thermochemistry help

thermochemistry help - Chapter 6 Chapter 6 1 Slide 1 The...

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Unformatted text preview: Chapter 6 Chapter 6 1 Slide 1 The heat capacity ( C ) of a substance is the amount of heat ( q ) required to raise the temperature of a given quantity ( m ) of the substance by one degree Celsius. Heat ( q ) absorbed or released: C = q / t t = t final - t initial Heat Capacity, C 90 C C 40 C C q = C t Units of C : J/8 C, J/K, cal/&C, cal/K T = T final - T initial Chapter 6 Chapter 6 2 Slide 2 The specific heat ( s ) of a substance is the amount of heat ( q ) required to raise the temperature of one gram of the substance by one degree Celsius. s = C / m Heat ( q ) absorbed or released: q = sm t t = t final - t initial Specific Heat (Capacity), s s = q / m t Units of s : J/g3 C, J/gK, etc. Chapter 6 Chapter 6 3 Slide 3 6.3 How much heat is required to raise the temperature of 1.0 x 103 kg of iron from 25 & C to 75 & C if the specific heat of iron is 0.45 J/g & C? MJ 22.5 or J 10 2.25 g J 0.45 kg 1,000g kg 10 1.0 q C g J heat specific ) ( mass(g) q(J) 7 o 3 = = = C C C t o 50 ) ( ) ( heat specific gK t m J q = Sample Problem Chapter 6 Chapter 6 4 Slide 4 6.4 A 237 g piece of molybdenum, initially at 100.0 oC, is dropped into 244 g of water at 10.0 oC. When the system comes to thermal equilibrium, the temperature of the system is 15.3 oC. What is the specific heat of the metal? gK J C g J C g C g C g J g C g J s C g T heat o 27 27 7 84 237 3 5 244 184 4 100 3 15 237 244 . . . . . s C ) . . ( 10.0)- (15.3 C g J 4.184 q mass capacity heat specific q metal by lost heat by water gained = = = - - = = =- = Sample Problem Chapter 6 Chapter 6 5 Slide 5 6.5 If 25.0 g Fe at 95.00 &C were added to a coffee cup calorimeter containing 75.0 g H2O at 28.00 C, what would be the final temperature of the contents of the calorimeter when equilibrium is established?...
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thermochemistry help - Chapter 6 Chapter 6 1 Slide 1 The...

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