c161l13_10_02

c161l13_10_02 - Other calculations Other Change in volume...

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Other calculations Other calculations W Change in volume due to a reaction W So much expansion that we can ignore the volume of solids and liquids Find the total number of moles produced V = nRT/P
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Example Example W How much room is occupied by the gases produced from exploding 2.5 mL of nitroglycerin at 25 °C and 1 atm final pressure? The density of nitroglycerin is 1.59 g/mL W Step 1: Balanced reaction 4C 3 H 5 (NO 3 ) 3 (l) 6N 2 (g) + O 2 (g) + 12CO 2 (g) + 10H 2 O(g) W Step 2: Find the number of moles of nitroglycerin. 2.5mL×1.59g/mL/227.1g/mol=0.035mol W Step 3: Find moles of gas produced 4 mol nitroglycerin = 29 mol of products 0.035 mol nitroglycerin = 0.254 mol products
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W Step 4: Find the volume occupied from ideal gas law V = nRT/P V = 0.254mol×0.08206 L atm mol -1 K -1 × 298.15K/1 atm 6.22L
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Gas Density Gas Density W The density of an ideal gas depends on temperature, pressure and the molar mass of the gas W d=PM/(RT) W This can be used to find the molar mass of a compound.
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This note was uploaded on 11/12/2011 for the course CHEM 160:161 taught by Professor Siegel during the Fall '09 term at Rutgers.

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c161l13_10_02 - Other calculations Other Change in volume...

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