College Physics (4th Edition)

Published by McGraw-Hill Education
ISBN 10: 0073512141
ISBN 13: 978-0-07351-214-3

Chapter 14 - Problems - Page 534: 26


$56,900~J$ of heat are required.

Work Step by Step

We can find the number of moles of hydrogen: $PV = nRT$ $n = \frac{PV}{RT}$ $n = \frac{(10.0)(1.013\times 10^5~Pa)(250\times 10^{-3}~m^3)}{(8.314~J/mol~K)(273.15~K)}$ $n = 111.5~mol$ We can find the required heat: $Q = c~n~\Delta T$ $Q = (20.4~J/mol~K)(111.5~mol)(25.0~K)$ $Q = 56,900~J$ $56,900~J$ of heat are required.
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