Answer
1680 K
Work Step by Step
We find:
$V=72.8\,L$
$n=7.41\,g\,He\times\frac{1\,mol\,He}{4.0026\,g\,He}=1.8513\,mol$
$P=3.50\,atm$
$T=\frac{PV}{nR}=\frac{(3.50\,atm)(72.8\,L)}{(1.8513\,mol)(0.08206\,L\,atm\,K^{-1}mol^{-1})}$
$=1680\,K$
General Chemistry: Principles and Modern Applications (10th Edition)
by Petrucci, Ralph H.; Herring, F. Geoffrey; Madura, Jeffry D.; Bissonnette, Carey
Published by
Pearson Prentice Hal
ISBN 10:
0132064529
ISBN 13:
978-0-13206-452-1
Chapter 6 - Gases - Exercises - Ideal Gas Equation - Page 232: 30
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