Midterm2-2005-Solutions

# Midterm2-2005-Solutions - 5 OLC-AT/ CJ/US Midterm #2 /...

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Unformatted text preview: 5 OLC-AT/ CJ/US Midterm #2 / Chemistry 4521 / Physical Chemistry for Engineers Helpful Information: PV=nRT 760 Torr = 1 atm R = 0.08206 atm dm3Klmorl T(K) = T(OC)+ 273.15 1.0 A= 1.0 X 10-10m = 1.0 x 1O~8cm 1 amu = 1.66 x 10-27kg 1 amu x Avogadro's Number = Mass of mole in grams Avogadro's Number = 6.022 x 1023morl dm3 = 1000 cm3 = 1 L dA/dt = -kA n First Order Reactions A(t) = A(O)exp( -kt) tl/2 = In2/k Second Order Reactions l/A(t) - l/A(O) = kt t1l2 = l/[A(O)k] Steady State Approximation, d[I]/dt = a2 + b2 = C2 nA = 2d sine Cubic Lattice: dhkl = a/(h2+ k2 + e)l/2 1. The fIrst-order decomposition of nitramide (NH2N02) in aqueous solution proceeds according to: NH2N02 ~ N2O(g) + H2O(l) This decomposition reaction can be analyzed by collecting the N2O gas evolved during the reaction. You are given that 5.00 x 10-2g of nitramide was allowed to decompose at 15c. The volume of N2O gas evolved after 70.0 min was measured to be 6.59 cm3at 1 atm pressure. Based on this information, find the rate constant and the half-life for nitramide decomposition. The molar mass of nitramide is 62.0 g/mol....
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## This note was uploaded on 02/26/2008 for the course CHEM 4521 taught by Professor Bierbaum during the Spring '03 term at Colorado.

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Midterm2-2005-Solutions - 5 OLC-AT/ CJ/US Midterm #2 /...

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