Thermodynamics: An Engineering Approach 8th Edition

Published by McGraw-Hill Education
ISBN 10: 0-07339-817-9
ISBN 13: 978-0-07339-817-4

Chapter 1 - Introduction and Basic Concepts - Problems - Page 44: 1-59

Answer

$h=230.51m$

Work Step by Step

First we calculated the atmospheric pressures: $P_{top}=\rho_{Hg}*g*h_{top,Hg}=(13600\frac{kg}{m^3})*(9.81\frac{m}{s^2})*(0.675m)=90055.8Pa$ $P_{bottom}=\rho_{Hg}*g*h_{bottom,Hg}=(13600\frac{kg}{m^3})*(9.81\frac{m}{s^2})*(0.695m)=92724.12Pa$ Then the difference of atmospheric pressures is: $\Delta P=92724.12Pa-90055.8Pa=2668.32Pa$ Knowing that: $P=\rho*g*h$ $h=\frac{P}{\rho*g}=\frac{2668.32kPa}{1.18\frac{kg}{m^3}*9.81\frac{m}{s^2}}=230.51m$
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