HW1soln - HOMEWORK 1 1.15 Normally, the gas constant R is...

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HOMEWORK 1
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1.15 Normally, the gas constant R is 8.314 in the units we've used so far with the eq; PV=nRT If we want to keep P,V, and n the same and just change the T such that R can be 1.00, then the equation above can be changed to PV = nGT' where T' = 8.314*T 1.20 Find the partial pressures of He and of N2 at sea level: P0(He) = 5.24E-6 * 101250 Pa = 0.53 Pa P0(N2) = 0.7808 * 101250 Pa = 79056 Pa Find the partial pressures of He and of N2 at 10 km using the formula provided: P10(i) = P0(i) * exp(-Mgz/RT); use this formula for calculating the total pressure as well. M(He) = 4.00 g/mol; M(N2) = 28.04 g/mol z = 10000 m; T = 300 K; R = 8.314 L Pa K-1 mol-1; g = 9.8 ms-2 Make sure your units cancel properly and plug-and-chug:
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1.24 Find the number of Ar atoms per cubic meter of atmosphere at the surface pressure (P0(ar)): P0(Ar) = 0.01 * 101250 Pa = 1012.5 Pa #A0(Ar) = N*P0(Ar) / RT = 6.023E-23 * 1012.5 Pa / 8.314 * 300 K = 2.41E23 atoms m-3 The total number of Ar atoms in the atmosphere is:
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HW1soln - HOMEWORK 1 1.15 Normally, the gas constant R is...

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