Pa) Note that 1 atm. = 1.01325 bar T = 298.15K (25 o C), unless stated otherwise. The following are in their standard states: H 2 O (l), Hg (l), CO 2 (g), P(white), Fe(s), C(s,graphite) The standard enthalpy of reaction ( Δ H o ) is the enthalpy change when reactants and products are in their standard states, unless otherwise noted.
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4 Hess’s Law If a process occurs in steps, the enthalpy change for the overall process is the sum of the enthalpy changes for the individual steps: Suppose we want to know the standard enthalpy of combustion of carbon to form carbon monoxide: C (s) + ½O 2 (g) CO(g) Δ H o = ? Unfortunately, if we burn C (s), we will only form CO
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Lecture 4 - Monday: Finishing through 9.6, Starting Chapter...

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