gas-stoichiometry

gas-stoichiometry - Gas Stoichiometry Stoichiometry Gas...

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Gas Gas Stoichiometry Stoichiometry

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Gas Stoichiometry Gas Stoichiometry We have looked at stoichiometry: 1) using We can use stoichiometry for gas reactions. As before, we need to consider mole ratios when examining reactions quantitatively. At times you will be able to use 22.4 L/mol at STP and 24.8 L/mol at SATP as shortcuts. grams (x) moles (x) moles (y) grams (y) molar mass of y mole ratio from balanced equation molar mass of x P, V, T (x) P, V, T (y) PV = nRT
Sample problem 1 Sample problem 1 CH 4 burns in O 2 , producing CO 2 and H 2 O(g). A 1.22 L CH 4 cylinder, at 15°C, registers a pressure of 328 kPa. a) What volume of O 2 at SATP will be required to react completely with all of the CH 4 ? First: CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) PV = nRT (8.31 kPa•L/K•mol)(288 K) (328 kPa)(1.22 L) = n = 0.167 mol P = 328 kPa, V = 1.22 L, T = 288 K mol O 2 = 0.167 mol CH 4 2 mol O 2 1 mol CH 4 x = 0.334 mol PV = nRT (100 kPa) (0.334 mol)(8.31 kPa•L/K•mol )(298 K) =V = 8.28 L P= 100 kPa, n= 0.334 mol, T= 298 K or # L = 0.334 mol x 24.8 L/mol = 8.28 L

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Sample problem 1 continued Sample problem 1 continued CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(g) b) How many grams of H 2 O(g) are produced? c) What volume of CO
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This note was uploaded on 11/09/2011 for the course CHEM 110 taught by Professor Sullivan during the Fall '10 term at BYU.

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gas-stoichiometry - Gas Stoichiometry Stoichiometry Gas...

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