ch9_ex - Example 1 One mol of H2O(g) at 1.00 atm and 100 C...

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1.00 atm 30.6 L 100. °C 1.00 atm 40.66 kJ Example 1 One mol of H 2 O(g) at 1.00 atm and 100 °C occupies a volume of 30.6 L. When one mol of H 2 O(g) is condensed to a mol of H 2 O(l) at 1.00 atm and 100 °C, 40.66 kJ of heat is released. If the density of H 2 O(l) is 0.996 g/mL, then calculate E, H, w and q.
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Example 1 kJ q H 66 . 40 - = = ( 29 ( 29 ( 29 kJ w K K mol J mol nRT w 10 . 3 373 / 31 . 8 00 . 1 = - - - = - = kJ kJ kJ w q E 56 . 37 10 . 3 66 . 40 - = + - = + = ( 29 kJ . w atm L J L mL L mL g g atm . w V P w 10 3 08206 . 0 31 . 8 6 . 30 1000 1 / 996 . 0 02 . 18 00 1 = - - - = - = or
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2.4 mol gas 4.00 L 32 °C Vacuum 4.00 L Example 2 2.4 mol of an ideal gas is contained in a 4.0 L flask at 32 °C. This flask is connected to another 4.0 L flask, initially evacuated, via a valve. When the valve is opened the temperature remains constant.
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Example 3 Reaction Enthalpy
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This note was uploaded on 05/11/2008 for the course CHEM 025 taught by Professor Axe during the Spring '08 term at Pacific.

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ch9_ex - Example 1 One mol of H2O(g) at 1.00 atm and 100 C...

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