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

This preview shows pages 1–4. Sign up to view the full content.

HOMEWORK 1

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
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:
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:

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

{[ snackBarMessage ]}

### Page1 / 5

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

This preview shows document pages 1 - 4. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online