General Chemistry: Principles and Modern Applications (10th Edition)

Published by Pearson Prentice Hal
ISBN 10: 0132064529
ISBN 13: 978-0-13206-452-1

Chapter 6 - Gases - Example 6-4 - Calculating a Gas Volume with the Ideal Gas Equation - Page 205: Practice Example B


464 K

Work Step by Step

$n=13.7 \,g\,Cl_{2}\times\frac{1\,mol\,Cl_{2}}{70.906\,g\,Cl_{2}}=0.1932\,mol$ $R=0.08314\,bar\,L\,mol^{-1}K^{-1}$ $P=0.993\,bar$ $V=7.50\,L$ From the ideal gas law, we have $ T=\frac{PV}{nR}=\frac{0.993\,bar\times7.50\,L}{0.1932\,mol\times0.08314\,bar\,L\,mol^{-1}K^{-1}}$ $=464\,K $
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