Chemistry: An Introduction to General, Organic, and Biological Chemistry (12th Edition)

Published by Prentice Hall
ISBN 10: 0321908449
ISBN 13: 978-0-32190-844-5

Chapter 8 - Section 8.6 - Volume and Moles (Avogadro's Law) - Questions and Problems - Page 272: 8.44a

Answer

There are 10.1 g of $Ne$ in 11.2 L of $Ne$ gas at STP.

Work Step by Step

1. Setup the conversion factors: For a gas at STP conditions, we can use the equality: $1 \space mole = 22.4 \space L$: $\frac{1 \space mole \space (Ne)}{22.4 \space L \space (Ne)}$ and $\frac{22.4 \space L \space (Ne)}{1 \space mole \space (Ne)}$ Molar mass of $Ne$: 20.18 g/mole $ \frac{1 \space mole \space (Ne)}{ 20.18 \space g \space (Ne)}$ and $ \frac{20.18 \space g \space (Ne)}{1 \space mole \space (Ne)}$ 2. Calculate the mass of $Ne$ in that sample: $11.2 \space L \space (Ne) \times \frac{1 \space mole \space (Ne)}{22.4 \space L \space (Ne)} \times \frac{20.18 \space g \space (Ne)}{1 \space mole \space (Ne)} = 10.1 \space g \space (Ne)$
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