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Lecture 12 (10am) Chapter 6 and Chapter 7 October 9, 2009

# Lecture 12 (10am) Chapter 6 and Chapter 7 October 9, 2009 -...

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Chapter 6 continued Lecture 12 October 9, 2009

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Key Points in Calorimetry
A common laboratory reaction is the neutralization of an acid with a base. When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of 0.500 M NaOH at 25.0°C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of acid? Assume the mixture has a specific heat capacity of 4.18 J/(g·K) and that the densities of the reactant solutions are both 1.00 g/mL. A. > 100 kJ B. 54 kJ C. 27 kJ D. 1300 J E. 670 J

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Standard Heats of Reaction We must take into account the fact that thermodynamic variables, such as enthalpy, can vary somewhat with conditions (changes in temperature, pressure, etc.) We establish “Standard States” for substances – a set of specified conditions and concentrations 1.Gases: Standard State is 1atm 2.Substance in Aqueous Solution: Standard State is 1M concentration 3.Pure substances (either element or compound): Standard State is the most stable form of that substance at 1atm and temperature of interest (typically 298K)

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o f of zero. 2. Most compounds have a negative ∆H
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Lecture 12 (10am) Chapter 6 and Chapter 7 October 9, 2009 -...

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